Final Review Practice Questions

Place 7 electrons in the 5d orbitals and give the four quantum numbers

(5, 2, 1, -1/2)

There are _____ (how many) elements in the periodic table. A horizontal row in the periodic table is called a _________. A vertical column in a periodic table is called a _________. The majority of elements in the periodic table are ________ (metal, nonmetal, or metalloid?)

- 118 - period - group - metal

Determine how many sig figs are recorded in each measured value - 260 - 98.0 - 40.10 - 306 - 0.3850 - 0.053

- 2 - 3 - 4 - 3 - 4 - 2

How many sig figs are in each of the following numbers? - 0.102 - 0.0012 - 12000 - 1.200 * 10^2

- 3 - 2 - 2 - 4

What is an electrolyte vs a nonelectrolyte? And what makes an electrolyte strong or weak?

- An electrolyte is a compound that dissociates in an aqueous solution (usually ionic compounds) - A nonelectrolyte is a compound that doesn't dissociate at all in an aqueous solution (usually molecular compounds) - An electrolyte that completely dissociates is a strong electrolyte and a weak one only partially dissociates

Write the element symbol that corresponds to the given element name - boron - bromine - calcium

- B - Br - Ca

Determine which ions are present in each of the compounds. - Cr2O3 - PbCl4 - Na3PO4 - Al(ClO4)3 - SrSO4

- Cr3+ & O2- - Cl- & Pb4+ - PO4 (3-) & Na+ - ClO4 (-) & Al 3+ - Sr 2+ & SO4 (2-)

Identify the oxidizing and reducing agents: - C2H4 + H2 ---> C2H6 - Fe2O3 + CO ---> 2FeO + CO2 - 2KI + Cl2 ---> KCl + I2

- Ox = C2H4, Red = H2 - Ox = Fe2O3, Red = CO - Ox = Cl2, Red = KI

List the polyatomic ions with a -3 charge and the one with a +1 charge

- PO3 - Phosphite - PO4 - Phosphate - NH4 - Ammonium (+1)

Precision means that _______ measurements are close to _______ Accuracy means that _______ measurements are close to _______

- Several, each other - Individual, an accepted value

Identify the reaction type for each of the following equations. - 2 H2(g) + O2(g) → 2 H2O(l) - MgI2(aq) + 2 AgNO3(aq) → 2 AgI(s) + Mg(NO3)2(aq) - CaCO3(s) → CaO(s) + CO2(g) - 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(l)

- Synthesis - Double-Replacement - Decomposition - Combustion

Which of the following statements about the element cesium (element #55) is TRUE? - cesium is an alkali metal. - cesium is a main group element. - cesium forms monoatomic ion with a -1 charge.

- True - True - False?

Calculate the change in the internal energy of a system when it releases 140 J of heat to the surroundings and does 85 J of work to the surroundings at the same time.

-225 J

Burning 1.00 mol of CH4 in a calorimeter warms 10.0 kg of water by 21.3°C. Calculate the heat produced in this combustion process: CH4(g)+2 O2(g)→CO2(g)+2 H2O(l)

-891 kJ (system lost 891 kJ)

A candle is lit and held under a tin can. Classify the following observations as either physical or chemical change. - Black smoke (soot) forms - Soot deposits at the bottom of the tin can - The tin can gets warm

-Chemical Change - Physical Change - Physical Change

How many moles of NaOH are present in 12.5 mL of 0.140 M NaOH?

0.00175 moles

Convert 755 mm to inches. (exactly 2.54 cm to 1 in)

29.7 in

How many subshells are in the n=3 shell?

3

What is the frequency of the light emitted from a 650. nm laser pointer? The speed of light is 3.00 x 10^8 m/s.

4.62 * 10^14 Hz

Convert the masses from grams to the indicated derived units. 0.475 g --> mg 483 g --> Mg 36.5 g --> kg

475 mg 4.83 * 10^-4 Mg 0.0365 kg

Calculate the volume of 7.11 g of nitrogen gas at 16 ºC and 799 torr.

5.74 L

Calculate the frequency of light that has a wavelength of 511 nm.

5.87 * 10^14 Hz

What is the volume (in mL) of 0.175 M AgNO3 solution needed to completely react with 25.3 mL of 0.125 M Na3PO3 solution? 3 AgNO3 (aq) + Na3PO3 (aq) ---> 3 NaNO3 (aq) + Ag3PO4 (s)

54.2 mL

K2CO3 is a common fertilizer used to supply K to plants. What is the mass% of K in K2CO3?

56.6%

How many orbitals are in the n = 3 shell?

9

The average diameter of human hair is 0.099 mm. What is the average diameter in "nm?"

9.9 *10^4 nm

Of these gases, which has the fastest-moving molecules (on average) at a given temperature? a) SO2 b) NO c) HCl d) They all have the same average speed

B

How many grams of copper are in 20.0 g of anhydrous copper sulfate?

CuSO4 7.96 g Cu

Describe the difference between intensive and extensive properties.

Extensive depends on the amount of the substance while intensive does not

Which of the following is a possible set of quantum numbers (n, l, ml) for an atomic orbital in the 4 dsubshell? I. (4, 2, 0) II. (4, 2, -1) III. (4, 3, +1)

I & II

Which of the following is a mixture? I. Beer II. Ethanol (C2H5OH) III. Nitrogen Gas IV. Seawater

I & IV

What did the discovery of neutrons do for the atomic model?

James Chadwick observed neutral particles and understood that they help account for additional mass of elements in nucleus

Complete the equation for the dissociation of K3PO4(aq)

K3PO4(aq) --> 3K+ + (PO4)3-

Calculate the percent composition of magnesium chlorite, MgCl2

Mg 25.52% Cl 74.47%

Determine the empirical formula of manganese(II) pyrophosphate, a compound containing 38.71% Mn, 21.82% P, and 39.46% O

Mn2P2O7

The density of a noble gas is 2.71 g/L at 3.00 atm and 0ºC. Identify the gas

Ne

Write balanced chemical equations for the following single-replacement reactions. - Ni(s) + Pb(ClO4)2(aq) --> - Zn(Cl2)(aq) + Mg(s) --> - Au(NO3)3(aq) + Ag(s) -->

Neutral metal is more reactive than ion so all reactions occur - Ni(s) + Pb(ClO4)2(aq) --> Pb(s) + Ni(ClO4)2(aq) - ZnCl2(aq) + Mg(s) --> Zn(s) + MgCl2(aq) - Au(NO3)3(aq) + 3 Ag(s) --> Au(s) + 3 AgNO3(aq)

A student needs to prepare 50.0 mL of 1.10 M aqueous H2O2 solution from 5.0 M H2O2 stock solution. Set up an equation to solve for the volume of stock solution needed.

V1 = (1.10M * 50.0 mL)/5.0 M

What is the charge on each cation in the following compounds? a) Cu2O b) CuO

a) +1 b) +2

A student adds 25 mL of a strong acid to 25 mL of a strong base inside a coffee cup calorimeter and immediately places the lid on top. The solution temperature rises from 20.5°C to 25.0°C. The specific heat of water is 4.184 J/g · °C and the density of water is 1.00 g/mL in this temperature range. Assume that the density of the acid and base solutions are also 1.00 g/mL. a) Calculate the enthalpy change of this reaction. b) Assuming that the strong acid has a concentration of 1.5 M, calculate the enthalpy change per mole of acid.

a) -940 J b) -25 kJ/mol

If a desperate prospector finds a nugget of fool's gold containing 0.25 mol of FeS2, (a) how many iron and sulfur atoms are in the nugget, and (b) if the nugget consists entirely of FeS2, how many atoms make up the nugget?

a) 1.5 * 10^23 Fe atoms & 3.0 * 10^23 S atoms b) 4.5 * 10^23 atoms total

How many protons, neutrons, and electrons are in a neutral atom each of the following isotopes? a) S-32 b) 19F c) A neon atom with equal numbers of protons and neutrons in its nucleus d) (238/92)U

a) 16, 16, 16 b) 9, 10, 9 c) 10, 10, 10 d) 92, 146, 92

How many atoms of each element are present in one formula unit of each of the following substances? a) Hg2CL2 b) NH4H2PO4

a) 2 Hg, 2 Cl b) 1 N, 6 H, 1 P, 4 O

Perform the following calculations and limit the answers to the correct number of sig figs a) 1.27 cm * 6.220 cm * 4.10 cm b) 9.030 g / (3.01 cm * 1.414 cm * 7.500 cm) c) (0.71 cm) ^3

a) 32.4 cm^3 b) 0.283 g/cm^3 c) 0.36 cm^3

Determine the chemical formulas for binary ionic compounds made up of the following (using monatomic ion charges): a) Al and O b) Na and Br c) Ba and F d) Pb 4+ and O

a) Al2O3 b) NaBr c) BaF2 d) PbO2

Based on the subshells that make up each one, how many electrons can each of the first three principal energy levels hold? a) n = 1, which consists only of the 1s subshell b) n = 2, which consists of the 2s and 2p subshells c) n = 3, which consists of the 3s, 3p, and 3d subshells

a) The 1s subshell can hold a maximum of two electrons, so the first principal energy level can hold a maximum of two electrons. b) The 2s subshell can hold two electrons and the 2p can hold six, so the second principal energy level can hold a total of eight electrons. c) The 3s subshell can hold 2 electrons, the 3p can hold 6, and the 3dcan hold 10, so the third energy level can hold a total of 18 electrons.

Classify the following compounds as ionic or covalent (molecular). a) NaBr b) NH3 c) AlCl3 d) CO2

a) ionic b) covalent (molecular) c) ionic d) covalent (molecular)

Which subshell is indicated by l=2 and what are the allowed m(l) values?

d sub shell and -2, -1, 0, 1, 2

Starting from the ideal gas law, derive the relationship between the density of a gas and its molar mass.

(P*MM)/RT = mass/V

Use the ΔH values for equations I and II to calculate ΔH for the vaporization of ethanol, C2H6O. I. C2H6O(l)→C2H6O(g)I 2 C(s)+3 H2(g)+12 O2(g)→C2H6O(g)ΔH=−235.1kJII 2 C(s)+3 II. H2(g)+12 O2(g)→C2H6O(l)ΔH=−277.7kJ

+42.6 kJ

Determine the oxidation state of the following elements. - Sulfur in the thiosulfate ion, (S2O3)2- - Sulfur in the sulfite ion, (SO3)2- - Chromium in the dichromate ion, (Cr2O7)2- - Cl in NaClO2 - Cl in HClO4

- +2 - +4 - +6 - +3 - +7

Predict the charge on the stable ion formed by each element: - Mg - P - Cl - Na

- +2 - -3 - -1 - +1

Indicate the charge of the monoatomic ions formed by the following elements. Make sure you include proper sign for the charge. For example: +1, -1 - Al - Cs - I

- +3 - +1 - -1

Determine the oxidation state of Cl in each: - Cl2O7 - AlCl4- - Ba(ClO2)2 - ClF4+

- +7 - -1 - +3 - +5

- A gas has a volume of 2.4 L at 25.1 °C and a pressure of 876 mmHg. How many moles of this gas are there? (1 atm = 760 mmHg; R= 0.08206 L* atm / mol*K) - If this gas weighs 8.923 grams, identify this gas from the periodic table.

- .113 mol - Selenium

2NO(g) + 5H2(g) --> 2NH3(g) + 2H2O(g) - If you started with 12.2 grams of Nitrogen Monoxide how many moles of water vapor would be produced? - If we started with 661 grams of nitrogen monoxide how many grams of hydrogen gas would react? - What mass in grams of hydrogen gas would be needed to generate 111 grams of ammonia?

- .407 mol H2O - 111.2 g H2 - 32.9 g H2

Calculate the molarity of the two solutions: - The first solution contains 0.300 mol of NaOH in 2.65 L of solution - The second solution contains 15.1 g of NaCl in 713 mL of solution

- 0.113 M - 0.362 M

Identify the number of sig figs in each of these values - 2000 - 140 - 0.009 - 0.0090 - 0.052000 - 20.00 - 11020

- 1 - 2 - 1 - 2 - 5 - 4 - 4

An aqueous potassium iodate stock solution is made by dissolving 5.53 mol KIO3 in sufficient water for the final volume of the solution to be 2.90L. - Calculate the molarity of the stock KIO3 solution - A 10.0 mL aliquot is removed from the described stock solution and diluted to a total volume of 100.0 mL. Calculate the molarity of the dilute solution.

- 1.91 M KIO3 - 0.191 M KIO3

Pb(NO3)2(aq) + 2NH4I(aq) --> PbI2 (s) + 2NH4NO3(aq) - What volume of a 0.330 M NH4I solution is required to react with 609 mL of a 0.300 M Pb(NO3)2 solution? - How many moles of PbI2 are formed for this reaction?

- 1110 mL - 0.183 mol PbI2

2C​2H​2 (g) + 5O2​ (g) → 4CO2​ (g) + 2H2​O(g) - How many grams of carbon dioxide could be produced if Joenon started with 72.01 g of acetylene and an unlimited supply of oxygen? - How many grams of carbon dioxide could be produced if she started with 140.01 grams of oxygen and assumed an unlimited supply of acetylene? - If Joenon used 72.01 grams of acetylene and 140.01 grams of oxygen, what is the theoretical yield of carbon dioxide? - What is the limiting reactant and the reactant in excess? - Joenon performed this combustion in the lab and found the yield of carbon dioxide to be 130.01 g. What is her percent yield?

- 243.3g CO2 - 154.05g CO2 - 154.05g CO2 - O2 & C2H2 - 84.395%

How many molecules are present in each sample? - 6.10 mol SO2 - 0.343 mol CO

- 3.67 * 10^24 - 2.07 * 10^23

Each 80Se^2- has ________ protons, _______ neutrons, and _______ electrons.

- 34 - 46 - 36

Specific Heats of Substances in cal/g•ºC: - Brick - 0.20 - Ethanol - 0.58 - Wood - 0.10 Calculate the amount of heat, in calories, that must be added to warm 99.6 g of brick from 21.5 ºC to 41.1 ºC Calculate the amount of heat, in calories, that must be added to warm 99.6 g of ethanol from 21.5 ºC to 41.1 ºC Calculate the amount of heat, in calories, that must be added to warm 99.6 g of wood from 21.5 ºC to 41.1 ºC Which substance requires the greatest input of heat energy?

- 390 cal - 1132 cal - 195 cal - Ethanol

How many significant figures are in each of the following numbers? - 0.9683 - 21.1 - 760 - 6.0225*10^23 - 0.08206 - 21.10 - 760. - 0.760

- 4 - 3 - 2 - 5 - 4 - 4 - 3 - 3

How many sig figs are in each number? - 1236 - 1001 - 7.0001 - 0.0011 - 6 atoms - 12.0 - 123.6 - 76500

- 4 - 4 - 5 - 2 - exact - 3 - 4 - 3

To how many sig figs should each answer be rounded? (6.626*10^-34 J*s)(2.9979*10^8m/s)/(4.490*10^-7m) = 4.424072472160 * 10^-19 J (unrounded) (6.022*10^23 atoms/mol)(0.769 g)/(20.18 g/mol) = 2.295*10^22 atoms (unrounded)

- 4 sig figs - 3 sig figs

Determine the: - number of neutrons, protons, and electrons for a bromide ion that has a mass number of 76, and a charge of -1 - element symbol, number or protons, and number of electrons for an ion that has a mass number of 56, 30 neutrons, and a charge of +3 - element symbol, mass number, and charge for an atom or ion that has 51 neutrons, 38 protons, and 36 electrons

- 41 neutrons, 35 protons, 36 electrons - Fe, 26 protons, 23 electrons - Sr, mass number of 89, +2 charge

At constant volume, the heat of combustion of a particular compound, compound A, is -3110.0 kJ/mol. When 1.417 g of compound A (molar mass = 108.29 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 7.525 ºC. - What is the heat capacity (calorimeter constant) of the calorimeter? Suppose a 3.107 g sample of a second compound, compound B, is combusted in the same calorimeter, and the temperature rises from 25.09 ºC to 30.12 ºC. - What is the heat of combustion per gram of compound B?

- 5.410 kJ/ºC - -8.758 kJ/g

2C8H18(l) + 25O2(g) --> 16CO2(g) + 18H2O(l) - How many moles of carbon dioxide can be produced from 7.7 moles of C​ H​ ? - How many moles of water will be produced from 8.9 grams of O​2?​ -How many grams of carbon dioxide will be produced from 88.9 grams of C​ H​ ?

- 61.6 mol - .20025 mol - 274.14g

The cancer chemotherapy drug, cisplatin, Pt(NH​3)2Cl​2 (MM = 300.05g/mol) can be made by reacting (NH​4)​2PtCl4​ ​(MM= 407.03 g/mol) with ammonia in aqueous solution as shown in the following equation. (NH​4)2​ PtCl4​ +2NH3​ →Pt(NH​3)2Cl2​ +2NH​4Cl. - To obtain 12.50g of cisplatin, what volume of 0.125 M NH​3(in mL) is required? - To obtain 12.50 g of cisplatin, what mass of (NH​ )​ PtCl​ is required?

- 666.6 mL NH3 - 16.96 g (NH4)2PtCl4 is required?

What is the valence electron configuration of the following elements? - Bi - I

- 6s26p3 - 5s25p5

Calculate the number of atoms in 1 gram of each elements: - Lithium - Manganese - Sulfur

- 8.68*10^22 - 1.10*10^22 - 1.88*10^22

Ammonium nitrate, NH4NO3, is an ionic compound that is soluble in water. The dissolution of ammonium nitrate is endothermic. NH4NO3(s) --> NH4+ (aq) + NO3- (aq) ∆H < 0 Suppose that 3.1 g of solid ammonium nitrate is added to enough water to make a solution of 60.0 mL, and the resulting temperature of the mixture drops from 20.1 ºC to 16.7 ºC ad the ammonium nitrate is dissolved. - Calculate the enthalpy change of this reaction. Assume that the density of the resulting solution is 1.00 g/mL - Calculate the enthalpy change per mole of ammonium nitrate (molar mass = 80.04 g/mol)

- 850 J = ∆H - ∆H = 22 kJ/mol

If an ideal gas is allowed to expand from 4.20 L to 39.9 L at constant temperature, by what factor does the volume increase? If the initial pressure was 133 bar, what is the final pressure?

