Chem Exam 1

Determine the name for Cl2O. A) chlorine oxide B) dichlorine monoxide C) chlorine (I) oxide D) chlorine (II) oxide E) chlorate

B) dichlorine monoxide

Which one of the following elements is a poor conductor of heat and electricity? A) copper B) fluorine C) iron D) lead

B) fluorine

How many of the following compounds are insoluble in water? KC2H3O2 CaSO4 SrS AlPO4 A) 0 B) 1 C) 2 D) 3 E) 4

C) 2

The compound, ClO, is named A) chlorite. B) hypochlorite. C) chlorine monoxide. D) chlorine (II) oxide.

C) chlorine monoxide.

Iodine belongs to the ________ group of the periodic table. A) alkali metal B) alkaline earth metal C) halogen D) noble gas

C) halogen

Which of the following elements is a gas at room temperature? A) bromine B) carbon C) helium D) sodium

C) helium

Determine the number of protons, neutrons and electrons in the following: 25/12X A) p+ = 12 n° = 25 e- = 12 B) p+ = 12 n° = 12 e- = 13 C) p+ = 12 n° = 13 e- = 12 D) p+ = 25 n° = 12 e- = 13 E) p+ = 12 n° = 13 e- = 25

C) p+ = 12 n° = 13 e- = 12

Which of the following is a molecular element? A) neon B) lithium C) selenium D) magnesium E) titanium

C) selenium

HCl , HI , H2SO4, LiCl , and KI are all classified as A) acids. B) nonelectrolytes. C) strong electrolytes. D) weak electrolytes.

C) strong electrolytes.

The chemical formula for lithium peroxide is A) LiOH. B) LiO2. C) Li2O. D) Li2O2.

D) Li2O2.

What is the identity of element Q if the ion Q2+ contains 10 electrons? A) C B) O C) Ne D) Mg

D) Mg

Which of the following is an oxidation-reduction reaction? A) HCl(aq) + LiOH(aq) → LiCl(aq) + H2O(l) B) NaI(aq) + AgNO3(aq) → AgI(s) + NaNO3(aq) C) Pb(C2H3O2)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2 NaC2H3O2(aq) D) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) E) All of the above are oxidation-reduction reactions.

D) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)

Choose the heterogeneous mixture from the list below. A) sports drink B) chlorine gas C) beer D) lasagna E) carbon (graphite)

D) lasagna

Identify the principal component of natural gas. A) propane B) ethane C) n-butane D) methane E) n-pentane

D) methane

Argon belongs to the ________ group of the periodic table. A) alkali metal B) alkaline earth metal C) halogen D) noble gas

D) noble gas

Determine the number of protons, neutrons and electrons in the following: 65/29X A) p+ = 36 n° = 29 e- = 36 B) p+ = 29 n° = 29 e- = 36 C) p+ = 36 n° = 36 e- = 29 D) p+ = 29 n° = 36 e- = 29 E) p+ = 29 n° = 36 e- = 36

D) p+ = 29 n° = 36 e- = 29

Which of the following elements has chemical properties similar to tellurium? A) fluorine B) hydrogen C) nitrogen D) sulfur

D) sulfur

The mass number is equal to A) the sum of the sum of the electrons and protons. B) the sum of the sum of the neutrons and electrons. C) the sum of the number of protons, neutrons, and electrons. D) the sum of the number of protons and neutrons.

D) the sum of the number of protons and neutrons.

choose the pure substance from the list below a. gatorade b. chlorine gas c. black coffee d. chicken noodle soup e. carbon (graphite)

e. carbon (graphite)

What species is represented by the following information? p+ = 12 n° = 14 e- = 10 A) Si4+ B) Mg C) Ne D) Si E) Mg2+

E) Mg2+

Which of the following elements is a nonmetal? A) Zn B) Cs C) Ca D) Co E) P

e. p

List the elements in a hydrocarbon.

hydrogen and carbon

define matter

matter is anything that occupies space and has mass

determine the mass of an object that has a volume of 88.6 mL and a density of 9.77 g/mL a. 298 g b. 1100 g c. 907 g d. 568 g e. 866 g

e. 866 g

two or more substances in variable proportions where the composition is variable throughout are considered a. a solution b. a homogeneous mixture c. a compound d. an amorphous solid e. a heterogeneous mixture

e. a heterogeneous mixture

which of the following statements is true? a. a scientific law is a fact b. once a theory is constructed, it is considered fact c. a hypothesis is a speculation that is difficult to test d. an observation explains why nature does something e. a scientific law summarizes a series of related observations

e. a scientific law summarizes a series of related observations

which of the following is an example of physical change? a. sugar is dissolved in water b. coffee is brewed c. dry ice sublimes d. ice melts e. all of these are examples of physical change

e. all of these are examples of physical change

Give the name for HNO2.

nitrous acid

The correct answer (reported to the proper number of significant figures) to the following is ________.