- 9.5 - 14 bar

Determine what was oxidized and what was reduced. What was the oxidizing agent and the reducing agent? - Al(s) + 3O2(g) --> 2Al2O3(s) - 2C2H2(g) + 5O2(g) --> 4CO2(g) + 2H2O(g)

- Al ox & reducing agent, O2 red & oxidizing agent - C2H2 ox & reducing agent, O2 red & oxidizing agent

What did the Rutherford's experiment demonstrate? - Atoms contain negative particles called electrons - Mass is conserved in chemical reactions - Atoms contain neutral particles called neutrons - Atoms have a small, dense, positive nucleus

- Atoms have a small, dense, positive nucleus

- The partial pressure of CH​4 is 0.175 atm and that of O2​ is 0.250 atm in a mixture of the two gases. What is the mole fraction of each gas in the mixture? - If the mixture occupies a volume of 10.5 L at 65°C, what is the total number of moles of gas in the mixture? - What is the number of grams of each gas in the mixture?

- CH4 - .412 & O2 - .588 - .161 mol - CH4 - 1.06 g & O2 3.03 g

A chemical reaction is performed in a flask that is connected to a piston. The initial volume of the system is 0.350 L and the final volume is 0.885 L. The pressure remains constant at 1.00 atm. - Determine whether the piston moves upward or downward over the course of this reaction - Given that 1 L • atm = 1010.325 J, calculate the amount of work performed (in joules) during this reaction.

- Change in volume is 0.535 L, since the volume increases, the piston moves upwards - Work performed = -54.2 J

Which of the changes are chemical changes? - Sugar dissolved in water - Warm soda bottle fizzes when opened - The copper roof turns green over time - Baking soda is dissolved in vinegar and bubbles form - A fog appears on the windshield in cold weather

- Copper roof - Baking soda

What would happen to an atom if... - The number of protons changed - The number of neutrons changed - The atom gained or lost e-

- Different element - Isotope change - Ion difference

Label the following as an element, compound, or mixture (is it heterogeneous or homogeneous) - O2 - Ba - NaCl - Sand - C6H12O - C2H4 - Fruit Salad - Mercury - H2O

- E - E - C - Mix homogenous - C - C - Mix heterogeneous - E - C

Water inside of a bowl evaporates after it is left outside on a hot summer day. This phase change absorbs 1150 kJ of heat from the surroundings. - Determine whether this reaction is endothermic or exothermic - Determine the value of ∆H for this reaction

- Energy is added to the system (water) in order for it to evaporate. Heat is transferred from surroundings to system --> endothermic (∆H > 0) - This is an open system so pressure is constant. ∆H is qual to amount of heat transferred and is positive because it's endothermic so ∆H = 1150 kJ

Determine if the following statements are TRUE or FALSE based on the kinetic molecular theory. - At the same temperature, all gas molecules in an ideal gas sample are moving at the same speed. - At the same temperature, all ideal gases have the same average kinetic energy.

- False - True

True or False (if false correct it) - Act of ice cream melting in the sun is a physical property - Concept of the fender on your car rusting is a chemical change - Process of your body digesting a piece of bread is a chemical change - Concept of a glass of water evaporating into the air is a physical property

- False: physical CHANGE not property - False: CONCEPT --> chemical property not change - True - True

Find the empirical formula of each of the following compounds (a) A compound containing 11.66 g iron (Fe) and 5.01 g oxygen (O) (b) a compound consists of C, O and F only with 21.7% C and 9.6% O by mass

- Fe2O3 - C3OF6

Write net ionic equations for the following acid-base reactions. - HNO3(aq) + KOH(aq) --> KNO3(aq) + H2O(l) - H3PO4(aq) + 3 NaOH(aq) --> Na3PO4(aq) + 3 H2O(l)

- H+(aq) + OH-(aq) --> H2O(l) - 3H3PO4(aq) + 3 OH-(aq) --> (PO4)3- (aq) + 3 H2O(l)

Water can be formed via the reaction of gaseous hydrogen and oxygen. 2 H2(g)+O2(g)→2 H2O(l)ΔH=-572 kJ - Write the balanced equation that shows 1 mol water produced. - Determine the enthalpy of the reaction in units of kJ/mol of water produced.

- H2 (g) + 1/2 O2 (g) --> H2O (l) - The reaction that produces 2 mol of H2 has an enthalpy of −572 kJ. Therefore, the enthalpy of the reaction per mole of water produced is: −572 kJ/2 mol water= −286kJ/mol water produced

List the polyatomic ions with a -1 charge

- H2PO4 - Dihydrogen Phosphate - C2H3O2 - Acetate - HSO3 - Hydrogen Sulfite - HSO4 - Hydrogen Sulfate - HCO3 - Hydrogen Carbonate - NO2 - Nitrite - NO3 - Nitrate - CN - Cyanide - OH - Hydroxide - ClO - Hypochlorite - ClO2 - Chlorite - ClO3 - Chlorate - ClO4 - Perchlorate

List the polyatomic ions with a -2 charge

- HPO4 - Hydrogen Phosphate - SO3 - Sulfite - SO4 - Sulfate - CO3 - Carbonate

Is Br an alkaline earth metal, halogen, alkali metal, or a chalcogen? As an ion, what is its charge and what type of ion is that?

- Halogen - -1 - Anion

Wood is burned in an open fireplace. The reaction releases 250 kJ of heat and does 15.0 kJ of work on the surroundings. - Determine whether this reaction is endothermic or exothermic. - Calculate ΔH for this reaction. - Calculate ΔU for this reaction.

- Heat is transferred from the system to the surroundings, so the reaction is exothermic (i.e., ΔH < 0). - Since this is an open system, the pressure is constant. Therefore, ΔH is equal to the amount of heat transferred and it has a negative value because the heat is transferred from the system to the surroundings: ΔH = q = −250 kJ. - ΔH depends only on q, but ΔU depends on q and w. In this case, the work (15.0 kJ) is done on the surroundings, so it also has a negative value. ΔU=q+w=(−250 kJ)+(−15.0 kJ)=−265 kJ

Identify each energy exchange as primarily heat or work, and determine whether the sign of the internal energy, ∆E, is positive or negative for the system. - An ice chest is filled with ice to cool down drinks. The drinks are the system. - A chair is pushed across a room. The chair is the system. - A pot of water is warmed by a flame. The water is the system.

- Heat, negative - Work, positive - Heat, positive

Determine if each example is an intensive property or extensive property - Density - Hardness - Weight - Temperature - Volume - Length

- I - I - E - I - E - E

A small mass of solid potassium chloride, KCl, is dissolved in 100 mL of water inside a constant-pressure calorimeter. As the reaction solution is mixed, temperature of the solution drops from 20.1°C to 17.4°C. - Determine the signs of q(soln) and q(p) in the reaction. - Determine whether the reaction is endothermic or exothermic.

- In this reaction, the temperature of the water inside the calorimeter decreases, indicating the heat is transferred from the water to the reaction. Therefore, qsoln is negative (heat is lost) and qp is positive (heat is gained). - Heat is transferred from the solution to the reaction, so the reaction is endothermic.

Lactose reacts with O2 to form CO2 and H2O. C12H22O11(s)+12 O2(g)→12 CO2(g)+11 H2O(l) A small mass of lactose reacts with excess O2 inside a bomb calorimeter and the temperature of the water inside the calorimeter increases from 19.4°C to 28.6°C. - Determine the signs of qsoln and qv in the reaction. - Determine whether the reaction is endothermic or exothermic.

- In this reaction, the temperature of the water inside the calorimeter increases, indicating the heat is transferred from the reaction to the water. Therefore, qsoln is positive (heat is gained) and qv is negative (heat is lost). - Heat is transferred from the reaction to the solution, so the reaction is exothermic.

Given Fe(s), Ag+, Sn(s), Mg2+, Li(s), and Ca2+, identify: - most active metal - most reactive metal ion - strongest reducing agent - best oxidizing agent

- Li - Ag+ - Li - Ag+

Name the compounds: - Li2SO4 - NH4NO3 - Mg(OH)2

- Lithium Sulfate - Ammonium Nitrate - Magnesium Hydroxide

What were the components of Dalton's Atomic Theory?

- Matter composed of tiny, indivisible* particles (atom) - Atoms of the same elements are the exact* same - Atoms combine to form molecules - Atoms of pairs of elements can combine with each other in different small, whole number ratios

In 1911, Hans Geiger and Ernest Marsden, working under Ernest Rutherford, conducted an experiment involving alpha particles and gold foil that led to the discovery of the nucleus in atoms. The nucleus of an atom accounts for: - Most the size and mass of the atom - very little of the size and mass of the atom - most of the atom's size but very little of its mass - most of the atom's mass but very little of its size

- Most of the atom's mass but very little of its size

Balance the given equations - N2 + O2 --> NO - TiCl4 + H2O --> TiO2 + HCl - CH4 + O2 --> CO2 + H2O - C2H6 + O2 --> CO2 + H2O - Al(NO3)3 + H2SO4 --> Al2(SO4)3 + HNO3

- N2 + O2 --> 2NO - TiCl4 + 2H2O --> TiO2 + 4HCl - CH4 + 2O2 --> CO2 + 2H2O - 2C2H6 + 7O2 --> 4CO2 + 6H2O - 2Al(NO3)3 + 3H2SO4 --> Al2(SO4)3 + 6HNO3

Write the formula for the ionic compound formed from each pair of elements. - Sodium & Sulfur - Potassium & oxygen - Aluminum & phosphorus - Bromine & magnesium

- Na2S - K2O - AlP - MgBr2

Write the formulae of the following compounds. You must recognize the names of common polyatomic ions and know their charges. - sodium sulfate - nickel (II) phosphate - zinc acetate - ammonium carbonate - barium hydroxide - iron (III) chlorate - aluminum nitrate - magnesium sulfite - beryllium hydrogen carbonate - potassium dihydrogen phosphate

- Na2SO4 - Ni3(PO4)2 - Zn(CH3COO)2 - (NH4)2CO3 - Ba(OH)2 - Fe(ClO3)3 - Al(NO3)3 - MgSO3 - Be(HCO3)2 - KH2PO4

Predict the products and write balanced total, ionic, and net ionic equations for the following reactions: - Na2SO4(aq) + BaCl2(aq) --> - Ca(NO3)2(aq) + KOH(aq) -->

- Na2SO4(aq) + BaCl2(aq) --> BaSO4(s) + 2 NaCl(aq) 2Na+(aq) + (SO4)2-(aq) + Ba2+(aq) + 2Cl-(aq) --> BaSO4(s) + 2Na+(aq) + 2Cl-(aq) Ba2+(aq) + (SO4)2-(aq) --> BaSO4(s) - Ca(NO3)2(aq) + 2KOH(aq) --> Ca(OH)2(s) + 2KNO3(aq) Ca2+(aq) + 2(NO3)-(aq) + 2K+(aq) + 2 OH-(aq) --> Ca(OH)2(s) + 2K+(aq) + 2(NO3)-(aq). Ca2+(aq) + 2OH-(aq) --> Ca(OH)2(s)

Write the formula of the compounds. Since a compound must be neutral, the charge of the ions can be used to determine the proper subscripts in the formula. - Sodium Iodide - Calcium Fluoride - Iron (III) Oxide - Aluminum Sulfite - Phosphorous Trioxide - Potassium Oxide - Copper (II) Chloride - Lithium Bromide - Titanium (IV) Nitride - Zinc (II) Hydride

- NaI - CaF2 - Fe2O3 - Al2S3 - PO3 - K2O - CuCl2 - LiBr - Ti3N4 - ZnH2

MgCl2 (aq) + 2NaOH (aq) --> Mg(OH)2 (s) + 2NaCl(aq) A 156.0 mL solution of 0.379 M MgCl2 reacts with a 40.18 mL solution of 0.726 M NaOH to produce Mg(OH)2 and NaCl - Identity the limiting reactant - Calculate the mass of Mg(OH)2 that can be produced - The actual mass of Mg(OH)2 isolated was 0.698g. Calculate the percent yield of Mg(OH)2

- NaOH - 0.851 g Mg(OH)2 - 82.0%

Name the following compounds: - NF3 - Ca(NO3)2 - Cu(OH)2 - SO2 - Fe2(CO3)3 - NH4ClO3 - Li3PO4 - CCl4 - PI3 - N2O4

- Nitrogen Trifluoride (molecular) - Calcium Nitrate (ionic) - Copper (II) Hydroxide (ionic) - Sulfur Dioxide (molecular) - Iron (III) Carbonate (ionic) - Ammonium Chlorate (ionic) - Lithium Phosphate (ionic) - Carbon Tetrachloride (molecular) - Phosphorus Triodide (molecular) - Dinitrogen Tetroxide (molecular)

Determine which of the following are redox reactions. - 2HBr(aq) + Ba(OH)2(aq) --> BaBr2(aq) + 2H2O(l) - 2CoCl2(aq) + Cl2(g) --> 2CoCl3(aq) - 2NH4I(aq) + Pb(NO3)2(aq) --> 2NH4NO3(aq) + PbI2(s) - (NH4)2S(aq) + CuCl2(aq) --> CuS(s) + 2NH4Cl(aq) - 2NaOH(aq) + H3PO4(aq) --> Na2HPO4(aq) + 2H2O(l) - H2O(l) + N2O5(g) --> 2HNO3(aq) - CuSO4(aq) + Zn(s) --> ZnSO4(aq) + Cu(s) - NH4NO3(s) --> N2O(g) + 2H2O(l)

- Not redox - Co oxidized, Cl reduced - Not redox - Not redox - Not redox - Not redox - Cu reduced, Zn oxidized - One N oxidized, other N reduced

For each element list the symbol, atomic number, mass number, and the numbers of protons, electrons, and neutrons. - Phosphorus - Beryllium - Cobalt

- P, 15, 31, 15, 15, 16 - Be, 4, 9, 4, 4, 5 - Co, 27, 59, 27, 27, 32

Classify each property as physical or chemical - Melting point - Color - Susceptibility to rust - Flammability - Conductivity - Boiling Point

- Physical - Physical - Chemical - Chemical - Physical - Physical

Determine whether a reaction will occur and identify the formula of the insoluble product, if any. - Na2SO4(aq) + BaCl2(aq) - Ca(NO3)2(aq) + KOH(aq)

- Precipitation - Precipitation

What are the four quantum numbers (symbols and name)? What do each of them describe?

- Principle Quantum Number (n): Size and energy of orbitals & which electron orbital it is - Angular Momentum Quantum Number (l):Type of orbital (s, p, d, f) - Magnetic Quantum Number (m(l)): orientation of orbital (px, py, or pz) - Spin Quantum Number (m(s)): spin of e- in orbital (up or down)

Identify which subatomic particles match each of these descriptions. - Have a relative charge of +1 - Have a relative charge of -1 - Have no charge - Located in nucleus of an atom - Have a much lower mass than the other two types of particles

- Protons - Electrons - Neutrons - Protons - Neutrons - Electrons

Classify these substances. More than one answer may apply (compound, pure substance, homogeneous mixture, heterogeneous mixture, solution, element) N2 O2 N2O Air (mostly N2 and O2

- Pure substance & element - Element & pure substance - Compound & pure substance - Homogeneous mixture & solution

Determine if each example is a qualitative or quantitative measure - The volume of the box is 4m^2 - The box is frozen - The box is blue

- Quantitative - Qualitative - Qualitative

Ernest Rutherford was a prominent scientist who contributed significantly to the theory of atomic structure. Which of the statements are true? - Rutherford theorized that atoms contain a positively charged region called the nucleus - Rutherford devised the solar system model to describe the layout of the atom - Rutherford disproved the plum pudding model of the atom - Rutherford devised the plum pudding model to describe the layout of an atom

- Rutherford theorized that atoms contain a positively charged region called the nucleus - Rutherford disproved the plum pudding model of the atom

The chemical symbols of several elements are provided, give the name of the element. - Na - Te - Fe - Rn

- Sodium - Tellurium - Iron - Radon

Are the following salts soluble or insoluble in water? - Ba(ClO4)2 - CaSO4 - Mg(OH)2 - CaCrO4

- Soluble - Insoluble - Insoluble - Insoluble

Give the systematic name of each covalent compound - SF6 - P4S3 - CO - P3N5

- Sulfur Hexaflouride - Tetraphosphorus Trisulfide - Carbon Monoxide - Triphosphorus Pentanitride

Describe the characteristics and give an example of: - Matter - Pure Substances - Mixtures - Elements - Compounds - Homogenous - Heterogeneous

- Takes up space & has mass (me!) - Single type of element/compound (24k gold) - Not bonded composition ≥ 2 substances (trail mix) - Single type of atom in a substance (gold) - ≥ 2 elements bonded (table salt) - Uniform composition in a mixture (sugar water) - Nonuniform composition in a mixture (pizza)

A chemical reaction is performed in a flask that is sealed with a piston, similar to the experimental setup shown in Figure 6.8. The initial volume of the system is 0.550 L and the final volume is 0.375 L. The pressure remains constant at 1.00 atm. - Given that 1 L · atm = 101.325 J, calculate the amount of work performed (in joules) during this reaction. - Determine whether the piston moves upward or downward over the course of this reaction.

- The change in volume, ΔV, is calculated as follows: ΔV=Vfinal−Vinitial=(0.375 L)−(0.550 L)=−0.175 L Next, multiply the change in volume by the pressure to calculate the work performed. w=−PΔV=−(1.00 atm)(−0.175 L)=0.175 L⋅atm The work value in units of L · atm is converted to units of J. w=0.175 L⋅atm(101.325 J/1 L⋅atm)=17.7 J - The sign of the work is positive, so the surroundings do work on the system, as further evidenced by the volume decrease. A decrease in volume means that the piston moves downward.

The equation and enthalpy for the combustion of methane, CH4, is as follows. CH4(g)+2 O2(g)→CO2(g)+2 H2O(l)ΔH=−891 kJ - Determine the amount of heat produced by the combustion of 3.30 mol of methane. - Determine the enthalpy for the equation: 2 CH4(g)+4 O2(g)→2 CO2(g)+4 H2O(l)

- The coefficient of CH4 in the equation is 1, so 891 kJ of heat are produced per 1 mol of CH4. 3.30 mol CH4(891 kJ/1 mol CH4)=2940 kJ - The equation coefficients have been multiplied by 2, so the enthalpy value must also be multiplied by 2. ΔH = 2(-891 kJ) = -1780 kJ.

A 9.49 g sample of calcium sulfide was decomposed into its constituent elements, producing 5.28 g of calcium and 4.21 g of sulfur. Which of the statements are consistent with the law of constant composition (definite proportions)? - The ratio of calcium to sulfur will vary based on how the sample was prepared - The mass ratio of Ca to S in every sample of calcium sulfide is 1.25 - Every sample of calcium sulfide will have 5.28 g of calcium - Every sample of calcium sulfide will have 55.6% mass of calcium - The mass percentage of calcium plus the mass percentage of sulfur in every sample of calcium sulfide equals 100%

- The mass ratio of Ca to S in every sample of calcium sulfide is 1.25 - Every sample of calcium sulfide will have 55.6% mass of calcium - The mass percentage of calcium plus the mass percentage of sulfur in every sample of calcium sulfide equals 100%

Elemental boron reacts with oxygen gas to form diboron trioxide, B2O3, 4 B (s) + 3 O2 (g) --> 2 B2O3 (s) ∆H < 0 A sample of elemental boron reacts with excess O2 inside a bomb calorimeter. - Determine whether the reaction is endothermic or exothermic. - Determine the signs of q(soln) and q(v) in the reaction.

- The reaction is exothermic since ∆H is negative - In an exothermic reaction inside a calorimeter the temperature of the water inside the calorimeter increases indicating the heat is transferred from the reaction to the water. Therefore, q(soln) is positive (heat is gained) and q(v) is negative (heat is lost). Despite the fact that ∆H is not mathematically equivalent to q(v), you can still kind of relate them by saying that the reactions releases heat tot he water and calorimeter

A small mass of solid calcium chloride, CaCl2, dissolves exothermically in 100 mL of water, originally at 21 ºC, inside a constant-pressure calorimeter - Determine the signs of q(soln) and q(p) in the reaction. - Determine whether the final temperature of the solution is above or below 21 ºC after the calcium chloride is completely dissolved.

- The reaction is exothermic, so the heat is transferred from the reaction to the water. Therefore, q(soln) is positive (heat is gained) and q(p) is negative (heat is lost) - Heat is transferred from the reaction to the solution, so final temperature of the water will be above 21 ºC

A chemical reaction is performed in a flask that is connected to a piston. Heat is allowed to enter or escape this system, but matter cannot. (Does this make the system open, closed, or isolated?) The reaction releases 890 J of heat to the surroundings and the gas produced performs 450 J of work on the surroundings by pushing the piston upward. - Determine the signs of q and w in this reaction. - Determine ∆U for this reaction

- The reaction produces heat and releases it to the surroundings, so q is negative: q = -890 J. The reaction produces a gas that does work on the surroundings, so w is negative, too: w = -450 J. - Negative values of q and w are used to calculate the change in internal energy: ΔU=q+w=(−890 J)+(−450 J)=−1340 J

True or False - The orbits in hydrogen atom can only exist at specific, fixed distances from the nucleus. - The closer an orbit is to the nucleus, the higher the energy of the electron in the orbit. - The electron in an orbit has specific, quantized energy. - When an electron goes from a lower orbit to a higher orbit, it loses energy by emitting a photon.

- True - False - True - False

Indicate whether each of the following is true or false: - Every compound is a pure substance - Every compound contains two or more elements - Every mixture contains two or more compounds - Every pure substance is a compound - All mixtures are homogeneous

- True - True - False: Mixes may contain elements, compounds, or both - False: Some pure substances, such as oxygen gas, are elements - False: Some mixtures, such as iron metal & solid sulfur, are heterogeneous.

What does the scientific method involve?

- What background info, data, or observations you have? - What is your initial explanation for background info and data? - How can you check? (experiments & analysis)

Determine whether the value of w or q is positive or negative in each of the following scenarios. - A person rolls a bowling ball across the floor, where the bowling ball is defined as the system. - A person rolls a bowling ball across the floor, where the person is defined as the system. - An ice pack is placed on a person's sore back, where the ice pack is defined as the system.

- Work is being done on the system (the bowling ball) by the surroundings. The value of w is positive. - Work is being done by the system (the person) on the surroundings. The value of w is negative. - Heat is being transferred from the surroundings (the person's back) to the system (the ice pack). The value of q is positive.

Identify the type of energy transfer (work or heat) in each scenario, then determine whether the sign of w or q is positive or negative. - A crane lifts a steel beam, where the steel beam is defined as the system - Steam condenses on a cool mirror, where the mirror is defined as the system

- Work is being done on the system (the steel beam) by lifting it against gravity. The value of w is positive. - Steam cools and loses thermal energy when it goes from the gas phase to the liquid phase on the surface of the mirror. The transfer of heat from the steam (part of the surroundings) to the mirror (the system) results in positive value of q.

Determine whether the following pairs of reactants will react. - Ni(s) + Pb2+(aq) --> - Na(s) + Ag(s) --> - Zn2+(aq) + Mg(s) --> - CaCl2(aq) + Cu(s) --> - Au(NO3)3(aq) + Ag(s) --> - Li+(aq) + Mn2+ (aq) -->

- Yes - Nickel is higher in activity series, able to donate e- to ion - No - Both metals so neither can accept e- - Yes - Magnesium is higher in activity series so able to donate e- to ion - No - Cu is less active than ion so it can't react - Yes - Ag is more active than ion so it donates e- - No - Both are ions so neither can donate

Identify the driving force for each of the following reactions. - 2HBr(aq) + Ba(OH)2(aq) --> BaBr2(aq) + 2H2O(l) - 2CoCl2(aq) + Cl2(g) --> 2CoCl3(aq) - 2NH4I(aq) + Pb(NO3)2(aq) --> 2NH4NO3(aq) +PbI2(s) - (NH4)2S(aq) + CuCl2(aq) --> CuS(s) + 2NH4Cl(aq) - 2NaOH(aq) + H3PO4(aq) --> Na2HPO4(aq) + 2H2O(l) - H2O(l) + N2O5(g) --> 2HNO3(aq) - CuSO4(aq) + Zn(s) --> ZnSO4(aq) + Cu(s) - NH4NO3(s) --> N2O(g) + 2H2O(l)

- acid-base = neutralization - synthesis = redox - double-replacement = precipitation - double-replacement = precipitation - acid-base = neutralization - synthesis = redox - single-replacement = redox - decomposition = redox

Which of the following ratio is correct as a conversion between "nm" and "m"? - 1nm/10^-9m - 1m/10^9nm - 10^-9nm/1m

- correct - correct - incorrect

Determine if each of the reactions are endothermic or exothermic. What are the signs of ΔH? - Water boiling - Water freezing

- exothermic -∆H - endothermic +∆H

The following combination of quantum numbers are NOT allowed. Identify which number violates the rules. - n = 1, l = 1, m(l) = 0 - n = -1, l = 1, m(l) = 1 - n = 2, l = 3, m(l) = 1 - n = 3, l = 1, m(l) = -2

- l - n - l - m(l)

Put the steps in order to describe and experiment that follows the scientific method. - test revised hypothesis - test initial hypotehsis - make an initial observation - the revised hypothesis may eventually become a theory - revise hypothesis - testing confirms the revised hypothesis - testing discredits the initial hypothesis - form initial hypothesis

- make initial observation - form initial hypothesis - test initial hypothesis - testing discredits the initial hypothesis - revise hypothesis - test revised hypothesis - testing confirms the revised hypothesis - the revised hypothesis may eventually become a theory

Identify the missing information for each neutral isotope. - A Se atom has a mass number of 77. Determine the number of neutrons, protons, and electrons in this neutral isotope - A neutral isotope has a mass number of 65 and 36 neutrons. Identify the element symbol of this isotope and determine the number of protons and electrons - A neutral isotope has 45 neutrons and 36 electrons. Identify the element symbol, mass number, and number of protons

- neutrons: 43, protons: 34, electrons: 34 - Cu, protons: 29, electrons: 29 - Kr, mass number: 81, protons: 36

To what decimal place should each answer be rounded? How many sig figs does the rounded answer have? - 9 cm + 2.8 cm = 11.8 (unrounded) - 0.135 atm + 0.6 atm = 0.735 atm (unrounded)

- ones place, 2 sig figs - tenths place, 1 sig fig

Classify each of these reactions as either acid-base, precipitation, redox, or none: - Ba(ClO3)2(s) --> BaCl2(s) + 3O2(g) - 2 NaCl(aq) + K2S(aq) --> Na2S(aq) + 2KCl(aq) - CaO(s) + CO2 (g) --> CaCO3(s) - KOH(aq) + AgNO3(aq) --> KNO3(aq) + AgOH(s) - Ba(OH)2(aq) + 2HNO2(aq) --> Ba(NO2)2(aq) + 2H2O(l)

- redox - none - none - precipitation - acid-base

A student adds 25 mL of a strong acid to 25 mL of a strong base inside a coffee cup calorimeter and immediately places the lid on top. The solution temperature rises from 20.5°C to 25.0°C. The specific heat of water is 4.184 J/g · °C and the density of water is 1.00 g/mL in this temperature range. Assume that the density of the acid and base solutions are also 1.00 g/mL. - Calculate the enthalpy change of this reaction. - Assuming that the strong acid has a concentration of 1.5 M, calculate the enthalpy change per mole of acid.

- ∆H = -940 J - ∆H = -25kJ/mol

A 17.3 mL sample of argon gas was originally at 0°C and 1.00 atm pressure. If its final volume is 10.9 mL and its final pressure is 678 torr, what is its final temperature in degrees Celsius?

-120 ºC

A sample of sulfur hexafluoride gas occupies 9.10 L at 198 °C. Assuming that the pressure remains constant, what temperature (in °C) is needed to reduce the volume to 2.50 L?

-144 ºC

Calculate ∆Hºrxn for the complete combustion of 1.00 mol of ethane, C2H6. C2H6 (g) + 5/2 O2(g) --> 2 CO2 (g) + 3 H20(l)

-1560.4 kJ

The temperature on Mercury may drop to -263 ºF at night. What is this temperature in degrees Celsius?

-163.8 ºC

Use the following reactions and given ΔH: Ca (s) + CO2 (g) + 1/2 O2 (g) → CaCO3 (s) ΔH1 = − 812.8 kJ 2 Ca (s) + O2 (g) → 2 CaO (s) ΔH2 = − 1269.8 kJ Calculate ΔHrxn for the following reaction: CaO (s) + CO2 (g) → CaCO3 (s)

-177.9 kJ

A 456 mL sample of argon gas is expanded at constant pressure to 1.75 L at 55 ºC. What was the original temperature of the gas in ºC?

-188 ºC

Calculate ΔH°rxn for the complete combustion of 1.00 mol of propane, C3H8, at 25°C and 1 atm. C3H8(g)+5 O2(g)→3 CO2(g)+4 H2O(l)

-2.220 * 10^3 kJ

A 3.50 g sample of glucose is ignited inside a bomb calorimeter in the presence of excess oxygen gas. The temperature rises from 20.0 ºC to 85.9 ºC. Given that the heat capacity of the calorimeter is 810.1 J/ºC, determine the ∆U(rxn) for the combustion of glucose in units of kJ.mol of glucose

-2.75 * 10^3 kJ/mol glucose

A 3.50 g sample of glucose is ignited inside a bomb calorimeter in the presence of excess oxygen gas. The temperature rises from 20.0 ºC to 85.9 ºC. Given that the heat capacity of the calorimeter is 810.1 J/ºC, determine ∆U(rxn) for the combustion of glucose in units of kJ/mol of glucose.

-2.75 * 10^3 kJ/mol glucose

Use the ΔH values for equations I, II, and III to calculate ΔH for the following reaction: C2H2+2H2(g)→C2H6 I 2C2H2+5O2→4CO2+2H2O ΔH=−2320kJ II 2C2H6+7O2→4CO2+6H2O ΔH=−3040kJ III 2H2+O2→2H2O ΔH=−572kJ

-212 kJ

Use the ΔH values for equations I, II, and III to calculate ΔH for the following reaction:C2H2+2H2(g)→C2H6 I. 2C2H2+5O2→4CO2+2H2O ∆H = -2320 kJ II. 2C2H6+7O2→4CO2+6H2O ΔH=−3040kJ III. 2H2+O2→2H2O ΔH=−572kJ

-212 kJ

Burning 1.00 mol of diborane, B2H6, in excess oxygen in a constant-volume calorimeter warms 20.0 kg of water by 25.7 ºC. Calculate the heat produced in this combustion process: B2H6 (g) + 3 O2 (g) --> B2O3 (s) + 3 H2O (l)

-2150 kJ (system lost heat)

The temperature on Mars during the winter may reach a low of -153 0C , which equals ________ 0F. Round your answer to 3 significant figures. Enter the numerical value only without the unit.

-243

Calculate the enthalpy change for the combustion of 1.00 mol of butane (bottled gas), C4H10, to give carbon monoxide, CO, and water, H2O. Use the following equation: 2 C4H10(g)+9 O2(g)→8 CO(g)+10 H2O(l)

-3490 kJ

The molecular formula of caffeine is C8H10N4O2. Each caffeine molecule contains _____ N atoms. Using the periodic table handed out in class (the Word one), the molecular weight of caffeine is ________ (include units). Round your answer to two decimal places.

-4 - 194.22 amu

Metallic mercury, Hg, can be obtained by heating the mineral cinnabar, HgS, in the presence of oxygen, O2. Use the following equation: HgS(s)+O2(g)→Hg(l)+SO2(g) Determine the amount of heat released when 5.50 g of HgS is heated in the presence of excess oxygen.

-5.64 kJ

Given that H2(g) + F2(g) --> 2HF(g) ∆Hºrxn = -546.6 kJ 2H2(g) + O2(g) --> 2H2O(l) ∆Hºrxn = -571.6 kJ calculate the value of ∆Hºrxn for 2F2(g) + 2H2O(l) --> 4HF(g) + O2(g)

-521.6 kJ

For the reaction O2 + 2SF4 --> 2OSF4, calculate the enthalpy of reaction using the following bond energies: S-F --> 310 S-O --> 265 S=O --> 523 O-O --> 142 O=O --> 498 O-F --> 180

-548 kJ/mol

A 1.000-g sample of decane, C10H22 is ignited inside a bomb calorimeter. The temperature rises from 20.0°C to 78.8°C. Given that the heat capacity of the calorimeter is 810.1 J/°C, determine ΔUrxn for the combustion of decane in units of kJ/mol of decane.

-6.78 * 10^3 kJ/mol

A 1.000-g sample of decane, C10H22 is ignited inside a bomb calorimeter. The temperature rises from 20.0°C to 78.8°C. Given that the heat capacity of the calorimeter is 810.1 J/°C, determine ΔUrxn for the combustion of decane in units of kJ/mol of decane.

-6.78 * 10^3 kJ/mol decane

A sample of oxygen gas is mixed with argon gas. The mixture has a total pressure of 876 mmHg and the argon gas has a partial pressure of 0.129 atm. What amount (in moles) of oxygen gas is contained in 1.28 L of the mixture at 25°C? ​(Hint: use the ideal gas law)

.0534 mol O2

What is the density (in g/L) of a metal that has a mass of 1,430 mg and occupies a volume of 7 L?

.2 g/L

Ricky wants to make a solution that is 7.89 M. He has a stock solution that is 10.1 M. How many L of the stock solution does he need to add to make 379 mL of his wanted 7.89 M solution? (Hint: Use M​ V​ =M​ V​ )

.296 L stock solution

A 1.00-L mixture of He, Ne, and Ar has a total pressure of 662 mmHg at 298 K. If the partial pressure of He and Ne is 341 mmHg and 112 mmHg, respectively, what is the mass (in g) of Ar in the mixture?

.449 g Ar

Perform the conversions: 548.8 mmHg --> atm 0.598 atm --> Torr 264.9 kPa --> atm 590.0 mmHg --> Pa

.7221 atm 454 Torr 2.614 atm 78660 Pa

Underline the significant digits in each of the following measurements. If a digit is uncertain, place a question mark under it. 0.0020 m 1.200 m 10.002 m 6000 m

0.0020 m The zeros to the left of the two are not significant (rule 1), but the one to the right is (rule 3). 1.200 m The zeros to the right of the two are significant (rule 3). 10.002 m Zeros between significant digits are significant (rule 2). 6000 m The 6 is significant because all nonzero digits are significant. The zeros to the right of all other digits in an integer are uncertain; they may reflect the precision or just the magnitude of the number. Without further information, it is impossible to tell (rule 4), so you would conclude that they are not significant.

(80.21 g -79.93 g)/65.22 cm^3

0.0043 g/cm^3

The normal concentration range of glucose in healthy human adult blood is 79.2-110 mg/dL. Calculate this concentration range in units of molarity. The molar mass of glucose is 180.16 g/mol.

0.00440 M - 0.00611 M

A chemist places 0.270 g NaNO3 in a flask and adds water until the total volume is 0.700L. Calculate the molarity of the solution. What is the concentration in millimolar (mM)?

0.00454 M 4.54 M

Calculate the number of moles of solute in 45.75 mL of 0.1155 M K2Cr2O7(aq).

0.005296 moles

How many moles of barium ions and how many grams of barium chloride would be required to produce 6.11 g of barium sulfate?

0.0262 mol Ba2+ 5.45 g BaCl2

In a certain reaction, 0.225 mol H2 gas reacts partially with N2 gas to yield gaseous NH3. If 0.033 mol H2 remains after the reaction is stopped, how many moles of N2 react with H2?

0.0640 mol N2 reacted

When 1.06 g Hg2O is decomposed in a sealed system, the oxygen produced has a pressure of 0.514 atm and a volume of 62.5 mL at 35.25°C. Calculate the value of R from these data. 2 Hg2O(s)heat−→4 Hg(l)+O2(g)

0.08206 (L*atm)/(mol*K)

My mother does not believe me that the pressure of the gas particles in my oven will increase if the temperature of my oven increases. To test her theory, I decided to set my oven to a temperature of 450 °F. The pressure of the gas particles in my oven were 0.0896 atm at this moment. I then turned the oven up to 475 °F. What ending pressure did the particles have in the oven? Was my mother correct? Why or why not?

0.0921 atm

Calculate the number of moles of oxygen gas in a 2.60 L container at 19°C and 755 torr.

0.108 mol

A mixture of oxygen and neon has a pressure of 1.031 atm. if the pressure of the oxygen is 0.922 atm, what is the pressure of the neon?

0.109 atm

A beaker containing 75.0 mL of salt water is left uncovered until all of the water has evaporated. If there are 0.505 g of NaCl left in the beaker, what is the concentration of NaCl in the original solution?

0.115M

The partial pressure of hydrogen and oxygen in a mixture are 148 torr and 740 torr, respectively. What is the mole fraction of hydrogen in the mixture?

0.167

A nurse must prepare 4.00 L of 0.250 M saline (NaCl) solution. What volume of 6.00 M solution should the nurse dilute?

0.167 L

How many moles of Na2SO4 are produced by the reaction of 0.550 mol H2SO4 with 0.375 mol NaOH? H2SO4(aq) + 2NaOH(aq) --> Na2SO4(aq) + 2H2O(l)

0.188 mol Na2SO4

A TA prepares a glucose solution by diluting 0.100 L of a 1.10 M glucose stock solution to 500.0 mL in a volumetric flask. What is the molarity of the diluted solution?

0.220M

A 73.0 mL aliquot of a 1.70 M solution is diluted to a total volume of 218 mL. A 109 mL portion of that solution is diluted by adding 147 mL of water. What is the final concentration? Assume the volumes are additive.