(1815 - 1806) × (9.11 × 7.92) = 600

Determine the oxidation state of Mn in KMnO4.

+7

How many moles of CO2+ are present in 0.150 L of a 0.200 M solution of CoI2?

0.0300

Calculate the concentration (M) of sodium ions in a solution made by diluting 40.0 mL of a 0.474 M solution of sodium sulfide to a total volume of 300 mL.

0.126

What is the concentration (M) of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

0.29

Balance the following equation. ____ C10H12 + ____ O2 → ____ H2O + ____ CO2

1 C10H12 + 13 O2 → 6 H2O + 10 CO2

What is the concentration (M) of sodium ions in 4.57 L of a .398 M Na3P solution?

1.19

Determine the mass percent (to the hundredths place) of H in sodium bicarbonate (NaHCO3).

1.20

There are ________ mol of bromide ions in 0.900 L of a 0.500M solution of AlBr3.

1.35

The correct answer (reported to the proper number of significant figures) to the following is ________.

11.5 × 8.78 = 101

If 294 grams of FeS2 is allowed to react with 176 grams of O2 according to the following unbalanced equation, how many grams of Fe2O3 are produced? FeS2 + O2 → Fe2O3 + SO2

160

38.325 lbs = ________ grams. (1 lb = 454 g)

17400

What is the concentration (M) of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in sufficient water to give exactly 230 mL of solution?

2.28

How many grams of NaOH (MW = 40.0) are there in 250.0 mL of a 0.275 M NaOH solution?

2.75

How many grams of H3PO4 are in 265 mL of a 1.50 M solution of H3PO4?

39.0

A flash drive contains 4 gigabytes. How many bytes does it contain?

4,000,000,000 bytes, 4 × 109 bytes, or 4,292,967,296 byte if someone is computer literate

How many grams of CH3OH must be added to water to prepare 150mL of a solution that is 2.0 M CH3OH?

9.6

Describe the difference between complete ionic and net ionic equations.

A complete ionic equation shows all of the substances present in the reaction mixture. A net ionic equation only shows the substances that are participating in the reaction. The spectator ions are absent in the net ionic equation.

Describe the difference between a molecular formula and an empirical formula. Give an example.

A molecular formula is the exact number of each type of atom necessary to build a specific molecule. An empirical formula is simply the smallest whole number ratio between atoms in a compound. For example, C2H4 is the molecular formula for ethene. The empirical formula for ethene is CH2, the smallest whole number ratio between the atoms.

what is the difference between a physical property and a chemical property? Give an example of each.

A physical property is one that a substance displays without changing its composition, whereas a chemical property is one that a substance displays only by changing its composition via a chemical change. Physical properties include color, appearance, melting point, boiling point, and density. Chemical properties include corrosiveness, flammability, acidity, and toxicity.

What causes a precipitation reaction to occur between two soluble compounds?

A precipitate, or insoluble compound, forms from a pair of the ions present that participate in a reaction. This "traps" some of the ions into a newly formed compound causing reaction.

Determine the oxidation state of P in PO33-. A) +3 B) +6 C) +2 D) 0 E) -3

A) +3

Give the oxidation state for S in SO3-2. A) +4 B) +6 C) -2 D) +2 E) +5

A) +4

How many grams of CaCl2 are formed when 15.00 mL of 0.00237 M Ca(OH)2 reacts with excess Cl2 gas? 2 Ca(OH)2(aq) + 2 Cl2(g) → Ca(OCl)2(aq) + CaCl2(s) + 2 H2O(l) A) 0.00197 g B) 0.00394 g C) 0.00789 g D) 0.0507 g

A) 0.00197 g

Which of the following solutions will have the highest electrical conductivity? A) 0.045 M Al2(SO4)3 B) 0.050 M (NH4)2CO3 C) 0.10 M LiBr D) 0.10 M NaI E) 0.10 M KF