0.242 M

How many liters of oxygen gas at 21°C and 1.13 atm can be prepared by the thermal decomposition of 0.950 g KClO3? 2 KClO3(s)heat−→2 KCl(s)+3 O2(g)

0.248 L O2

What is the molarity of the solution when 123 mL of a 1.1 M glucose stock solution is diluted to 500. mL.

0.27 M

A 10.5 L sample of gas at 292 K contains O2 at 0.622 atm and N2 at 0.517 atm. Calculate (a) the total number of moles of gas in the sample and (b) the number of moles of O2 present.

0.273 mol

A mixture of 6.00 g oxygen and 9.00 g methane (CH4) is placed in a 15.0 L vessel at 0 ºC. What is the partial pressure of O2 (in atm) in the vessel?

0.280 atm

A 2.48 L sample of gas at 272 K and 0.934 atm contains 2.95 g O2 and an unknown amount of N2. Calculate (a) the partial pressure of O2 and N2 and (b) the mass of N2 present.

0.325 g N2

The mass percent of titanium dioxide (TiO2) in an ore can be evaluated by carrying out the following reaction and measure the amount of O2 gas produced: 3 TiO2 (s) + 4 BrF3 (l) → 3 TiF4 (s) + 2 Br2 (l) + 3 O2 (g) If 2.376 g of a TiO2-containing ore generates 0.143 g O2, what is the mass percent of TiO2 in the ore sample?

0.357g TiO2 15.0%

How many moles of helium are in a party balloon that contains 2.74*10^23 helium atoms?

0.455 mol He

A solution is prepared using 3.55 L of water and 2.10 mol solute. The total volume is 3.75 L. What is the molarity of the solute?

0.560 M

Calculate the molarity of 11.6 mL of a solution that contains 0.750 g CaCl2.

0.583 M

Calculate the molality (m) of the chloride ion (Cl-) in a 0.317 m aqueous solution of MgCl2

0.634 m

A 20.95 g sample of a substance is initially at 20.7 ºC. After absorbing 1343 J of heat, the temperature of the substance is 103.2 ºC. What is the specific heat of the substance?

0.7770 J/g•ºC

What concentration of Br- results when 799 mL of 0.709 M KBR is mixed with 743 mL of 0.539 M FeBr2?

0.887 M

Calculate the number of joules of heat required to raise the temperature of 123 g of iron from 14.7 ºC to 31.1 ºC. Does heating the iron take more energy or less energy than heating the same mass of water?

0.892 kJ Heating takes less energy than heating the same mass of water because the specific heat of iron is less than water's

Aluminum's molar heat capacity is 24.20 J/mol•K Convert the molar heat capacity of aluminum to the specific heat capacity of aluminum

0.8970 J/g•ºC

Calculate the concentration of each ion in a solution made by mixing 10.0 mL of 0.800 M (NH4)3PO4 with 14.9 mL of 1.44 M NH4Cl and diluting to 50.0 mL

0.910 M NH4+ 0.160 M (PO4)3- 0.430 M Cl-

Calculate the volume of 12.7 g of mercury (density = 13.53 g/mL)

0.939 mL

What are the values of each of the ​standard states - Pressure of gasses ______________ - Pressure and temperature of liquids and solids ____________ - Substance in solution (the molarity) ___________

1 atm 1 atm / 25ºC 1.0 M

Which is smaller: 10 µm or 10 nm?

1 µg = 10^-6 and 1 ng = 10^-9. 10 ng is smaller than 10 µg

Which statements are true? 1) Zn2+ is formed from the oxidation of Zn(s) 2) An oxidizing agent gains electrons 3) The oxidation number for Cu(s) is +2 4) The oxidation number for Hg(l) is 0 5) Na+ is formed from the reduction of Na(s) 6) A reducing agent gains electrons

1, 2, & 4

Jared becomes sick and needs to take an antibiotic. Dr. Iken prescribes him a medicine that requires 5.0 g/lb of his weight (every 6 hours). This medication has a density of 0.9799 g/mL, and Jared weighs 88.9 kg. How many mL of medicine does he need to take per dose (once every 6 hours)? (1 lb = 453.592 g)

1.0*10^3

Calculate the pressure at which oxygen has a density of 1.44 g/L at 22°C.

1.09 atm

Calculate the molarity of a solution containing 4.50 mmol NaCl in 3.80 mL of solution.

1.18 M NaCl

A sample of nitrogen gas occupies a volume of 0.325 L. What will the new volume be if the number of moles of N2(g) is increased from 0.225 to 0.866, with no change in temperature or pressure?

1.25 L

Determine the density of nitrogen gas at 0°C and 1.00 atm pressure.

1.25 g/L

A 1.45 L sample of argon gas has a pressure of 0.950 atm. What is its volume after its pressure is increased to 787 torr at constant temperature?

1.33 L

Calculate the final concentration after 87.3 mL of 1.71 M sugar solution is combined with 71.7 mL of 3.11 M sugar solution and the resulting solution is diluted to 275 mL.

1.35 M

A hot air balloon is filled with 1.13 * 10^6 L of an ideal gas on a cool morning (11ºC). The air is heated to 115 ºC. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon.

1.54 * 10^6 L

Diamond is another allotrope of carbon. If a 1-carat diamond has a mass of 0.200 g, how many moles of carbon is that?

1.67*10^-2 mol C

Calculate the enthalpy change for the combustion of 1.00 mol of butane (bottled gas), C4H10, to give carbon monoxide, CO, and water, H2O. Use the following equation: 2 C4H10(g)+9 O2(g)→8 CO(g)+10 H2O(l)

1.75 * 10^3 kJ

A 3.50 L sample of hydrogen gas has a pressure of 0.750 atm. What is its volume if its pressure is increased to 1.50 atm at constant temperature?

1.75 L

How many total atoms are there in 0.750 mol of hydrazine (N2H2)?

1.8*10^24

A weather balloon is filled with helium to a volume of 1.61 L at 734 torr. What is the volume of the balloon after it has been released and its pressure dropped to 0.844 atm. Assume that the temperature remains constant.

1.84 L

Calculate the pressure of 0.0789 mol of chlorine gas that occupies 891 mL at -15ºC.

1.88 atm

The wavelength of a dental X-ray is 0.10 nm. What is the energy of each X-ray photon (in J) emitted by the dental X-ray machine? Find the constants you need. Pay attention to unit!

1.99 * 10^-15 J

How many electrons in an atom can be described by the quantum numbers n=3 and l=2?

10

The element chlorine has ______ core electrons and _____ valence electrons

10, 7

An irregularly shaped piece of metal weighs 118 g . A graduated cylinder contains 30.0 mL of water initially. After the piece of metal is dropped into the graduated cylinder, it sinks to the bottom and becomes completely submerged under water. The water level in the graduated cylinder rises to 41.2 mL. The density of the metal is _________ g/cm3? Enter the numerical value without the unit. Round your answer to 3 significant figures.

10.5

A liquid solvent is added to a flask containing an insoluble solid. The total volume of the solid and liquid together is 85.0 mL. The liquid solvent has a mass of 26.5 g and a density of 0.865 g/mL. Determine the mass of the solid given its density is 2.00 g/mL

108.7 g

What volume is occupied by 0.447 mol of CO2 at 377.4 K and 959 mmHg?

11.0 L

A gas sample has a volume of 23.5 L at a temperature of 205 0C and a pressure of 1.35 atm. What is the final volume (in L) of the gas if the pressure increases to 2.84 atm and the temperature rises to 233 0C? Enter a numerical answer only without the unit.

11.8

Ethanol is a common laboratory solvent and has a density of 0.789 g/mL. What is the mass, in grams, of 145 mL of ethanol?

114.4 g

Your friend has a rectangular object which has a length of 4 cm, a width of 3 cm, and a 3​ height of 2 cm. This object's density is 4.90 g/cm​ . ​What is the mass of this object?

118 g

If 16 moles of NO combine with 29 moles of H2, how many moles of NH3 can form? 2NO(g) + 5H2(g) --> 2NH3(g) + 2H2O(g)

12 NH3 (H2 is limiting)

A sample of Br2(g) takes 24.0 min to effuse through a membrane. How long would it take the same number of moles of Ar(g) to effuse through the same membrane?

12 min

The element carbon has two naturally occurring isotopes. The isotopic masses and abundances of these isotopes are shown. Find the average atomic mass - 12C - Isotopic mass (u) 12.00, abundance (%) 98.93 - 13C - Isotopic mass (u) 13.00, abundance (%) 1.07

12.01 u

A student rents a car to drive from Laramie to Denver International airport. The trip is 151 miles according to the odometer. When he fills up the tank before returning the car, he found that he used 5.00 gallon of gas for the trip. What is the average gas mileage for the trip in km/L? 1 mile = 1.61 km. 1 gal = 3.78 L.

12.9 km/L

Antimony has two naturally occurring isotopes, 121Sb and 123Sb. 121Sb has an atomic mass of 120.9038 u, and 123Sb has an atomic mass of 122.9042 u. Antimony has an average atomic mass of 121.7601 u. What is the percent natural abundance of each?

121Sb = 57.194% 123Sb = 42.806%

When rounded to the proper number of sig figs, the answer of the following calculation is ________ which contains ________ sig figs. (1.7*10^6)/(2.63*10^5) + 7.338 =

13.8, 3

A pitcher throws a baseball with a mass of 5.13 oz (0.145 kg) at a velocity of 95.0 mph (42.5 m/s). Using the correct SI units, calculate the kinetic energy of the baseball.

131 kg • m^2/s^2 (J)

Given the following standard enthalpies of formation data: SiO2 (s)= -910.9 HCl (g) = -92.3 SiCl4 (g) =657.0 H2O (g) = -241.8 Calculate the ΔHºrxn for the following reaction: SiO2 (s) + 4 HCl (g) --> SiCl4 (g) + 2 H2O (g)

139.5 kJ

A 12 in. balloon holds ~ 15 L of helium at room temperature (25ºC). What will be the volume of the balloon if it is taken outside where the temperature is -1ºC. Assume the pressure is the same inside and outside.

15 L

HBr(aq) + NaHCO3(aq) --> NaBr(aq) + CO2(g) + H2O(l) Determine the mass of NaBr produced when the reaction of 25.0 g HBr with 12.3 g NaHCO3 is complete.

15.1 g NaBr

A piece of 4.50-g copper block at 25.0 °C is heated using a Bunsen burner. After it has absorbed 224 J of heat, the temperature of the copper is ________ °C. The specific heat capacity of copper is 0.38 J/(g•°C).

156

What is the molar mass of iron(III) oxide, a compound better known as rust?

159.69 g/mol

A 1.81 mol sample of Kr has a volume of 523 mL. How many moles of Kr are in a 4.68 L sample at the same temperature and pressure?

16.2 mol

Calculate the volume that 48.3 g of sulfur dioxide gas occupies at 0°C and 1.00 atm pressure.

16.9 L

Calculate the sum of 10.10 cm + 1.332 cm + 6.4 cm. Use the correct number of sig figs.

17.832 cm --> 17.8 cm

A pill contains 50.0 mg of a drug per pill. The drug is metabolized in the human body at a constant rate of 0.0236 oz/hr. If a patient ingests 4 pills, how long will it take for the drug to be completely metabolized in minutes? Report the answer in proper number of significant figures. 1 oz = 28.35 g.

17.9 minutes

Assuming an efficiency of 23.40%, calculate the actual yield of magnesium nitrate formed from 125.2 g of magnesium and excess copper(II) nitrate. Mg+Cu(NO3)2 --> Mg(NO3)2 + Cu

178.6g

What is the molar mass of caffeine, C8H10N4O2?

194.19 g/mol

Calculate the temperature at which oxygen has a density of 3.00 g/L at 1.50 atm.

195 K

How many cubic feet of cement can be held in a cement mixer with a capacity of 7.34 yd^3?

198ft^3

Give the first 11 subshells that electrons occupy in order of increasing energy:

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p

How many electrons in an atom can be described by the quantum numbers n=3, l=2, m(l)=-2?

2

Calculate the specific heat of ice if 128 J is required to raise the temperature of 4.00 g of ice by 15.3 ºC.

2.09 J/g•ºC

Burning 1.00 mol of diborane, B2H6, in excess oxygen in a constant-volume calorimeter warms 20.0 kg of water by 25.7 ºC. Calculate the heat produced in this combustion process: B2H6 (g) + 3O2 (g) --> B2O3 (s) + 3H2O (l)

2.15 * 10^3 kJ

A container measures 18.0 ft * 18.0 ft * 24.0 ft (W*L*H). What is the volume of the container in liter (L)? 1 ft = 30.5 cm

2.21*10^5 L

A standard 250-square-foot role of household kitchen aluminum foil weighs 102 g. How many aluminum atoms is that?

2.28*10^24 Al atoms

What is the partial pressure of compound C if compound A has a partial pressure of 0.329 atm, compound B has a partial pressure of 0.985 atm, compound D has a partial pressure of 0.756 atm and the total mixture has a partial pressure of 4.37 atm?

2.30 atm

3 Ba(s) + Al2O3(s) --> 3BaO(s) + 2Al(s) Calculate the number of individual atoms of barium metal that react when heated with excess aluminum oxide to form solid barium oxide and 7.33 g of aluminum.

2.45*10^23 Ba atoms

Consider a cloudless day on which the sun shines down across the United States. If 2681 kJ of energy reaches a square meter of the United States in one hour, how much total solar energy reaches the entire United States per hour? The entire area of the United States is 9,158,960 km^2.

2.455*10^6

2 NaOH(aq) + H2SO4(aq) --> Na2SO4(aq) + 2H2O (l) Calculate the number of formula units of NaOh that must reaction completely with H2SO4 to produce 1.24 * 10^15 formula units of Na2SO4.

2.48 * 10^15 formula units NaOH

A sample of helium gas initially occupies 35.0 mL at 1.50 atm. What needed to reduce its volume to 20.5 mL at constant temperature?

2.56 atm

Calculate the initial pressure of a 485 mL sample of helium gas that has been changed at constant temperature to 1.16 L and 1.18 atm.

2.82 atm

Calculate the relative effusion rates of helium and oxygen gases.

2.83

Many international computer communications are carried by optical fibers in cables laid along the ocean floor. In each cable, there are 6 strands of optical fibers. If 1 strand of optical fiber weighs 1.19 x 10-3 lb/m, what is the mass (in kg) of a cable long enough to link New York and Paris (8.84 x 103 km)? 1 kg = 2.2 lbs

2.87*10^4 kg

Calculate the wavelength (in m) of a radio signal with a frequency of 100.7 MHz.

2.98 m

Calculate the final temperature after 11.3 g of iron (c = 0.44 J/g • ºC) at 60.0 ºC is placed in 97.2 g of water at 19.0 ºC.

20 ºC

Calculate the final temperature after 6.80 g of aluminum (c = 0.892 J/g · °C) at 67.4°C is placed in 195 g of water at 19.6°C

20.0 ºC

Neon (Ne) has three naturally occurring stable isotopes. In a sample of neon, 90.92% of the atoms are Ne−20 (atomic mass: 19.99 amu). Another 0.3% of the atoms are Ne−21 (atomic mass: 20.99 amu). The final 8.85% of the atoms are Ne−22 (atomic mass: 21.99 amu). What is the atomic weight of neon?

20.18 amu

Neon (Ne) has three naturally occurring stable isotopes. In a sample of neon, 90.92% of the atoms are Ne─20, with an atomic mass of 19.99 amu. Another 0.3% of the atoms are Ne─21 with an atomic mass of 20.99 amu. The final 8.85% of the atoms are Ne─22, with an atomic mass of 21.99 amu. What is the atomic weight of neon?

20.18 amu

Calculate the volume of 0.898 mol methane gas (CH4) at 292 K and 1.06 atm.

20.3 L

One mole of gas will always equal _____________ L at STP regardless of the type of gas.

22.4

An average Iron Age sword weighed about 1.3 kg. How many moles of iron (Fe) are in an Iron Age sword that contains 1.3 kg of iron?

23 mol Fe

What amount of K​2O (in grams) would I need to make 2,760 mL of 0.89 M solution?

231.4g K2O

A gas cylinder that contains neon has an internal volume of 2.24 L. A pressure gauge attached to the cylinder reads 1850 psi (1 atm = 14.7 psi) at 22.4 ºC. What mass of neon is contained in the cylinder?

235 g

A sample containing 22.0 g of gaseous carbon dioxide occupies a volume of 15.3 L. What will the new volume be if an additional 15.0 g CO2(g) are added, with no change in temperature or pressure?

25.7 L

HNO3(aq) + Ba(OH)2(aq) --> Ba(NO3)2(aq) + H2O(l) Find the volume (in mL) of 0.5000 M HNO3 needed to react with 41.77 mL of 0.1603 M Ba(OH)2

26.78 mL HNO3

How many grams of NaNO3 is needed to prepare 250.0 mL of a 1.3 M NaNO3 solution?

27 g NaNO3

Rubidium (Rb) has two naturally occurring stable isotopes, Rb─85 (atomic mass: 84.912 amu) and Rb─87 (atomic mass: 86.909 amu). The atomic weight of rubidium is 85.468 amu. What is the percent abundance of Rb─87?

27.8%

Charlotte is driving at 50.8 mi/hr and receives a text message. She looks down at her phone and takes her eyes off the road for 3.67 s. How far has Charlotte traveled in feet during this time?

273.439 ft

In the combustion of hydrogen gas, hydrogen reacts with oxygen from the air to form water vapor. Hydrogen + oxygen --> water. If you burn 34.7 g of hydrogen and produce 3.10 * 10^2 g of water, how much oxygen reacted?

275.3 g

A gas cylinder is filled with argon at a pressure of 177 atm and 25 °C. What is the gas pressure when the temperature of the cylinder and its contents are heated to 195 °C.

277 atm

Given the following thermochemical equation, calculate the amount of heat (in kJ) that is released when 35.0 g of Na2O2 completely react with excess amount of water . 2 Na2O2 (s) + 2 H2O (l) → 4 NaOH (aq) + O2 (g) Δ H = - 126 kJ

28.3 kJ

Calculate the molar mass of a gas if a 3.38 g sample occupies 2.76 L at 22 ºC and 793 torr.

28.4 g/mol

A 31.1-g wafer of pure gold at 69.3 °C is submerged into 64.2 g of water at 27.8 °C in a well-insulated container. Assume no heat is lost to the air and no work is done during the process. What is the final temperature inside the container at thermal equilibrium? The specific heat capacity for Au and water is 0.128 J/(g∙°C) and 4.184 J/(g∙°C), respectively.

28.4ºC

Calculate the liters of Methane at STP required to form 47.2 g of water. CH4​ + 2 O​2 → CO​2 + 2 H​2O

29.3 L

Balance NH4I+Pb(NO3)2 --> NH4NO3+PbI2

2NH4I+Pb(NO3)2 --> 2NH4NO3 + PbI2

Which subshell is designated by each set of quantum numbers? n=2, l=0 n=4, l=1 n=5, l=1 n=3, l=1

2s 4p 5p 3p

What is the quantum numbers of the 14th electron in the ground-state electron configuration of a phosphorus (P) atom? Enter "one half" as 1/2. Principal quantum number _____ angular momentum quantum number ______ magnetic quantum number ______ electron spin quantum number _____

3, 1, 0, 1/2

Any p subshell contains _____ atomic orbitals and can hold a maximum of _______ electrons.

3, 6

How many grams of sodium hydroxide are present in 250.0 mL of a 0.300 M NaOH solution?

3.00 grams

Phosphine (PH3) was recently detected in the atmosphere of Venus, which was cited as evidence that some kind of life form might exist on Venus. What is the total number of atoms in a sample of 4.50 g of PH3?

3.19 x 10^23

Calculate and compare the energy of a photon of wavelength 3.3 µm with that of wavelength 0.154 nm.

3.3 µm = 6.0 * 10^-20 J 0.154 nm = 1.29 * 10^-15 J

Determine the density of SO3 at 25 ºC and 789 torr.

3.40 g/L

Calculate the final pressure of a sample of helium gas that has an initial volume of 8.35 L at 10 ºC and 1.13 atm pressure if the number of moles doubles and the volume is changed to 5.25 L with no changed in temperature.

3.59 atm

Calculate the relative effusion rates of hydrogen and carbon monoxide gases.

3.73

Convert the given lengths from the derived units to meters 0.389 mm 529 Mm 92.9 km

3.89 * 10^-4 5.29 * 10^8 9.29 * 10^4

If 2.30 mol of a gas occupies 50.5 mL how many moles of the gas will occupy 85.5 mL at the same temperature and pressure?

3.89 mol

Perform the calculation and report using the correct number of sig figs (1.012*10^-3 J)/(0.022456g)(298.3682-298.3567)K =

3.92 J/gK

Suppose that you go on a road trip where your car averages a fuel economy of 37.2 mpg for 65% of the trip, 24.2 mpg for 23% of the trip, and 8.8 mpg for 12% of the trip. Determine the car's average fuel economy for the trip.

30.8 mpg

A reaction forms a gas at 32.0ºC. Report this value using the temperature scale required for gas law calculations

305.15 K

Calculate the pressure of 0.0855 mol neon gas if it occupies mL at 25 ºC.

31.6 atm

While driving your rental char on your vacation in Europe, you find that you are getting 13.5 km/L of gasoline . What does this value correspond to in miles per gallon?

31.75 mi/gal

Based on the subshells that make up the fourth principal energy level, what is the maximum number of electrons the fourth principle energy level can hold?

32 electrons

Calculate the volume of 42.6 g of oxygen gas at 35°C and 792 torr.

32.3 L

At 1.43 atm and 13.04 ºC, a 3.07 g sample of gas occupies a volume of 1560 mL. Calculate the molar mass of the gas.

32.3 g/mol

A hot lump of 38.2 g of aluminum at an initial temperature of 90.5 ºC is placed in 50.0 mL H2O initially at 25.0 ºC and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given the the specific heat of aluminum is 0.903 J/(g*ºC)? Assume no heat is lost to surroundings.

34.3 ºC

A hot lump of 38.2 g of aluminum at an initial temperature of 90.5 ºC is placed 50.0 mL H2O initially at 25.0 ºC and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/g•ºC?

34.3ºC

Calculate the volume of 1.63 mol carbon dioxide gas at 295 K and 1.14 atm.

34.6 L

A sample of Freon-12 (CF2Cl2) occupies 25.5 L at 298 K and 153.3 kPa. Find its volume at STP. 1 atm = 101.325 kPa.

35.3 L

Convert 177.8 ºF to kelvins

354.15 K

If 100.0 grams of carbon is converted to carbon dioxide gas, how many grams of CO2 would be formed?

366.4g CO2

Table sugar melts at 186ºC. What is the melting point of sugar in ºF?

367ºF

What is 98.6ºF on the Celsius scale?

37.0ºC

Benzoic acid, C7H6O2, occurs naturally in many berries. A 1.50-g sample of benzoic acid is combusted in a bomb calorimeter. The temperature of the calorimeter increases from 22.50 ºC to 31.69 ºC. The calorimeter contains 775 g water and has a heat capacity of 893 J/ºC. Based on this information, how much energy (in kJ) is released when you metabolize 1.50 g of benzoic acid? The specific heat capacity of water is 4.184 J/(g⋅ºC).

38.0 kJ

How many grams of Ni are formed from 53.8 g of Ni2O3? 2Ni2O3(s) --> 4Ni(s) + 3O2(g)

38.2 g Ni

Naturally occurring potassium consists of the following isotopes in the percentages listed: 39K: 38.9637 u (93.258%) 40K: 39.9640 u (0.0117%) 41K: 40.9618 u (6.7302%) What is the atomic mass of potassium?

39.0983 u

When methanol, CH3OH, is burned in the presence of oxygen gas, O2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation. CH3OH(g) + 3/2O2(g) --> CO2(g) + 2H2O(l). ∆H = -764 kJ How much methanol, in grams, must be burned to produce 935 kJ of heat?

39.2 g

If the first two quantum numbers for an electron are n = 3 and ℓ = 2, which energy level and subshell does that electron occupy?

3d

Identify the exact numbers: - 3 lbs (weight of an object measured on a scale) - 56.00 s (a time measured by a stopwatch) - 4 choices (the number of choices in this list) - 2.54 cm (the number of centimeters in exactly 1 in)

4 choices & 2.54 cm

For a 4f subshell, the principal quantum number, n = _____; the angular momentum quantum number l = _____.

4, 3

If you want to prepare 500 mL of 0.100 M HNO3 solution, how many mLs of the concentrated HNO3 solution (12 M) do you need?

4.2 mL

Calculate the pressure required to change a 3.38 L sample of neon gas initially at 1.15 atm to 925 mL, at constant temperature.

4.20 atm

The volume of a sample of gas is measured as 4227.9 cm^3. Convert the volume to cubic meters

4.2279*10^-3

How many photons are produced in a laser pulse of 0.159 J at 591 nm?

4.72 * 10^17

Carry out the given conversions from one metric unit to another 0.483 µL --> mL 48.7 km --> dm

4.83 * 10^-4 mL 4.87 * 10^5 dm

Calculate the kinetic energy of a 1.95*10^5 kg locomotive that is traveling at 22.4 m/s.

4.89 * 10^7 J

Lithium has a work function equal to 4.65 * 10^-19 J. If a violet photon wavelength of 405 nm impacts a lithium surface in a vacuum, will an electron be ejected?

4.91 * 10^-19 J

One tablespoon of cookie dough has a mass of 13.19 g. It is combusted in a calorimeter whose heat capacity is 72.25 kJ/ºC. The temperature of the calorimeter rises from 21.03 ºC to 24.79 ºC. Find the food caloric content of the cookie dough in Calories per gram

4.923 Cal/g

Determine the molar mass of an unknown gas if a sample of this gas weighing 0.389 g is collected in a flask with a volume of 218 mL at STP. The universal gas constant R = 0.0821 (atm⋅L)/(mol⋅K)

40.0 g/mol

Hot air balloons heated by candles were used in the 3rd century for military signaling purpose. A hot air balloon is heated to 200ºC and inflated to 32.5 L under a pressure of 0.978 atm. It cools down to 150ºC when it rises to an altitude where the pressure is 0.693 atm. What is the final volume (in L) of the balloon?

41.0 L

Calculate the wavelength of light that corresponds to a frequency of 7.30 × 1014 per second. Report your answer in units of nanometers (1 m=1×109 nm).

411 nm

Calculate the volume of a sample of hydrogen gas that occupies 575 mL at 737 torr and 22 ºC if its temperature and pressure are changed to 85 ºC and 1.55 atm, respectively.

437 mL

What is the volume of a sample of neon gas at 0ºC and 760 torr pressure if it has a volume of 49.7 mL at 52 ºC and 811 torr?

44.5 mL

Calculate the final temperature after 1485 J of energy is added to 16.7 g of water at 23.4°C.

44.7 ºC

What is the average atomic mass of titanium according to these values? - 46Ti - 73.000% - 45.95263 u - 48Ti - 12.200% - 47.94795 u - 50Ti - 14.800% - 49.94479 u

46.787 u

A silver medal from the 2016 Olympics weighs 500 g and contains 4.29 mol of silver of gold. How many grams of pure silver were used to make each of these medals?

463 g Ag

The surface temperature on Venus may approach 749 K. What is this temperature in degrees Celsius?

475.85 ºC

What color is a photon that has an energy of 4/01 * 10^-19 J?

496 nm --> green to blue-green

The shubshell to be occupied after the 3p subshell is the _______ subshell; the subshell to be occupied after the 4d subshell is the _______ subshell.

4s, 5p

How many moles of ammonium ions are required to produce 250 g of solid ammonium phosphate?

5.0 mol NH4+

What is the frequency of light in Hz that absorbs a wavelength of 578 nm? What color of light​ does this represent?

5.19 * 10^14 Hz (green-yellow)

3.76 g of Mg burns with 9.01 g O2 2Mg(s) + O2(g) --> 2MgO(s) The reaction goes to completion, but in the process some of it was lost. The percent yield for the reaction is 86.1%. How many grams of product are recovered? How many grams of the excess reactant remain?

5.37 g MgO 6.54 O2

At constant volume, the heat of combustion of a particular compound, compound A, is -3110.0 kJ/mol. When 1.1417 g of compound A (molar mass = 108.29 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 7.525 ºC. What is the heat capacity (calorimeter constant) of the calorimeter?

5.410 kJ/ºC

What is the volume of 8.0 g of O2 (behaving as an ideal gas) at STP? At STP, 1 mol of any ideal gas occupies a volume of 22.4 L.

5.6 L

According to a 2016 estimate by the Environmental Protection Agency, the average passenger car in the United States emits 9.34 mol of CO2 gas per mile driven. Based on this value, how many carbon atoms and how many oxygen atoms are in the CO2 emissions of a car making a 1 mi drive?

5.62*10^24 C & 1.12*10^25 O

Silver has two naturally occurring isotopes: 107Ag (atomic mass: 106.91) and 109Ag (atomic mass: 108.90 amu). The atomic weight of silver is 107.87 amu. What is the percent abundance of the lighter isotope of silver?

51.2 %

A sample of H2 gas is placed in a sealed container at 25ºC and has a pressure of 500 torr. If the gas is heated and reach a pressure of 1.75 atm, what is the temperature (in ºC) of the gas?

520. ºC

Using the root mean square velocity, find the average velocity of gaseous Li atoms at 76K. (1 J= kg*m​^2/s​^2)

523 m/s

Sodium metal has a work function equal to 3.78 × 10-19 J. What minimum frequency of light is necessary to remove a surface electron from sodium? To what wavelength of light (in nm) does this correspond?

526 nm

The pressure of a nitrogen gas sample of unknown volume was changed from 1.20 atm to 744 tor at constant temperature, resulting in a volume of 70.4 mL. What was its initial volume?

57.4 mL

If 6.35 g of CuNO3 is dissolved in water to make a 0.860 M solution, what is the volume of the solution in milliliters?

58.8 mL

What is the valence electron configuration of Tellurium (atomic number 52)?

5s^25p^4

The answer with proper number of significant figures for the following calculation is ______. (2.648/0.87) x (84-81.98) = 6.1482299

6

Specify the number of valence electrons each of the following atoms has. Each sulfur (S) atom has ______ valence electrons; Each xenon (Xe) atom has _______ valence electrons; Each phosphorus (P) atom has ______ valence electrons.

6, 8, 5

A gold medal from the 2016 Olympics weighs 500 g and contains 0.0305 mol of gold. How many grams of pure gold were used to make each of these medals?

6.01 g Au

Calculate the final temperature after 987 J of energy is removed from 14.9 g of water at 22.0 ºC.

6.2 ºC

A liquid has a volume of 0.0069 L. Convert this volume to cubic centimeters.

6.9 cm^3

If the moles of gas and pressure remain constant, what would the final temperature be if a bucket of gas particles has an initial volume of 22.5 mL, an initial temperature of 75 K, and a final volume of 18.6 mL?

62 K

A 93 g sample of a pure gaseous substance occupies 29.5 L at 27°C and 1.25 atm. What is the molar mass of the gas?

62 g/mol

A gas-filled weather balloon with a volume of 57.0 L is held at ground level, where the atmospheric pressure is 771 mmHg and the temperature is 21.7 ºC. The balloon is released and rises to an altitude where the pressure is 0.0832 bar and the temperature is -6.30 ºC. Calculate the weather balloon's volume at the higher altitude.

635 L

How many grams of Br2 are needed to form 72.1 g of AlBr3? 2Al(s) + 3 Br2(l) --> 2AlBr3(s)

64.8 g Br2

Calculate the wavelength of red light (in nm) with a frequency of 4.62 * 10^14 Hz

649 nm

A naturally occurring sample of an element contains only two isotopes. The first isotope has a mass of 68.9255 amu and a natural abundance of 60.11%. The second isotope has a mass of 70.9247 amu. Find the atomic weight of the element.

69.72 amu

What is the next subshell to be occupied after the 5p subshell?

6s

A teaspoon of sugar is about 0.0123 mol of sucrose, C12H22O11. how many C12H22O11 molecules are in a teaspoon of sugar?

7.41 *10^21 molecules of C12H22O11

At STP, 10.5 g of a gas occupies a volume of 3.32 L. What is the molar mass of the gas? Enter the numerical answer without the unit. Round your answer to 3 significant figures.

70.9

A group of architects are designing a whale shaped gas tank to hold their carbon monoxide molecules so that no one dies. Currently, it has a volume of 4.56 L. The pressure is 3.4 atm. If the architects want the tank to have a pressure of 2.2 atm, what size does the tank need to be in mL?

7047 mL

N2(g) + 3H2(g) --> 2NH3(g) Suppose that 4.80 g of ammonia is formed by the reaction of 5.50 g N2 with 1.50 g H2. Determine the percent yield of ammonia.

71.7%

2 CH3OH(g) + 3O2(g) --> 2CO2(g) + 4H2O(l) ∆Hrxn = -1452 kJ Given the thermochemical equation of the combustion above, we know that when 1 mol of CH3OH is burned, _____ of energy is ________.

726 kJ, released

The initial volume of water in a graduated cylinder is 30.0 mL. A 121.5-g piece of aluminum cube is dropped into the graduate cylinder and become completely submerged under water. What is the volume reading after the aluminum cube is dropped into the graduated cylinder? The density of aluminum is 2.70 g/cm^3

75.0 mL

C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(g) Calculate the volume of liquid water (density 1.00 g/mL) produced by burning 48.4 g of propane and condensing the gaseous water produced. Assume lots of O2

79.1 mL H2O

Element 113 (official symbol, Nh) is one of the last 4 elements to be formally named. What is the valence electron configuration of Nh?

7s2 7p1

The industrial process for the production of sodium metal and chlorine gas involves the electrolysis of molten (melted) sodium chloride in the absence of water. Calculate the mass of sodium in grams that can be prepared by the electrolysis of 207 kg of sodium chloride. 2 NaCl(l) ---> 2Na(l) + Cl2(g)

8.14*10^4 g Na

Calculate the number of joules of heat required to raise the temperature of 123 g of water from 14.7°C to 31.1°C.

8.44 kJ

Calculate the final volume of a sample of hydrogen gas that has an initial volume of 7.10 L at 0°C and 760 torr pressure, if the temperature and pressure are changed to 33°C and 696 torr, respectively.

8.7 L

Using the ∆Hºf values, calculate the ∆Hºrxn of the following reaction: 2CuO(s) + NO(g) --> Cu2O(s) + NO2(g) CuO = -156.1 NO = 90.37 Cu2O = -170.7 NO2 = 33.84

84.93 kJ

A sample of 50.8 g of tetraphosphorous decoxide (P4O10) reacts with 84.2 g of water. Calculate the percent yield of H3PO4 if 60.1 g H3PO4 is isolated after the reaction P4O10 + 6H2O --> 4H3PO4

85.7 %

In 1997, carbon monoxide (CO) level in the air in Los Angeles reached 15.0 ppm (v/v). An average human inhales about 0.50 L of air per breath and takes about 20.0 breaths per minute. How many milligrams of carbon monoxide would a person inhale in exactly 8 hours under those conditions? Assume CO has a density of 1.2 g/L. (Note: 15.0 ppm CO means 15.0 L CO per 106 L air).

86 mg of CO per 8 hours

Consider the following reaction: 2 Mg (s) + O2 (g) --> 2 MgO (s) Δ𝐻=−1204𝑘𝐽ΔH=−1204kJΔ𝐻=−1204𝑘𝐽ΔH=−1204kJ Calculate the amount of heat transferred when 3.55 g of Mg (s) reacts with excess amount of O2 under constant pressure.

87.9 kJ

A 678 mL sample of helium gas, initially at 0°C, is heated at constant pressure. If the final volume of the gas is 0.896 L, what is its final temperature in °C?

88 ºC

Burning 1.00 mol of CH4 in a calorimeter warms 10.0 kg of water by 21.3°C. Calculate the heat produced in this combustion process: CH4(g)+2 O2(g)→CO2(g)+2 H2O(l)

891 kJ

The "lead" in a pencil is actually graphite, an allotrope of carbon. If the graphite in a pencil weighs 1.09 g, how many moles of carbon is that?

9.08*10^-2 mol C

Convert 3.49 cm^3 to gallons

9.219*10^-4 gal

The active ingredient in aspirin is acetylsalicylic acid, HC9H7O4. A regular-strength aspirin tablet contains 1.80 * 10^-2 mole HC9H7O4. How many carbon, hydrogen, and oxygen atoms are in the active ingredient of a regular-strength aspirin tablet?

9.76*10^21 C 8.67*10^21 H 4.34*10^21 O

When methanol, CH3OH, is burned in the presence of oxygen gas, O2, a large amount of heat energy is released, as shown in the combustion reaction. CH3OH(g) + 3/2O2 (g) --> CO2(g) + 2H2O(l). ∆H = -764kJ Based on the balanced thermochemical reaction, how much heat is produced when 38.5 g of methanol reacts with 59.7 g of oxygen?