A) 0.045 M Al2(SO4)3

What is the molarity of a potassium triiodide solution, KI3(aq), if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.200 M thiosulfate solution, K2S2O3(aq)? The chemical equation for the reaction is 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq). A) 0.0833 M B) 0.120 M C) 0.167 M D) 0.333 M

A) 0.0833 M

How many moles of BCl3 are needed to produce 10.0 g of HCl(aq) in the following reaction? BCl3(g) + 3 H2O(l) → 3 HCl(aq) + B(OH)3(aq) A) 0.0914 mol B) 0.274 mol C) 0.823 mol D) 10.9 mol

A) 0.0914 mol

Lithium and nitrogen react to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) How many moles of lithium nitride are produced when 0.450 mol of lithium react in the presence of excess nitrogen? A) 0.150 B) 0.900 C) 0.0750 D) 1.35 E) 0.225

A) 0.150

In an acid-base neutralization reaction 38.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution? A) 0.194 M B) 0.387 M C) 0.775 M D) 1.29 M

A) 0.194 M

How many H+ ions can the acid, H2SO4, donate per molecule? A) 0 B) 1 C) 2 D) 3

C) 2

1.06g of Na2CO3 is dissolved in 100mL of water. What is the molarity of Na+ ions in the solution? A) 0.2 M B) 0.1 M C) 1 × 10-4 M D) 0.01 M

A) 0.2 M

The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)? A) 0.20 M B) 0.40 M C) 0.10 M D) 0.36 M E) 0.25 M

A) 0.20 M

A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150. mL of solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make water to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution? A) 0.274 M B) 0.356 M C) 2.81 M D) 3.65 M

A) 0.274 M

Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO2(g) + H2O(l) → HNO3(l) + NO(g) Suppose that 4mol NO2 and 2 H2O mol combine and react completely. How many moles of the reactant in excess are present after the reaction has completed? A) 0.7 B) 1 C) 0 D) 3

A) 0.7

A solution is prepared by adding 1.60 g of solid NaCl to 50.0 mL of 0.100 M CaCl2. What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL. A) 0.747 B) 0.647 C) 0.132 D) 0.232 E) 0.547

A) 0.747

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution? A) 0.801 B) 0.315 C) 0.629 D) 125 E) 0.400

A) 0.801

Which of the following numbers has the greatest number of significant figures? A) 0.8010 B) 0.504 C) 742000 D) 9.05 × 1024

A) 0.8010

What mass, in g, of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl2 solution? 2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq) A) 0.838 g B) 1.72 g C) 0.859 g D) 2.56 g E) 1.70 g

A) 0.838 g

Convert 10 cm3 to m3. A) 1 × 10-5 m3 B) 1 × 10-1 m3 C) 1 × 103 m3 D) 1 × 107 m3

A) 1 × 10-5 m3

Predict the charge that the ion formed from bromine would have. A) 1- B) 2+ C) 1+ D) 4+ E) 2-

A) 1-

When 31.2 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, how many grams of AgCl are formed? AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq) A) 1.07 g B) 2.24 g C) 3.31 g D) 6.44 g

A) 1.07 g

If 1.4% of the mass of a human body is calcium, how many kilograms of calcium are there in a 185-pound man? A) 1.2 kg Ca B) 5.7 kg Ca C) 1.2 × 102 kg Ca D) 5.7 × 102 kg

A) 1.2 kg Ca

How many moles of N2O3 contain 2.55 × 1024 oxygen atoms? A) 1.41 moles N2O3 B) 4.23 moles N2O3 C) 12.7 moles N2O3 D) 7.87 moles N2O3 E) 2.82 moles N2O3

A) 1.41 moles N2O3

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution. A) 1.50 M B) 1.18 M C) 0.130 M D) 0.768 M E) 2.30 M

A) 1.50 M

According to the balanced equation shown below, 4.00 moles of oxalic acid, H2C2O4, reacts with ________ moles of permanganate, MnO4-. 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + Mn2+(aq) + 8 H2O(l) A) 1.60 B) 4.00 C) 8.00 D) 9.00

A) 1.60

When 7.00 × 1022 molecules of ammonia react with 6.00 × 1022 molecules of oxygen according to the chemical equation shown below, how many grams of nitrogen gas are produced? 4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g) A) 1.63 g B) 1.86 g C) 4.19 g D) 6.51 g

A) 1.63 g

Methane and oxygen react to form carbon dioxide and water. What mass of water is formed if 0.80 g of methane reacts with 3.2 g of oxygen to produce 2.2 g of carbon dioxide? A) 1.8 g B) 2.2 g C) 3.7 g D) 4.0 g

A) 1.8 g

Silver has an atomic mass of 107.868 amu. The Ag-109 isotope (108.905 amu) is 48.16%. What is the amu of the other isotope? A) 106.905 amu B) 106.908 amu C) 106.903 amu D) 106.911 amu

A) 106.905 amu

How many moles of potassium are contained in 449 g of potassium? A) 11.5 moles B) 17.6 moles C) 69.2 moles D) 23.9 moles E) 41.5 moles

A) 11.5 moles

Give the theoretical yield, in grams, of CO2 from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O A) 112.7 g B) 102.4 g C) 176.0 g D) 704.0 g

A) 112.7 g

What is the coefficient for O2 when the equation is balance with smallest whole number coefficients? _____ C4H10 + _____ O2 = _____ CO2 + _____ H2O A) 13 B) 6.5 C) 1 D) 26

A) 13

What is the volume (in cm3) of a 43.6 g piece of metal with a density of 2.71 g/cm3? A) 16.1 B) 19.5 C) .425 D) 6.65 E) none of the above

A) 16.1

Calculate the molar mass of C8H6O4. A) 166.13 g/mol B) 182.09 g/mol C) 150.18 g/mol D) 172.13 g/mol

A) 166.13 g/mol

A 14.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3). If ammonia is the only product, what mass of ammonia is formed? A) 17.01 g B) 1.10 g C) 14.01 g D) 3.02 g E) 23.07 g

A) 17.01 g

An ion has 8 protons, 9 neutrons, and 10 electrons. The symbol for the ion is ________. A) 17O2- B) 17O2+ C) 19F+ D) 19F- E) 17Ne2+

A) 17O2-

What are the coefficients in front of NO3-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution: ____ NO3-(aq) + ____ Cu(s) → ____ NO(g) + ____ Cu2+(aq)? A) 2, 3 B) 2, 6 C) 3, 4 D) 3, 6

A) 2, 3

How many liters of air are in a room that measures 10.0 ft × 11.0 ft and has a(n) 8.00 ft ceiling? 1 in. = 2.54 cm (exactly); 1 L = 103 cm3. A) 2.49 × 104 B) 92.8 C) 26.8 D) 2.68 × 107 E) 8.84 × 105

A) 2.49 × 104

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl3. 2 ICl3 + 3 H2O → ICl + HIO3 + 5 HCl A) 2.78 × 1024 molecules HCl B) 1.67 × 1024 molecules HCl C) 5.02 × 1025 molecules HCl D) 6.09 × 1025 molecules HCl E) 3.65 × 1024 molecules HCl

A) 2.78 × 1024 molecules HCl

According to the following balanced reaction, how many moles of NO are formed from 8.44 moles of NO2 if there is plenty of water present? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) A) 2.81 moles NO B) 25.3 moles NO C) 8.44 moles NO D) 5.50 moles NO E) 1.83 moles NO

A) 2.81 moles NO

What is the concentration of an AlCl3 solution if 150. mL of the solution contains 450. mg of Cl- ion? A) 2.82 × 10-2 M B) 6.75 × 10-2 M C) 8.46 × 10-2 M D) 2.54 × 10-1 M

A) 2.82 × 10-2 M

Because of the high heat and low humidity in the summer in Death Valley, California, a visitor requires about one quart of water for every two miles traveled on foot. Calculate the approximate number of liters required for a person to walk 10. kilometers in Death Valley. A) 2.9 L B) 12 L C) 30 L D) 47 L

A) 2.9 L

Calculate the molar mass for Mg(ClO4)2. A) 223.21 g/mol B) 123.76 g/mol C) 119.52 g/mol D) 247.52 g/mol E) 75.76 g/mol

A) 223.21 g/mol

How many milliliters of 0.260 M Na2S are needed to react with 40.00 mL of 0.315 M AgNO3? Na2S(aq) + 2 AgNO3(aq) → 2 NaNO3(aq) + Ag2S(s) A) 24.2 mL B) 48.5 mL C) 66.0 mL D) 96.9 mL