918 kJ (methanol is limiting reactant)

- In a bomb calorimeter, a certain amount of methane (CH​ ) undergoes combustion. The 4​ temperature starts at 67.9 °C. The q​(cal) = 122kJ. Find the final temperature of the calcium in the​ bomb calorimeter. (The heat capacity of the bomb calorimeter is 4.90 kJ/°C ). - If the q​(cal) =122 kJ, what is the q​(rxn)? - If 2.33 g of methane was combusted, what was the change in energy of the combustion in kJ/mol. Was this heat released or absorbed? (ΔE = q​ rxn/ mol) ​

92.8 ºC 122.104 kJ -842.09 kJ/mol

Calculate the volume of a sample of hydrogen gas that originally occupies 908 mL at 717 torr and 20°C after its temperature and pressure are changed to 72°C and 1.07 atm, respectively.

943 mL

Calculate the answer to the proper precision: 62.44 cm - 7.145 cm + 27.7 cm

= 82.995 cm --> 83.0 cm

For an ideal gas, which of the following is inversely proportional to each other? a) pressure and volume b) volume and amount of gas c) pressure and temperature d) volume and temperature

A

What is the valence electron configuration of Group 6A elements? a) ns2np4 b) ns2np6 c) ns6 d) np6

A

Which gas molecules have the highest average kinetic energy at a given temperature? a) They all have the same average kinetic energy b) HCl c) NO d) SO2

A

Which of the statements is true of an exothermic reaction? a) Weak bonds break and strong bonds form b) The bonds that break and those that are formed are of approximately the same strength c) Strong bonds break and weak bonds form

A

Which of the statements is true of the energies of the bonds that break and form in an exothermic reaction? a) The energy required to break the necessary bonds is less than the energy released when new bonds form. b) The energy required to break the necessary bonds is greater than the energy released when the new bonds form. c) The energy required to break the necessary bonds is about the same as the energy released when the new bonds form.

A

What is a calorie vs a Calorie?

A calorie is the amount of energy needed to raise 1 gram of water by 1 ºC (4.184 Joules) and a Calorie is 1000 calories (4184 Joules)

A sample of a shiny substance is heated in air, yielding a white powder with twice the mass. Is the change a chemical reaction? Is the powder an element?

A chemical reaction takes place, creating a new substance with definite properties of its own. The powder is not an element; it is a compound

Classify the substances represented by the following microscopic representations as either element, compound, or mixture.

A) Compound B) Element C) Mixture D) Mixture (I think)

Classify the compounds as acids, bases, or salts. - H2C2O4 - KOH - HClO4 - NH4Br - CaCl2 - Ca(OH)2 - HI - KI

Acids: HI, H2C2O4, & HClO4 Base: Ca(OH)2, KOH Salts: NH4Br, KI, CaCl2

What is the Arrhenius definition of an acid and a base?

Acids: Substances that dissociate to produce H+ when dissolved in water (H+ actually exist as H3O+ in water) Bases: Substance that contain OH & produce OH- when dissolved in water

What is the charge of a silver ion?

Ag+

Two different gases are separated by a valve. The volume of gas 1 is V1. The volume of gas 2 is V2. After the valve is open, which of the following is true? I. Gas 1 will diffuse to the right and mix with gas 2 II. Gas 2 will diffuse to the left and mix with gas 1 III. The final volumes of gas 1 and gas 2 will both equal to V1 + V2

All are true

Indicate whether each of the following chemical formulas is a valid empirical formula. If not, determine the correct empirical formula for that compound. a) BO1.5 b) C6H6 c) Na0.5P0.25O d) C3H2.67O1.33

All invalid a) Multiply by two to get a whole number - B2O3 b) Lowest whole number ratio - CH c) Multiply by four to get whole numbers - Na2PO4 d) Multiple by three to get whole numbers - C9H8O4

What type of particles were shot at the gold foil? - Alpha particles - Gold nuclei - Gold atoms - Beta particles - Cathode rays (electrons)

Alpha particles

At a given temperature, nitrogen gas effuses approximately 1.2 times faster than which of the following gases?

Argon

What is the general periodic trend of atomic radius going from left to right across a period? Explain your reasoning.

Atomic radius decreases going from left to right across a period. C and F is an example. The valence electrons of the elements in the same period are in the same electron shell. But the effective nuclear charge / core charge increases going from left to right across a period, making the size of the atom smaller.

What is the general periodic trend of atomic radius going down a group? Explain your reasoning.

Atomic radius increases going down a group. This is because an additional electron shell is occupied by electron(s) every time we move to a new period.

What is the Nuclear Atomic Model?

Atoms are composed of protons (p+), electrons (e-), and neutrons (n0) Nucleus - Contains all the p+ & n0 of an atom - Most of the mass - Small fraction of the volume - Each p+ has +1 charge - n0 has no charge Electrons - e- surround the nucleus - Much lighter than p+ & n0 - Occupies most of the volume - e- has a charge of -1 Atoms are neutral --> number of e- = number of p+

What did the discovery of electrons do for the atomic model?

Atoms must not be an indivisible ball --> made the plum pudding model. Found by JJ Thompson with the "cathode ray" which was emitted by most atoms

What was the billiard ball model?

Atoms seen as indivisible balls that reacted with one another (Dalton)

At 25ºC, the rate of effusion of an unknown gas is twice as fast as SO2 (MM = 64.0 g/mol). This gas could be: a) He (MM = 4.00 g/mol) b) CH4 (MM = 16.0 g/mol) c) O2 (MM = 32.0 g/mol) d) HI (MM = 128 g/mol)

B

What does 2p designate? a) an electron shell b) a subshell c) an atomic orbital d) B & C e) all

B

Identify all allowable combinations of quantum numbers for an electron: a) n = 3, l = -2, m(l) = 2, m(s) = 1/2 b) n = 3, l = 2, m(l) = 2, m(s) = 1/2 c) n = 5, l = 4, m(l) = -3, m(s) = 1/2 d) n = 3, l = 3, m(l) = -1, m(s) = -1/2 e) n = 4, l = 2 m(l) = 3, m(s) = -1/2 f) n = 2, l = 1, m(l) = 1, m(s) = -1

B & C

Predict where the largest jump between successive ionization energies occurs for K.

Between the first and second ionization energies

Predict where the largest jump between successive ionization energies occurs for Be.

Between the second and third ionization energies

Which of the following statements are TRUE? I. For a gas sample at a constant temperature, increased volume leads to lower pressure. II. For a gas sample in a container with a fixed volume, higher temperature leads to a higher pressure.

Both

The density of copper decreases with increasing temperature (as does the density of most substances). Which statement about raising temperature of a copper sample from room temperature to 95ºC is true? a) The copper sample contracts b) The copper sample becomes heavier c) The copper sample expands d) The copper sample becomes lighter

C

What does 3d(xy) designate? a) an electron shell b) a subshell c) an atomic orbital d) B & C e) All

C

Which of the following bonds would you expect to be the most polar? a) O-F b) C-N c) C-O d) P-S e) N-O

C

With regard to M1V1 = M2V2 which of the expressions is equal to the volume of stock solution V1? a) (M1M2)/V2 b) (M2V1/M1) c) (M2V2/M1)

C

Naphthalene is a white solid that consists only of carbon and hydrogen. It was once used as the active ingredient in mothballs. When combustion analysis was carried out on a 5.00 g sample of naphthalene, 17.17 g CO2 and 2.81 g H2O were produced. If the molar mass of naphthalene is 128.17 g/mol, what is the molecular formula of naphthalene?

C10H8

Naphthalene is a white solid that consists only of carbon and hydrogen. It was once used as the active ingredient in mothballs. When combustion analysis was carried out on a 5.00 g sample of naphthalene, 17.17 g CO2and 2.81 g H2O were produced. If the molar mass of naphthalene is 128.17 g/mol, what is the molecular formula of naphthalene?

C10H8

Calculate the empirical formula of each of the substances from the following analyses: a) 5.52 g C, 0.464 g H, 13.1 g F b) 75.95 g C, 9.57 g H, 224.2 g Cl

C2H2F3 C2H3Cl2

A 72.33 g sample of a compound contains 28.90 g of carbon, 4.86 g of hydrogen, and 38.57 g oxygen. If the molar mass of the compound is 60.05 g/mol, then what is its molecular formula?

C2H4O2

The most widely used antifreeze, ethylene glycol, is composed of 38.70% carbon, 9.74% hydrogen, and 51.56% oxygen. Its molar mass is 62.07 g/mol. Find its molecular formula.

C2H6O2

A 0.2684g sample of a compound containing only C,H, and O was burned and 0.480 g of CO​2​ and 0.1964 g of H​2​O were isolated. In a separate experiment the molar mass of the compound was found to be 148.2 g/mol. Find the empirical formula and the molecular formula of the compound. (Hint: what are the masses of C, H, and O)

C3H6O C6H12O2

Rotting animal tissue such as road kill produces a foul-smelling compound commonly known as cadaverine. Cadaverine contains C, H, & N only. When combustion analysis was carried out on a 3.75 g sample of cadaverine, 8.08 g CO2 and 4.63 g H2O were produced. If the molar mass of cadaverine is 102.18 g/mol, what is the molecular formula of cadaverine?

C5H14N2

Determine the empirical formula for a compound that is 76.6% C, 6.4% H, and 17.0% O by mass.

C6H6O

Determine the molecular formula of hydrocarbon, a compound made up of only carbon and hydrogen, which contains 89.94% carbon and has a molar mass of 80.2 g/mol.

C6H8

Butyl butyrate, which contains C, H, and O only, is a naturally occurring compound found in many different kinds of fruit, including apples, bananas, melons, cherries, and strawberries. It is added as an artificial flavoring to some foods and drinks to create sweet, fruity flavors. When combustion analysis was carried out on a 2.50 g sample of butyl butyrate, 6.10 g CO2 and 2.50 g H2O were produced. If the molar mass of butyl butyrate is 144.21 g/mol, what is the molecular formula of butyl butyrate?

C8H16O2

The octane rating on a gas pump is a measure of how efficiently that fuel burns compared with pure 2,2,4-trimethylpentane, a liquid compound that consists entirely of carbon and hydrogen. When combustion analysis was carried out on a 1.75 g sample fo 2,2,4-trimethylpentane, 5.39 g CO2 and 2.48g H2O were produced. If the molar mass of 2,2,4-trimethylpentane is 114.23 g/mol, what is the molecular formula of it?

C8H18

Octane and heptane are two ingredients of gasoline. Octane has 84.12% carbon and 15.88% hydrogen, and heptane has 83.90% carbon and 16.10% hydrogen. Their molecular masses are 114 u and 100 u, respectively. What are their molecular formulas?

C8H18 C7H16

Styrene, used in manufacturing Styrofoam™ and polystyrene packaging, is composed of 92.26% carbon and 7.74% hydrogen. Determine its empirical formula.

CH

In "The Empire Strikes Back," Han Solo is frozen in a fictional substance called "carbonite." If carbonite existed and was named systematically as an oxyanion, what would its formula be?

CO2 (2-)

Determine the formula of the ionic compound formed from calcium and oxygen

CaO

A sample of sulfur dioxide, SO2, consists of 16.04 g of sulfur and 16.00 g of oxygen, whereas a sample of sulfur trioxide, SO3, consists of 16.04 g of sulfur and 24.00 g of oxygen. Show that SO2 and SO3 follow the law of multiple proportions

Calculate the sulfur-to-oxygen ratios for both: SO2 (16.04 g S/16.00 g O) = 1.003 SO3 (16.04 g S/24.00 g O) = 0.6683 The S:O mass ratios can be compared now, divide the larger value by the smaller value: (1.003/0.6683) =1.501 Multiplying 1.501 by two gives a ratio of 3.002. The ratio of S:O mass ratios for these compounds is a whole number, 3, so SO2 and SO3 follow the law of multiple proportions

Explain the difference between a cation and an anion

Cation = positive (lost electrons) Anion = negative (gain electrons)

What did the discovery of radioactivity do for the advancement of the atomic model?

Challenged the idea that atoms are indivisible

Describe the difference between chemical and physical changes

Chemical (chemical reaction) --> Results in a change in the substance Physical --> Substance remains the same

Name the cation in CrCl2

Chromium (II) ion

What is oxidized and reduced in the following redox reaction? Cu (s) + 4 HNO3 (aq) → Cu(NO3)2 (aq) + 2 H2O (l) + 2 NO2 (g)

Cu is oxidized (0 --> +2), HNO3 is reduced (+5 --> +4)

What is the formula for copper(II) phosphate and how many atoms of phosphorus are in 4.20 mol of it?

Cu3(PO4)2 - 5.06*10^24

Identify the unbalanced half-reaction in which a species is reduced: a) Cr2O3(s) --> (CrO4)2- (aq) b) Al(s) --> Al3+ (aq) c) 2I- (aq) --> I2 (s) d) (SO4)2-(aq) --> H2S(g) e) C(s) --> CO(g)

D

What does 2s designate? a) an electron shell b) a subshell c) an atomic orbital d) B & C e ) all

D

The law of _______________ states that a compound always contains the same elements in the same proportion as mass.

Definite proportions

Calculate the density of a rectangular metal bar that is 7.00 cm long, 4.00 cm wide, and 1.00 cm thick and has a mass of 220.0 g. Identify the metal

Density = 7.86 g/mL which is likely iron

What did Robert Millikan's oil drop experiment do for the advancement of the atomic model?

Determined the electrical charge of an electron

What did the discovery of radioactivity do for the atomic model?

Discovered that there are probably subatomic particles (positively, negatively, and no charge). Found by Marie Curie and Henri Becquerel.

Classify each as electrolytes or nonelectrolytes: - NaBr - C4H8O4 - LiOH - HNO3

Electrolyte: HNO3, NaBr, & LiOH Nonelectrolyte: C4H8O4

For elements, compounds, and mixtures explain the type of atoms/element (how many), the number of substances, and if it's a pure substance.

Element: 1, 1, yes Compound: ≥2, 1, yes Mixture: ≥2, multiple, no

What did the discovery of the proton do for the atomic model?

Ernest Rutherford found that alpha particles occasionally reflected when hitting atoms implying a positively charged mass --> protons in nucleus

Who performed this experiment? - Robert Millikan & Harvey Fletcher - J.J. Thompson - Ernest Rutherford, Hans Geiger, and Ernest Marsden - Niels Bohr

Ernest Rutherford, Hans Geiger, and Ernest Marsden

The specific heat capacities for several substances are listed here: (J/g•ºC) - copper - 0.39 - air - 1.01 - ethanol - 2.44 - concrete - 0.88 If there are equal masses of each substance, which substance must absorb the greatest amount of heat to increase the temperature by the same amount?

Ethanol

The combustion of acetylene is shown below 2C​2​H​2​ (g) + 5O​2​ (g) → 4CO​2​ (g) + 2H​2​O(g) ΔH= - 1299kJ Is this reaction endothermic or exothermic?How much heat is released or absorbed by the reaction of 876.9 g of acetylene?

Exothermic, -21870 kJ

Identify the elements that are diatomic - Na, F, As, Kr, I, H, U, O, Fe

F, I, H, O

Select true or false for these statements about resonance structures: - The actual structure of formate switches back and forth between the two resonance forms - Each resonance bond is somewhere between a single and a double bond (ex CHO2) - Each resonance bond has a double bond 50% of the time - The actual structure of formate is an average of the two resonance forms

F, T, F, T

What is the charge on each cation in the following compounds? a) FeCl3 b) SnO2

Fe 3+ Sn +4

What is the chemical formula for the compound formed between: - iron(III) and the nitrate ion - iron(II) and the borate ion

Fe(NO3)3 FeBO3

A 360.0 g sample of a compound contains 12.78 g of nitrogen and 347.2 g of iodine. The molar mass of the compound is 394.7 g/mol. What is the molecular formula for the compound?

Find the empirical formula = NI3 Given molar mass / empirical's molar mass = 1 so it's the same as the empirical

Which of these mixtures are heterogeneous? - Granite (a type of rock with multicolor spots) - Brass (an alloy of copper and zinc) - Salt and water - Oil and water

Granite & oil and water

An unknown gas and CH​ 4 gas are in a beaker together. If the unknown gas effuses at a rate 3.99 times faster than methane, what is the identity of the unknown gas?

H

What is the molar mass of acetic acid, HC2H3O2, the acid found in vinegar?

H - 4.032 g/mol C - 24.022 g/mol O - 31.998 g/mol 1 mol of acetic acid = 60.052 g/mol

Write the names and symbols of elements 1-20 & label them as metals(m), nonmentals(nm), or metalloids(ml)

H-Hydrogen (nm), He-Helium (nm), Li-Lithium (m), Be-Beryllium (m), B-Boron (ml), C-Carbon (nm), N-Nitrogen (nm), O-Oxygen (nm), F-Fluorine (nm), Ne-Neon (nm), Na-Sodium (m), Mg-Magnesium (m), Al-Aluminum (m), Si-Silicon (ml), P-Phosphorus (P), S-Sulfur (nm), Cl-Chlorine (nm), Ar-Argon (nm), K-Potassium (m), Ca-Calcium (m)

Write the net ionic equation with phases HCN(aq) + KOH(aq) --> H2O(l) + KCN(aq)

HCN(aq) + OH- (aq) --> H2O(l) + CN- (aq)

List the strong acids (there's 7)

HClO3 - Chloric Acid HBr - Hydrobromic Acid HCl - Hydrochloric Acid HI - Hydroiodic Acid HNO3 - Nitric Acid HClO4 - Percholric Acid H2SO4 - Sulfuric Acid Strong Acid if # of O - # of H ≥ 2

What did Rutherford's gold foil experiment do for the advancement of the atomic model?

Helped make the idea of the nuclear atomic model

Which of the following statements about the subatomic particles are TRUE? I. Protons and neutrons account for most of an atom's mass. II. Protons and neutrons occupy most of the space in an atom III. Protons and neutrons account for most of an atom's charge

I only

A gas sample is a homogeneous mixture of gas 1, gas 2, and gas 3. Which of the following is always TRUE? I. n1 = n2 = n3 II. T1 = T2 = T3 III. V1 = V2 = V3

II & III

For a fixed amount of gas, which of the following will double the volume of the gas from 100 mL to 200 mL? I. Increase the temperature from 25ºC to 50ºC at constant pressure. II. Reduce the pressure from 760 torr to 380 torr at constant temperature

II only

What temperature scale must always be used to specify temperature in a gas law calculation?

Kelvin

Identify these elements based on their locations in the periodic table. Give the symbol - period 2, group 1 (1A) - period 4, group 11 (1B) - period 4, group 16 (6A)

Li Cu Se

List the strong bases (there's 7)

LiOH - Lithium Hydroxide NaOH - Sodium Hydroxide KOH - Potassium Hydroxide CsOH - Caesium Hydroxide Ca(OH)2 - Calcium Hydroxide Sr(OH)2 - Strontium Hydroxide Ba(OH)2 - Barium Hydroxide OH of group 1 (alkali metals) & the heavy elements of group 2 (alkali earth metals) are strong bases

In a mixture of H2 and O2 gases, the average molecular speed of O2 molecules in the same is _______ than the average molecular speed of the H2 molecules.