A) 24.2 mL

How many electrons are in the ion, Cu2+? A) 27 B) 29 C) 31 D) 64

A) 27

How many electrons are in nickel? A) 28 B) 30 C) 31 D) 30.7 E) 58.7

A) 28

Calculate the mass percent composition of sulfur in Al2(SO4)3. A) 28.12% B) 9.372% C) 42.73% D) 21.38% E) 35.97%

A) 28.12%

How many phosphorus atoms are contained in 158 kg of phosphorus? A) 3.07 × 1027 phosphorus atoms B) 2.95 × 1027 phosphorus atoms C) 3.25 × 1028 phosphorus atoms D) 1.18 × 1024 phosphorus atoms E) 8.47 × 1024 phosphorus atoms

A) 3.07 × 1027 phosphorus atoms

Which of the following has the greatest mass? A) 3.88 × 1022 molecules of O2 B) 1.00 g of O2 C) 0.0312 mol of O2 D) All of the above have the same mass.

A) 3.88 × 1022 molecules of O2

If the percent yield for the following reaction is 75.0%, and 45.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq) are produced? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) A) 30.8 g B) 41.1 g C) 54.8 g D) 69.3 g

A) 30.8 g

What mass (in g) does 3.99 moles of Kr have? A) 334 g B) 476 g C) 211 g D) 240 g E) 144 g

A) 334 g

How many protons (p) and neutrons (n) are in an atom of 90/38Sr? A) 38 p, 52 n B) 38 p, 90 n C) 52 p, 38 n D) 90 p, 38 n

A) 38 p, 52 n

How many moles of CH3CH2OH are contained in 548 mL of 0.0788 M CH3CH2OH solution? A) 4.32 × 10-2 mol B) 2.32 × 10-2 mol C) 6.95 × 10-2 mol D) 1.44 × 10-2 mol E) 5.26 × 10-2 mol

A) 4.32 × 10-2 mol

Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed from 6.20 g of carbonic acid? H2CO3 → H2O + CO2 A) 4.40 g B) 8.80 g C) 2.20 g D) 6.20 g

A) 4.40 g

How many argon atoms are contained in 7.66 × 105 mmol of argon? A) 4.61 × 1026 Ar atoms B) 1.84 × 1028 Ar atoms C) 1.15 × 1028 Ar atoms D) 7.86 × 1020 Ar atoms E) 3.24 × 1026 Ar atoms

A) 4.61 × 1026 Ar atoms

Sodium metal and water react to form hydrogen and sodium hydroxide. If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide, what mass of water was involved in the reaction? A) 4.68 g B) 5.98 g C) 10.14 g D) 10.66 g

A) 4.68 g

How many moles of Kr are contained in 398 mg of Kr? A) 4.75 × 10-3 moles Kr B) 33.4 moles Kr C) 2.11 × 10-4 moles Kr D) 2.99 × 10-3 moles Kr E) 1.19 × 10-4 moles Kr

A) 4.75 × 10-3 moles Kr

Which of the following volumes is equal to 40 mL? A) 40 cm3 B) 40 dm3 C) 0.40 L D) 0.00040 kL

A) 40 cm3

Which of the following is the smallest volume? A) 44 cm3 B) 1.0 dL C) 5.5 × 103 mL D) 1.0 × 108 nL

A) 44 cm3

Calculate the atomic mass of element "X", if it has 2 naturally occurring isotopes with the following masses and natural abundances: X-45 44.8776 amu 32.88% X-47 46.9443 amu 67.12% A) 46.26 amu B) 45.91 amu C) 46.34 amu D) 46.84 amu E) 44.99 amu

A) 46.26 amu

Calculate the mass, in kg, of 4.87 × 1025 atoms of Zn. A) 5.29 kg B) 1.89 kg C) 8.09 kg D) 1.24 kg E) 1.09 kg

A) 5.29 kg

How many protons (p) and neutrons (n) are in an atom of barium-130? A) 56 p, 74 n B) 56 p, 130 n C) 74 p, 56 n D) 130 p, 56 n

A) 56 p, 74 n

What is the molar mass of 1-butene if 5.38 × 1016 molecules of 1-butene weigh 5.00 μg? A) 56.0 g/mol B) 178 g/mol C) 224 g/mol D) 447 g/mol

A) 56.0 g/mol

An atom of 14C contains ________ protons. A) 6 B) 20 C) 8 D) 10 E) 14

A) 6

Calculate the mass (in ng) of 2.33 × 1020 atoms of oxygen. A) 6.19 × 106 ng B) 1.62 × 107 ng C) 2.25 × 103 ng D) 3.73 × 106 ng E) 4.69 × 107 ng