Lower (I think)

A standard 250-square-foot roll of household kitchen aluminum foil weighs 102 g. How many aluminum atoms is that?

Mass-->moles-->atoms 2.28*10^24 atoms

Calculate the percent composition of magnesium chloride

MgCl2 25.53% Mg 74.47% Cl

Determine the empirical formula of manganese (II) pyrophosphate, a compound containing 38.71% Mn, 21.82% P, and 39.46% O

Mn2P2O7

Classify these substances as molecular or ionic - AgNO3 - Cl2 - CaO - CuS - KCl - CH4 - H2O - BaSO4 - NaOH - NH3 - C6H12O6

Molecular: - C6H12O6 - NH3 - Cl2 - CH4 - H2O Ionic: - KCl - NaOH - BaSO4 - AgNO3 - CuS - CaO

What was the nuclear atomic model?

Most of mass in the positive nucleus with neutrons, most of volume from electrons around nucleus (Rutherford)

Calculate the percent composition of (NH4)3PO4

N = 28.186% H = 8.113% P = 20.776% O = 42.925%

List the weak base

NH3 - Ammonia (NH3 • H2O, NH4OH)

Determine the molecular formula of a substance if its empirical formula is NO2 and its molar mass is a) 46.0 g/mol b) 92.0 g/mol

NO2 N2O4

Consider the set of successive ionization energies: IE1 = 496 kJ/mol IE2 = 4562 kJ/mol IE3 = 6910 kJ/mol IE4 = 9543 kJ/mol Identify the element in period 3 that corresponds to this set of ionization energies.

Na

Determine the empirical of "hypo," a compound once popularly used in photographic film development, if a sample contains 2.453 g of sodium, 3.422 g of sulfur, & 2.561 g of oxygen.

Na2S2O3

A 18.0 mg sample of a compound containing C, H, and O was burned in air. The products were 26.4 mg of CO2 and 10.8 mg of H2O. What is the empirical formula of the sample?

No answer in book

A 6.055 g sample of a hydrate of copper(II) sulfate, CuSO4 • xH2O, is heated until all the water is driven off. After the anhydrous salt cools, its mass is 3.870 g. Calculate the value of x. (Hint: Treat this problem as an empirical formula problem with one of the "elements" H2O, and the other, CuSO4).

No answer in book

A 6.09 mg sample of a hydrocarbon was burned in air. The products were 17.9 mg of CO2 and 11.0 mg of H2O. What is the empirical formula of the sample?

No answer in book

Calculate the percent composition of - sodium dichromate - potassium permanganate

No answer in book

Calculate the percent composition of thiamine (a vitamin of the B complex family), C12H17N4OSCl

No answer in book

Classify the following water-soluble substances as being strong electrolytes, weak electrolytes or nonelectrolytes: - ZnCl2 - (NH4)2S2O3 - Li2SO4 - H3PO4 - CCl4

No answer in book

Classify the following water-soluble substances as being strong electrolytes, weak electrolytes, or nonelectrolytes: CuSO4 - H2S - HNO2 - UO2(NO3)2 - (NH4)2Cr2O7

No answer in book

Decide whether each of the following is an empirical formula: - C2H8N2 - Na2S2O8 - K2Cr2O7 - S4N4 - C12H21

No answer in book

Given the equation below, identify: a) the reactant that is reduced, b) the reactant that is oxidized, c) the reducing agent, and d) the oxidizing agent. NiSO4(aq) + Mg(s) → MgSO4(aq) + Ni(s)

No answer in book

Identify the type of reaction for each of the following: - Aqueous lithium hydroxide reacts with gaseous carbon dioxide to produce aqueous lithium hydrogen carbonate. - Solid calcium sulfite, on heating, produces solid calcium oxide and sulfur dioxide gas. - Pentene gas (C5H10) burns in excess oxygen to produce carbon dioxide and water. - Lithium metal when heated with nitrogen gas reacts to produce solid lithium nitride.

No answer in book

Polyethylene, a plastic that is commonly used for plastic bags and bottles, is composed of 85.63% carbon and 14.37% hydrogen. a) How many grams of each element are in 100.0 g of polyethylene? b) How many moles of each element are in 100.0 g of polyethylene? c) What is the mole ratio in integers? d) what is the empirical formula?

No answer in book

Predict if a precipitation reaction will occur. - Na3PO4(aq) + MgCl2(aq) → - Na2SO4(aq) + KOH(aq) → - MgSO4(aq) + CaCl2(aq) →

No answer in book

Predict if a precipitation reaction will occur: - Hg2(NO3)2(aq) + BaBr2(aq) → - Ca(OH)2(aq) + Ba(NO3)2(aq) → - Fe(C2H3O2)2(aq) + Li2S(aq) →

No answer in book

When KBr solution and Pb(ClO4)2 solution are mixed together, ____________________.

PbBr2 precipitate forms; K+ and ClO4- are spectator ions

Classify each of the possible reactions according to whether a precipitate will form or will not form a) Kl (aq) + NaCl(aq) --> ? b) KOH (aq) + FeCl3(aq) --> ? c) Na2CO3(aq) + CuCl2(aq) --> ? d) CrCl2 (aq) + Li2CO3 (aq) --> ? e) LiNO3(aq) + Na2SO4(aq) --> ?

Precipitate Forms: c, b, d No Precipitate: a & e

Rubidium (Rb) has two naturally occurring stable isotopes, Rb−85 (atomic mass: 84.912 amu) and Rb−87 (atomic mass: 86.909 amu). The atomic weight of rubidium is 85.468 amu. What is the percent abundance of Rb−87?

Rb-85 = 72.16% Rb-87 = 27.84%

Metallic mercury, Hg, can be obtained by heating the mineral cinnabar, HgS, in the presence of oxygen, O2. Use the following equation: HgS(s)+O2(g)→Hg(l)+SO2(g) Determine the amount of heat released when 5.50 g of HgS is heated in the presence of excess oxygen.

Releases 5.64 kJ of heat

If SeO4 (2-) is named selenate, then what is the name of SeO3 (2-)?

Selenite

For the reaction below, find the limiting reactant based on the initial amounts of reactants. 2 Na (s) + Br2 (g) → 2 NaBr (s) Then determine the moles of product formed. 12.6 mol Na, 6.9 mol Br2

Since 12.6 mol Na produce less NaBr than 6.9 mol Br2; Na is the limiting reactant. 12.6 mol of NaBr will be produced

How does the attraction between the individual atoms change between the different phases of matter?

Solid -- Liquid -- Gas Strong intermolecular forces----->Weak forces

What are the three phases of matter and explain the shape, volume, and if it's compressible

Solid: shape is fixed, volume is fixed, not compressible Liquid: shape is not fixed, volume is fixed, a little compressible Gas: shape & volume are not fixed, compressible

Determine whether each compound is soluble or insoluble in water - KBr - NiPO4 - PbCl2 - KNO3 - CuCO3 - KCl - Hg2Cl2

Soluble - KBr, KCl, & KNO3 Insoluble - PbCl2, NiPO4, Hg2Cl2, & CuCO3

For each of the following provide the number of electron groups, the hybridization of the central atom, the bond angles, the lewis structure, the number of valence electrons, the electron group geometry, the molecular geometry (including the drawing), and the polarity: - CH3Br - ICl2+ - C2H2 - CH3CH2CO2- - XeCl2 - COF2 - ICl4- - PO4(3-)

Sorry no pictures

A 186-g sample of a metal at 74.0 ºC is placed in 251 g of water at 18.0 ºC, and the final temperature of the system is 26.4 ºC. Calculate the specific heat of the metal. Which of the metals in table 6.3 could it be?

Specific heat of metal = 1.00 J/g • ºC Magnesium

A 25.0-g sample of a metal at 87.7°C is placed in 37.4 g of water at 10.3°C, and the final temperature of the system is 15.4°C. Calculate the specific heat of the metal. Which of the metals in Table 6.3 is it most likely to be?

Specific heat of the metal = 0.44 J/g • ºC, close to iron, chromium, and cobalt.

What did the discovery of the electron do for the advancement of the atomic model?

Spurred the idea of the plum pudding model

Determine the formula of the ionic compound formed from strontium and nitrogen.

Sr3N2

Classify these compounds as strong/weak acids/bases: - HF - HCl - KOH - Ba(OH)2 - H2CO3 - NH3 - HNO3

Strong Acids: HNO3 & HCl Weak Acids: H2CO4 & HF Strong Bases: KOH & Ba(OH)2 Weak Base: NH3

Classify each as a strong, weak, or non electrolyte: - HClO4 - NH3 - CH3OH - H3PO4 - C6H12O6 - KOH - CaCl2

Strong: HClO4, KOH, & CaCl2 Weak: H3PO4, & NH3 Non: CH3OH & C6H12O6

Calculate the final temperature after 11.3 g of iron (c = 0.44 J/g*ºC) at 60.0 ºC is placed in 97.2 g of water at 19.0 ºC.

T(final) = 20 ºC

Calculate the final temperature after 6.80 g of aluminum (c=0.892 J/g*ºC) at 67.4 ºC is placed in 195 g of water at 19.6 ºC

T(final) = 20.0 ºC

True/False - Oxidizing agents can convert CO into CO2 - A reducing agent gets oxidized as it reacts - If something is reduced, it is formally losing electrons - In the redox reaction Fe3+ + Co2+ --> Fe2+ + Co3+, Fe3+ is the reducing agent and CO2+ is the oxidizing agent - If there are no changes in the oxidation state of the reactants or products of a particular reactions hat reaction is not a redox reaction - If something is oxidized, it is formally losing electrons

T, T, F, F, T, T

Determine whether temperature is a state function or a path function and explain your reasoning.

Temperature is a state function. Recall that state functions describe the current state of a system and not the path taken to achieve that state. For example, the sample of ethanol in Figure 6.7 is at 25°C, whether it was originally a solid at -115°C or a gas at 79°C. The amount of energy that the liquid ethanol at 25°C possesses is described as a temperature (a state function) and not as heat (a path function).

What did Millikan discover?

The charge of an electron

Calculate the specific heat of water if 83.68 J is required to raise the temperature of 4.000 g of water by 5.000°C.

The heat flow of a reaction is given by the equation q=mcΔT After substituting the mass of water and the temperature increase, you can solve for the specific heat, c. 83.68 J=(4.000 g)(c)(5.000°C) c=(83.68 J)(4.000 g)(5.000°C)=4.184 J/g⋅°C Note that the unit for specific heat has two different units in its denominator (g and °C).

What's a spectator ion in an ionic equation?

The ions are dissociated and those that don't form another compound are the spectator ions.

When iodine (a purple solid) is added to ethyl alcohol (a colorless liquid), a uniform transparent liquid mixture with a brown color is formed. Is the iodine-ethyl alcohol mixture homogeneous or heterogeneous?

The mix is homogeneous because it is uniform in composition

The average kinetic energy of ideal gas molecules is directly proportional to the absolute temperature of the gas. (KE)avg = 3/2RT At a given temperature, all ideal gases have _______ average kinetic energy and _________ average molecular speed.

The same, different

Most of the particles in the Rutherford experiment: - went straight through the foil undeflected - were deflected at large angles - bounced backwards off the foil

Went straight through the foil undeflected

Which pair of the following atoms are isotopes, (235/118)X, (233/116)Y, (235/116)Z, & (233/117)Q (Note that X,Y,Z, and Q are not actual element symbols)

Y & Z

Under constant-volume conditions, the heat of combustion of glucose (C6H12O6) is 15.57 kJ/g. A 3.500-g sample of glucose is burned in a bomb calorimeter. The temperature of the calorimeter increases from 20.94 to 24.74 °C. a) What is the heat capacity of the calorimeter? b) If the size of the glucose sample had been exactly twice as large, and the initial temperature of the calorimeter and its content is 22.75 °C, what would the final temperature of the calorimeter be?

a) 14.4 kJ/ºC b) 30.3 ºC

Under constant-volume conditions, the heat of combustion of glucose (C6H12O6) is 15.57 kJ/g. A 3.500-g sample of glucose is burned in a bomb calorimeter. The temperature of the calorimeter increases from 20.94 to 24.72 °C. a) What is the total heat capacity of the calorimeter? b) If the size of the glucose sample had been exactly twice as large, and the initial temperature of the calorimeter and its content is 22.75°C, what would the final temperature of the calorimeter be?

a) 14.4 kJ/ºC b) 30.32 ºC

Perform the following calculations and report the answers to the correct number of sig figs. a) 2.171 cm * 4.20 cm b) 4.92 g / 1.64 cm^3

a) 2.171 cm×4.20cm=9.1182cm2=9.12cm2 9.1182 cm2 must be rounded to three significant digits because the second factor (4.20 cm) has only three significant digits. b) (4.92 g/1.64cm3)=3.00 g/cm3 It must have three significant digits because both the dividend (4.92 g) and the divisor (1.64 cm3) have only three significant digits. In this case, the division comes out to be exactly 3, so despite the fact that your calculator shows only a 3, you have to add two zeros to the answer given by the calculator to get the correct number of significant digits. Since the units were different in the dividend and the divisor, the final answer has units from both the original values.

How many moles of each element are in each of the following samples? a) 4.0 mol CCl4 b) 0.50 mol Fe3(PO4)2

a) 4.0 mol of C, 16 mol of Cl b) 1.5 mol Fe, 1.0 mol P, 4.0 mol O

For violet light with a frequency of 7.50 × 1014 s−1, calculate a) the energy of a single photon in joules. b) the energy of a mole of photons in joules per mole.

a) 4.97 * 10^-19 J b) 2.99 *10^5 J/mol

Limestone has the chemical name calcium carbonate, CaCO3 a) How many calcium, carbon, and oxygen atoms are in 1.00 mol of limestone? b) What is the total number of atoms in 1.00 mol of limestone?

a) 6.022*10^23 Ca atoms, 6.022*10^23 C atoms, & 1.807*10^24 O atoms b) 3.011*10^24 atoms total

When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffer cup calorimeter, the temperature rises from 21.6 to 37.8 °C. The specific heat capacity of water is 4.184 J/(g∙°C). a)Calculate the quantity of heat (in kJ) released in the reaction. Assume that the specific heat of the NaOH solution is the same as that of pure water. b) Using your results from part a, calculate ΔH (in kJ/mol NaOH) for the dissolution process. c) Since ΔH for the dissolution process is ____________ (positive or negative), we know that when NaOH is dissolves in water, it _____________ (absorbs or releases) heat which makes it an ______________ (endothermic or exothermic) process.

a) 7.22 kJ b) -44.4 kJ/mol = ∆H c) negative, releases, exothermic

When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffer cup calorimeter, the temperature rises from 21.6 to 37.8 °C. The specific heat capacity of water is 4.184 J/(g∙°C). a) Calculate the quantity of heat (in kJ) released in the reaction.Assume that the specific heat of the solution is the same as that of pure water. b) Using your results from part (a), calculate ΔH (in kJ/mol NaOH) for the dissolution process.

a) 7.22 kJ of heat is released when 6.50 g of NaOH is dissolved in water b) -44.4 kJ/mol NaOH

What are the names of the following cations? a) Ba 2+ b) Ag + c) Co 2+ d) Co 3+ e) Li +

a) Barium ion b) Silver ion c) Cobalt (II) ion d) Cobalt (III) ion e) Lithium ion

Name the following compounds: a) BaSO4 b) Al(C2H3O2)3 c) Co(ClO3)3

a) Barium sulfate b) Aluminum acetate c) Cobalt(III) chlorate

Valproic acid, used to treat seizure and bipolar disorder, consists of C, H and O. A 0.165-g sample is burned in a combustion analysis apparatus. The gain in mass of the H2O absorber is 0.166 g. The gain in mass of the CO2absorber is 0.403 g. a) What is the empirical formula for valproic acid? b) If the molar mass is 144 g/mol, what is the molecular formula?

a) C4H8O b) C8H16O2

Which energy conversions are exhibited by (a) a firework exploding and (b) a loud motorcycle accelerating up a hill?

a) Chemical energy in the firework is converted to sound, light, heat, and kinetic energy as the paper shreds go flying. b) Chemical energy in the gasoline that fuels the motorcycle is converted to potential energy as the motorcycle goes up the hill, to kinetic energy as it accelerates, and to heat and sound in the engine.

Which energy conversions are exhibited by (a) using the flashlight app on your cell phone and (b) recharging your cell phone battery by plugging it into a wall outlet?

a) Chemical energy in your cell phone battery is converted to electrical energy, which is converted to light. b) Electrical energy from the wall outlet is converted to chemical energy in your phone's battery.

Classify the following elements as main group, transition elements, or inner transition elements. a) Cs b) In c) U

a) Cs (group 1, period 6) is a main group element b) In (group 13, period 5) is a main group element c) U is an inner transition element - an actinide

Which of the following statements are true and which are false? a) If a subshell contains two electrons, then it must be an s subshell. b) Any orbital can contain zero, one, or two electrons, with two being the maximum. c) A d subshell can hold more electrons than can a p subshell because the d subshell is made up of more orbitals than is the p subshell.

a) False b) True c) True

Water can be formed via the reaction of gaseous hydrogen and oxygen. 2 H2(g)+O2(g)→2 H2O(l)ΔH=-572 kJ a) Write the balanced equation that shows 1 mol water produced. b) Determine the enthalpy of the reaction in units of kJ/mol of water produced.

a) H2(g) + 1/2 O2(g) --> H2O(l) b) -286 kJ/mol water

Name the acids and bases first and classify them as strong / weak acid or strong / weak base. (a)HF (b)HBr (c)HNO2 (d)HBrO3 (e)HCN (f)H2S (g)H2SO4 (h)Ba(OH)2 (i)NH3∙H2O (j)CH3COOH

a) Hydrofluoric acid weak acid b) Hydrobromic acid strong acid c) Nitrous acid weak acid d) Bromic acid strong acid e) Hydrocyanic acid weak acid f) Hydrosulfuric acid weak acid g) Sulfuric acid strong acid h) Barium hydroxide strong base i) Ammonia weak base j) Acetic acid weak acid

Lactose reacts with O2 to form CO2 and H2O. C12H22O11(s)+12 O2(g)→12 CO2(g)+11 H2O(l) A small mass of lactose reacts with excess O2 inside a bomb calorimeter and the temperature of the water inside the calorimeter increases from 19.4°C to 28.6°C. a) Determine the signs of qsoln and qv in the reaction. b) Determine whether the reaction is endothermic or exothermic.

a) In this reaction, the temperature of the water inside the calorimeter increases, indicating the heat is transferred from the reaction to the water. Therefore, qsoln is positive (heat is gained) and qv is negative (heat is lost). b) Heat is transferred from the reaction to the solution, so the reaction is exothermic.

Assuming the element symbols are correct, which of the following isotopic symbols are correct? Explain why. a) (6/14)C b) O-17 c) (_/2) H d) (14/6)N e) S-6

a) Incorrect. Carbon has an atomic number of 6, not 14. Carbon can have a mass number of 14, though, so the atomic and mass numbers must be switched b) Correct c) Incorrect. Hydrogen has 1 proton, not two d) Incorrect. Nitrogen's atomic number is 7 not 6 e) Incorrect. Sulfur has an atomic number of 16 and a smaller mass number is impossible

Determine the names of the following compounds: a) MgCl2 b) MgCl2 * 6 H2O

a) Magnesium chloride b) Magnesium chloride hexahydrate

Which of the following elements are metals and which are nonmetals? a) Calcium, Ca b) Phosphorus, P c) Nickel, Ni d) Carbon, C

a) Metal b) Nonmetal c) Metal d) Nonmetal

Given the properties of the following elements, determine whether the element is most likely a metal, nonmetal, or metalloid. a) Shiny, malleable, conducts electricity b) Shiny, brittle, conducts electricity c) Dull, brittle, doesn't conduct electricity

a) Metals b) Metalloid c) Nonmetals

What are the symbols of the following elements? a) Manganese b) Arsenic c) Germanium d) Plutonium

a) Mn b) As c) Ge d) Pu

Determine whether the following mixtures are homogeneous or heterogeneous. a) Mud (a mixture of dirt and water that settles out over time) b) Carbonated water (a mixture of water and carbon dioxide) before the bottle is opened c) Carbonated water (a mixture of water and carbon dioxide) immediately after the bottle is opened

a) Mud is heterogeneous. After mud settles over time into dirt and water, its nonuniform composition is revealed. b) Before the bottle is opened, you cannot see the bubbles, which suggests a homogeneous mixture. c) Immediately after opening the bottle, the gas bubbles can be seen within the liquid, which suggests a heterogeneous mixture

a) If sample A weighs twice as much as sample B, is it possible to tell which sample is iron and which is powdered sugar? b) If sample A is attracted by a magnet and sample B is a white powder, is it possible to tell which sample is iron and which is powdered sugar?

a) No. The weight of a sample is an extensive property that does not tell anything about the material's identity. b) Yes. The magnetism of sample A and the physical appearance of sample B are intensive properties that can be used to identify sample A as iron and sample B as powdered sugar.

Write the formulas for the following compounds: a) Lead(IV) sulfate b) Aluminum sulfide

a) Pb(SO4)2 b) Al2S3

The percentage of carbon in a small box of the pure substance sucrose (table sugar) is 42.1%. a) Is sucrose an element or a compound? b) What is the percentage of carbon in a large box of sucrose?

a) Sucrose is a compound - it contains more than one element. If it contained just carbon, then the percentage of carbon would be 100%, 42.1% b) The larger box also contains 42.1% carbon because a given compound always contains the same percentage of each of its elements, no matter what the size of the sample.

a) A 4.33 g sample of dinitrogen monoxide, N2O, is composed of 63.65% nitrogen and 36.35% oxygen by mass. What is the percent composition of a 14.9 g sample of N2O? b) Nitrogen monoxide, NO, has a percent composition of 46.68% nitrogen and 53.32% oxygen by mass. What possible percentages of nitrogen could be in a mixture of N2O and NO?

a) The 14.9 g sample is 63.65% nitrogen and 36.35% oxygen by mass also. According to the law of definite proportions, all pure samples of N2O have the same percent composition. b) The possible percentages of nitrogen in the N2O/NO mixture would be between 63.65% (the percentage of nitrogen in N2O) and 46.68% (the percentage of nitrogen in NO).

a) A pure substance is heated in air until no further reaction takes place. A different pure substance is produced that has a mass that is 58.5% of that of the original substance. Can you tell whether each substance in this reaction is an element or a compound? b) After a different pure substance is heated in air, a new pure substance is formed that has a mass of 138% of that of the original substance. Can you tell whether each substance in these reactions is an element or a compound?

a) The first substance (the reactant) is a compound. When it is heated, it decomposes into a different material that is left behind and some gaseous product that escapes into the air. Because the mass of the new material is less than the mass of the original substance, the original substance must have decomposed—in which case, it cannot be an element. The new product might or might not be decomposable, so you cannot tell from the information given whether it is an element or a compound. b) The second substance (the product) gained mass, so it must have combined with something in the air. The product is therefore a combination of substances and cannot be an element. You do not know if the original substance (the reactant) can be decomposed (it was not decomposed in this experiment), so you cannot tell if it is an element or a compound.

Suppose a bathroom scale registers 2 lb with no load. An object is weighed repeatedly on this bathroom scale, and each results in a reading of 117 lb. a) Are the measurements precise? b) Are the measurements accurate? c) What is the probable true weight of the object?

a) The measurements are precise because exactly the same weight value (to the precision of the device) was obtained each time. b) They are not accurate because the no-load value was incorrect. c) Since the scale reads 2 lb with no load, it is likely giving readings that are falsely high by 2 lb. Therefore, the true weight is probably 117 lb - 2 lb = 115 lb.

A scientist conducts a few experiments in her lab and comes up with an initial explanation for her observations. a) What is the proper term for this initial explanation? b) Suppose that the scientist and several of her colleagues conduct numerous additional experiments and that none of the new results contradict the original explanation. What is the proper term for the explanation at this point?

a) The scientist's initial explanation for her observations is known as a hypothesis. b) After numerous additional experiments are performed and none of the results contradicts the original hypothesis, the explanation may become a scientific theory.

Determine the relative number of each type of element in the following compounds. a) CO2 b) PCl3 c) Fe(OH)3 d) Na2S e) B2H6 f) Ni(ClO4)2

a) Two oxygen, one carbon b) Three chlorine, one phosphorus c) Three oxygen, three hydrogen, one iron d) Two sodium, one sulfur e) Six hydrogen, two boron f) Two chlorine, eight oxygen, one nickel

Write formulas for the following compounds: a) Zinc nitrate b) Cobalt (III) hypochlorite

a) Zn(NO3)2 b) Co(ClO)3

Write formulas for the following compounds: a) Anhydrous zinc sulfate b) Zinc sulfate heptahydrate

a) ZnSO4 b) ZnSO4 * 7 H2O

Write the isotopic symbol that correctly represents each of the following. a) A hydrogen isotope with two neutrons b) An iodine isotope with 78 neutrons c) A polonium isotope with 42 more neutrons than protons

a) ^3 H b) ^131 I c) ^210 Po

Write symbols for each of the following isotopes by using an element symbol with a superscript. a) A helium atom with a mass number of 3 b) An oxygen atom with 7 neutrons in the nucleus c) A boron atom with equal numbers of protons and neutrons in the nucleus d) A carbon atom that has one more neutron than protons in its nucleus

a) ^3He b) ^15O c) ^10B d) ^13C

Write the empirical formulas for the compounds containing carbon, C, and hydrogen, H, in the following ratios. a) 2 mol carbon to 3 mol hydrogen b) 1.0 mol carbon to 1.5 mol hydrogen c) 0.1712 mol carbon to 0.2568 mol hydrogen

a) just the ratio C2H3 b) multiply to get whole numbers C2H3 c) divide each by the smallest to get whole numbers C2H3

How many unpaired electrons are in (a) an aluminum atom and (b) an argon atom?

a) one unpaired b) no unpaired

Name the following compounds: a) NaNO3 b) Cu2S c) (NH4)2SO4

a) sodium nitrate b) copper(I) sulfide c) ammonium sulfate

Given the thermochemical equation below, we know that this reaction ________ heat which makes it an __________ reaction. 2 C (s) + H2 (g) ⟶ C2H2 (g) ΔHrxn = 226.8 kJ

absorbs, endothermic

A 25.0-g sample of a metal at 87.7°C is placed in 37.4 g of water at 10.3°C, and the final temperature of the system is 15.4°C. Calculate the specific heat of the metal. Which of the metals in Table 6.3 is it most likely to be?

c(metal) = 0.44 J/g*ºC -- Closest to iron but chromium and cobalt are close too

A 186-g same of a metal at 74.0ºC is placed in 251 g of water at 18.0ºC, and the final temperature of the system is 26.4ºC. Calculate the specific heat of the metal. Which of the metals in Table 6.3 could it be?

c(metal) = 1.00 J/g*ºC Magnesium

In general, atomic radius _______ from left to right across a period and ionization energy ______ going down a group.

decreases, decreases

- When heat flows INTO the system, the reaction is ______thermic. - ∆E __ 0 & ∆H __ 0 - This type of reaction is _____ to the touch

endo >, > cool

- When heat flows OUT of the system, the reaction is _____thermic - ∆E ____ 0 & ∆H ____ 0 - This type of reaction is ______ to the touch

exo <, < hot

Determine the empirical formula of a compound that has a percent composition of 43.7% P and 56.3% O.

in grams --> moles --> divide by smallest --> multiply for whole numbers : P2O5

Styrene is used commercially to prepare the plastic wrapping material polystyrene. It is a molecular compound made up of carbon and hydrogen only. It contains 92.26% carbon and has a molar mass of 104 g/mol. What is the molecular formula of styrene?

in grams --> moles --> find empirical --> find molar mass of empirical and compound --> divide to get multiplier : C8H8

What information is needed to determine the general shape of an orbital?

l

Identify which type of orbital would be present if l= 0, 1, 2, or 3. Draw each of the orbitals for l = 0 and 1

l = 0, 1, 2, or 3: s=0, p=1, d=2, f=3

What values are needed to determine the energy of an electron in a many-electron atom?

l and n

Electromagnetic radiation with a lower frequency has a _______ wavelength and _______ energy.

longer, lower

Oxidation occurs when an atom in a substance ___________ electron(s) which causes the oxidation number of the atom to ________ going from the reactant to the product.

loses, increase

The standard atmospheric pressure at sea level is 1 atm or 760 mmHg. On a typical day in Denver (elev: 5280 ft), the atmospheric pressure is _________.

lower than 760 mmHg

What information is needed to determine the orientation of an orbital?

m(l)

What information is most important in determining the size of an orbital?

n

Which quantum numbers, n & l, are valid for the third energy level?

n = 3 l = 0, 1, & 2

What quantum numbers specify these subshells? 2s 4p 4d

n-2, l=0 n=4, l=1 n=4, l=2

What color is a photon that has an energy of 3.28 × 10-19 J?

orange to red-orange

A photon with a higher frequency has a ______ wavelength and _____ energy.

shorter, higher

What are the quantum numbers of electron #8 in a Na atom?

(2, 1, 1, -1/2)

What are the four quantum numbers of electron #15 in Cl?

(3, 1, -1, 1/2)

A radio station broadcasts at a frequency of 1.01*10^8 Hz. Express this frequency in MHz

101 Mhz

Write the balanced equation for the neutralization reaction between HCl & Ba(OH)2 in an aqueous solution

2HCl + Ba(OH)2 --> 2H2O + BaCl2

Complete and balance the molecular equation: CuCl2(aq) + K3PO4(aq) -->

3CuCl2(aq) + 2K3PO4(aq) --> Cu3(PO4)2(s) + 6KCl(aq)

What is the amount, in moles, in 0.0355 g of Zn?

5.43 * 10^-4 mol Zn

How many electrons in an atom can be described by the quantum number n = 2?

8

What was the plum pudding model?

After the discovery of electrons, atoms seen as a ball of positive mass sprinkled with negatively charged particles. (Thompson)

List the weak acids (there's 10)

HF - Hydrofluoric Acid HCN - Hydrocyanic Acid H2S - Hydrogen Sulfide HNO2 - Nitrous Acid H2SO3 - Sulfurous Acid HClO2 - Chlorous Acid CH3COOH - Acetic Acid HClO - Hypochlorous Acid H2CO3 - Carbonic Acid H3PO4 - Phosphoric Acid Whenever you see -COOH, it's a weak acid

Alpha particles are _________ and have a __________ charge.Beta particles are __________ and have a __________ charge. Gamma-ray particles are ____________ and have a ________ charge.

He 2+, positive e-, negative energy, no

What is the oxidation state of each element in K2Cr2O7?

K = 1 O = -2 Cr = +6

nah

No answer in book

How many protons and electrons are in each of the following ions? a) F- b) Mg 2+ c) N 3- d) W 6+

a) 9 protons, 10 electrons b) 12 protons, 10 electrons c) 7 protons, 10 electrons d) 74 protons, 68 electrons

Name the following acids. Correct spelling matters. - HClO - HF - H2SO4

ah

Draw an electromagnetic wave and label the amplitude and wavelength. What do each of these determine? What is the frequency?

sorry no pic

Use electronic energy-level diagrams to determine the number of unpaired electrons in (a) a fluorine atom, (b) an oxygen atom, and (c) a boron atom.

sorry no pics

Rank the following masses from the lightest to the heaviest: 9.8 x 10^3 mg 9.8 x 10^-8 kg 9.8 x 10^4 µg

uh

Identify the following properties as either physical or chemical: - Honey can be easily dissolved in hot water. - Cheese spoils easily without refrigeration. - A chunk of sulfur is brittle and shatters when dropped.

um - Chemical - Chemical - Physical is what I answered but one of them is wrong so

Determine the frequency and energy for light with a. wavelength of 694.0 nm. What color is the light?

v = 4.32 * 10^14 E = 172.8 kJ/mol (remember, a mol = 6.022*10^23 photons) Red

A gaseous mixture contains 0.540 bar H2(g), 0.497 bar N2(g), and 0.127 bar Ar(g). Calculate the mole fraction, x, of each of these gases.

x(H2) = .463 x(N2) = .427 x(Ar) = .109

Determine the wavelength and energy for light with a frequency of 5.831 * 10^14 Hz. What color is the light?

y = 514.5 nm E = 232.8 kJ/mol green

A system does 536 kJ of work and loses 261 kJ of heat to the surrounding. What is the change in internal energy, ∆E, of the system?

∆E = -797 kJ

Use the ∆H values for equations I, II, and III to calculate the enthalpy change of the general reaction Z + Q --> X + 2R I. E + 2D --> Z + Q ∆H = 41.7 kJ II. J + A --> E + 2D ∆H = -17.1 kJ III. J + A --> X + 2R ∆H = 10.6 kJ

∆H = -14.0 kJ

Determine the enthalpy change for this reaction from the following data. 4NO(g)+6H​ O→4NH​ (g)+5O​ (g) N​2 (g)+3H​2 (g)→2NH​ 3(g). ΔH=-97.8kJ N​2(g)+O​2(g)→2NO(g) ΔH=167.5kJ 2H2​ (g)+O​2(g)→2H​2O(g) ΔH=-698.7kJ

∆H = 1565.5kJ

For a compound, the standard enthalpy of formation equals the enthalpy change of the reaction when one mol of the compound forms from its constiuent elements in their standard states. Based on this definition, ∆Hºf(NH3,g) = ________. N(g) + 3H(g) --> NH3(g) ∆Hºrxn1 N2(g) + 3H2(g) --> 2NH3(g) ∆Hºrxn2 1/2N2(g) + 3/2H2(g) --> NH3(g) ∆Hºrxn3

∆Hºrxn3

How many sig figs are in: - 0.9683 - 0.08206 - 21.1 - 21.10 - 760 - 760. - 6.0225 * 10^23 - 0.760

- 4 - 4 - 3 -4 - 2 - 3 - 5 - 3

Write the formula for each: - Selenium tetrafluoride - Oxygen difluoride - Dinitrogen monoxide - Phosphorus trichloride

- SeF4 - OF2 - N2O - PCl3

If the first two quantum numbers for an electron are n = 3 and ℓ = 1, which values for mℓ are possible, and which orbital does the electron occupy?

-1, 0, 1

Methane, CH4, can be synthesized by the following reaction of carbon dioxide, CO2, with hydrogen gas, H2: CO2(g) + 4H2(g) --> CH4(g) + 2H2O(g) Determine the amount of heat released when 25 kg of H2 is heated in the presence of excess CO2.

-5.1 * 10^5 kJ

What is the maximum number of electrons in the n = 3 shell?

18

What is the valence electron configuration of Sb?

5s25p3

Convert a speed of 397 cm/s to units of inches per minute.

9380 in/min

What is the speed of an e-​ if it has a wavelength of 765nm?The mass of an e-​ is 9.11x10​^-31 kg.(1J=kg*m​^2/s^2)

950.76 m/s

Predict the solubility of the following salts: - Ba(NO3)2 - Ag2SO4 - PbCl2 - ZnS

No answer in book

Write a balanced chemical equation for the reaction of aqueous potassium hydroxide with phosphoric acid to yield potassium phosphate plus water.

No answer in book

Write the indicated equations for the aqueous reaction of formic acid (HCO2H) with potassium hydroxide. - a balanced total equation - a complete ionic equation - a net ionic equation

No answer in book

Richard performed the following reaction. 2C​2H2​ + 5O2​ → 4CO2​ + 2H​2O He began with 7.98g of starting material and ended with 5.99g of total product (both carbon dioxide and water). Is this possible? Why or why not?

No because of the law of conservation of mass (mass of products should be equal to the mass of the reactants)

Horace Slughorn wanted to improve the yield of his felix felicis, (He just wanted a larger volume.) If he started with 2.22 moles of solution and a volume of 3 mL, he figured that he could get his yield to be 4.5 mL. But, at the end of his planning, he decided that he needed to start instead with 1.79 moles and the same volume. Would Slughorn's plan to use less moles give him a greater yield? Why or why not?

No, 1.79 moles would make 2.41 mL not 4.5 mL

A gaseous mixture is made by combining 1.69 g Ar and 4.61 g Kr in an evacuated 2.50 L container at 25.0 ºC. Calculate the partial pressures of each gas and the total pressure exerted by the gaseous mixture.

P(Ar) = 0.419 bar P(Kr) = 0.545 bar P(total) = 0.965 bar

A mixture of oxygen and neon contains oxygen at a pressure of 726 torr and neon at a pressure of 44 torr. What is the total pressure of the mixture?

P(total) = 770 torr or just over 1 atm

Rank the following atom and ions in decreasing order of radius: Se2−, Kr, Rb+, Br−

Rb+ < Kr < Br- < Se2-

What is the charge of a zinc ion?

Zn 2+

Determine the formula of the compound containing the following pairs of ions. a) Cr (2+) and SO4 (2-) b) Cr (3+) and CO3(2-)

a) CrSO4 b) Cr2(CO3)3

Consider a reaction as the system. When ∆Hrxn = q > 0, the reaction _______ heat, which makes it an _______ reaction.

absorbs, endothermic