A) 6.19 × 106 ng

How many atoms of oxygen are in 5.00 g of ethanol, C2H6O? A) 6.52 × 1022 B) 6 C) 5.52 × 1024 D) 6.02 × 1023

A) 6.52 × 1022

The mass of a He atom is ________. A) 6.64 × 10-24 g B) 4.003 g C) 2.40 × 1024 g D) 6.64 × 1022 g

A) 6.64 × 10-24 g

Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. ____ NH3(g) + ____ O2(g) → ____ NO(g) + ____ H2O(l) A) 7.32 L B) 11.1 L C) 11.5 L D) 17.3 L

A) 7.32 L

Gallium has an atomic mass of 69.723 amu. The Ga-69 isotope (68.926 amu) is 60.11%. What is the amu of the other isotope? A) 70.924 amu B) 70.928 amu C) 70.932 amu D) 70.920 amu

A) 70.924 amu

When silver nitrate reacts with barium chloride, silver chloride and barium nitrate are formed. How many grams of silver chloride are formed when 10.0 g of silver nitrate reacts with 15.0 g of barium chloride? A) 8.44 g B) 9.40 g C) 11.9 g D) 18.8 g

A) 8.44 g

How many C2H4 molecules are contained in 45.8 mg of C2H4? The molar mass of C2H4 is 28.05 g/mol. A) 9.83 × 1020 C2H4 molecules B) 7.74 × 1026 C2H4 molecules C) 2.71 × 1020 C2H4 molecules D) 3.69 × 1023 C2H4 molecules E) 4.69 × 1023 C2H4 molecules

A) 9.83 × 1020 C2H4 molecules

According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed? 2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l) A) 99.8 g S B) 66.6 g S C) 56.1 g S D) 44.4 g S E) 14.0 g S

A) 99.8 g S

Which of the following statements about subatomic particles is true? A) A neutral atom contains the same number of protons and electrons. B) Protons have about the same mass as electrons. C) Electrons make up most of the mass of an atom. D) Protons and neutrons have opposite, but equal in magnitude, charges. E) Neutrons and electrons are found in the nucleus of an atom.

A) A neutral atom contains the same number of protons and electrons.

Choose the statement below that is true. A) A weak acid solution consists of mostly nonionized acid molecules. B) The term "strong electrolyte" means that the substance is extremely reactive. C) A strong acid solution consists of only partially ionized acid molecules. D) The term "weak electrolyte" means that the substance is inert. E) A molecular compound that does not ionize in solution is considered a strong electrolyte.

A) A weak acid solution consists of mostly nonionized acid molecules.

Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s) A) Ag B) Ni C) Cl D) O E) This is not an oxidation-reduction reaction.

A) Ag

What species is represented by the following information? p+ = 47 n° = 62 e- = 46 A) Ag+ B) Nd C) Pd D) Ag E) Pd+

A) Ag+

What reagent could be used to separate Br- from CH3CO2- when added to an aqueous solution containing both? A) AgNO3(aq) B) Ba(OH)2(aq) C) CuSO4(aq) D) NaI(aq)

A) AgNO3(aq)

What reagent could not be used to separate Br- from CO32- when added to an aqueous solution containing both? A) AgNO3(aq) B) Ca(NO3)2(aq) C) Cu(NO3)2(aq) D) Fe(NO3)2(aq)

A) AgNO3(aq)

Which of the following elements is a noble gas? A) Ar B) Br C) N D) O E) K

A) Ar

Which of the following statements is not correct? A) Atoms are invisible. B) Atoms are made of subatomic particles. C) Each element contains different atoms. D) An atom has mass.

A) Atoms are invisible.

What is the element symbol for an atom that has 5 protons and 6 neutrons? A) B B) C C) H D) Na

A) B

The mixing of which pair of reactants will result in a precipitation reaction? A) Ba(NO3)2(aq) + Na2CO3(aq) B) K2SO4(aq) + Cu(NO3)2(aq) C) NaClO4(aq) + (NH4)2S(aq) D) NH4Br(aq) + NH4I(aq)

A) Ba(NO3)2(aq) + Na2CO3(aq)

Which set has the same number of protons? A) Br, Br-, Br+ B) N, O, F C) Na+, Mg2+, Al3+ D) K+, Rb+, Cs+

A) Br, Br-, Br+

What is the empirical formula of a substance that contains 2.64 g of C, 0.444 g of H, and 3.52 g of O? A) C H2O B) C2H4O2 C) C2H4O3 D) C3H4O4

A) C H2O

Determine the empirical formula for a compound that is 70.79% carbon, 8.91% hydrogen, 4.59% nitrogen, and 15.72% oxygen. A) C18H27NO3 B) C18H27NO2 C) C17H27NO3 D) C17H26NO3

A) C18H27NO3

What is the empirical formula for C4H10O2? A) C2H5O B) CHO C) C2H4O D) CHO2 E) CH2O

A) C2H5O

Determine the empirical formula for a compound that contains C, H and O. It contains 51.59% C and 35.30% O by mass. A) C2H6O B) CHO C) C4H13O2 D) CH4O3 E) CH3O

A) C2H6O

Choose the reaction that represents the combustion of C6H12O2. A) C6H12O2(l) + 8 O2(g) → 6 CO2(g) + 6 H2O(g) B) Mg(s) + C6H12O2(l) → MgC6H12O2(aq) C) 6 C(s) + 6 H2(g) + O2(g) → C6H12O2(l) D) C6H12O2(l) → 6 C(s) + 6 H2(g) + O2(g) E) None of the above represent the combustion of C6H12O2.

A) C6H12O2(l) + 8 O2(g) → 6 CO2(g) + 6 H2O(g)

Write a possible molecular formula for C4H4O. A) C8H8O2 B) C12H12O2 C) C2H2O D) C8H8O

A) C8H8O2

Which of the following is one possible form of pentane? A) CH3CH2CH2CH2CH3 B) CH3CH=CHCH2CH3 C) CH3CH2CH2CH2CH2CH3 D) CH3CH2CH2CH2CH2NH2 E) CH3CH2-O-CH2CH2CH3

A) CH3CH2CH2CH2CH3

Identify the compound with covalent bonds. A) CH4 B) Kr C) KBr D) Li E) NaCl

A) CH4

Which of the compounds H2C2O4, Ca(OH)2, KOH, and HI, behave as bases when they are dissolved in water? A) Ca(OH)2 and KOH B) H2C2O4 and HI C) only HI D) only KOH

A) Ca(OH)2 and KOH

Which of the following compounds is soluble in water? A) CaS B) MgCO3 C) PbCl2 D) BaSO4 E) None of these compounds is soluble in water.

A) CaS

Which of the following assumptions of Dalton's Atomic Theory are no longer valid? A) Each element is composed of atoms. B) All atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements. C) Atoms combine in simple, whole-number ratios to form compounds. D) Atoms of one element cannot change into atoms of another element.

A) Each element is composed of atoms.

In which of the following sets do all species have the same number of electrons? A) F-, Ne, Mg2+ B) Ge, Se2-, Br- C) K+, Rb+, Cs+ D) Br, Br-, Br+

A) F-, Ne, Mg2+

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 and KOH are mixed. A) H+(aq) + OH-(aq) → H2O(l) B) 2 K+(aq) + SO42-(aq) → K2SO4(s) C) H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + K2SO4(s) D) H22+(aq) + OH-(aq) → H2(OH)2(l) E) No reaction occurs.

A) H+(aq) + OH-(aq) → H2O(l)

Give the formula for sulfurous acid. A) H2SO3 B) HSO3 C) H2SO4 D) HSO4

A) H2SO3

Identify the formula for nitric acid. A) HNO3 B) HNO2 C) HNO D) HNO4

A) HNO3

Which of the following compounds is insoluble in water? A) Hg2I2 B) MgSO4 C) (NH4)2CO3 D) BaS E) All of these compounds are soluble in water.

A) Hg2I2

Which of the following is an ionic compound? A) LiCl B) NO2 C) PCl3 D) CF4 E) SeBr2

A) LiCl

What is the chemical formula for magnesium hydride? A) MgH2 B) MgOH C) MgOH2 D) Mg(OH)2

A) MgH2

Which of the following is considered a strong electrolyte? A) NH4NO3 B) C12H22O11 C) PbCl2 D) HC2H3O2 E) CH3OH

A) NH4NO3

Write the formula for strontium nitride. A) Sr3N2 B) Sr(NO3)2 C) SrN D) Sr2N3 E) Sr(NO2)2

A) Sr3N2

Which one of the following compounds contains ionic bonds? A) SrO B) HBr C) PBr3 D) SiO2

A) SrO

Which of the following elements is an actinide? A) U B) Pm C) Rf D) Po

A) U

Which glassware is best to measure 10.5 mL of a liquid? A) a graduated buret (with marking every 0.1 mL) B) a graduated cylinder (with marking every 1 mL) C) a fixed volume pipet (with only one marking) D) a graduated beaker (with marking every 10 mL )

A) a graduated buret (with marking every 0.1 mL)

Cesium belongs to the ________ group of the periodic table. A) alkali metal B) alkaline earth metal C) halogen D) noble gas

A) alkali metal

Identify a cation. A) an atom that has lost an electron B) an atom that has gained an electron C) an atom that has lost a proton D) an atom that has gained a proton

A) an atom that has lost an electron

All of the following elements are nonmetals except A) barium. B) carbon. C) hydrogen. D) oxygen.

A) barium.

What type of bonding is found in the compound OF2? A) covalent bonding B) hydrogen bonding C) ionic bonding D) metallic bonding

A) covalent bonding

Determine the name for N2O5. A) dinitrogen pentoxide B) nitrogen oxide C) nitrogen (IV) oxide D) nitrogen (II) oxide E) nitrogen tetroxide

A) dinitrogen pentoxide

An aqueous solution of H2S is named A) hydrosulfuric acid. B) hydrosulfurous acid. C) sulfuric acid. D) sulfurous acid.

A) hydrosulfuric acid.

Semiconductors usually are A) metalloids. B) noble gases. C) nonmetals. D) metals.

A) metalloids.

What does "X" represent in the following symbol? 28/14X A) silicon B) sulfur C) zinc D) ruthenium E) nickel

A) silicon

What element is defined by the following information? p+ = 11 n° = 12 e- = 11 A) sodium B) vanadium C) magnesium D) titanium

A) sodium

A covalent bond is best described as A) the sharing of electrons between atoms. B) the transfer of electrons. C) a bond between a metal and a nonmetal. D) a bond between a metal and a polyatomic ion. E) a bond between two polyatomic ions.

A) the sharing of electrons between atoms.

Determine the name for TiCO3. Remember that titanium forms several ions. A) titanium (II) carbonate B) titanium carbide C) titanium carbonite D) titanium (II) carbonite E) titanium (I) carbonate

A) titanium (II) carbonate

Describe an atom and what it is made up of according to modern atomic theory.

An atom is made up of a nucleus surrounded by electrons. The nucleus contains protons (positively charged particles) and neutrons (neutral particles) and is where most of the mass of an atom comes from, but is a tiny fraction of an atom's volume. The nucleus is surrounded by negatively charged electrons, the same number as there are protons in the nucleus. An atom is therefore neutral overall.

Describe the difference between an intensive and extensive property using examples

An intensive property does not depend on the amount of the substance present, such as temperature or density. An extensive property is one that does depend on the amount of the substance, such as mass or volume.

Describe the difference between ionic and molecular compounds. Give an example of each.

An ionic compound is formed between a metal and a nonmetal (or polyatomic ions) and is held together through the attraction of opposite charges. An example is NaCl. A molecular compound is usually formed between 2 or more nonmetals and is held together through the sharing of electrons between atoms. An example is CO2.

How can one compound contain both ionic and covalent bonds? Give an example.

An ionic compound that contains a polyatomic ion, such as NaNO3, has both ionic bonds (that hold the sodium and nitrate ions together) as well as covalent bonds (that hold the atoms within the nitrate ion together).

Are anions typically larger or smaller than their corresponding atom? Why?

Anions are larger than their corresponding atom because the anion contains more electrons than the atom. Since electrons repel one another and determine the size of the atom or ion, adding electrons to the atom to form an anion makes it larger.

What element is defined by the following information? p+ = 20 n° = 20 e- = 20 A) zirconium B) calcium C) potassium D) neon E) argon

B) calcium

How can you tell if a reaction is an oxidation-reduction reaction?

At least one species is losing electrons while at least one other species is gaining electrons. This can be evaluated by assigning oxidation numbers to each element present and looking to see if these change from reactant to product.

Describe the difference between an atomic element and a molecular element.

Atomic elements exist in nature with a single atom at their basic unit; molecular elements exist in nature with more than one atom as their basic unit.

Determine the oxidation state of Sn in Sn(SO4)2. A) +2 B) +4 C) +6 D) 0 E) -2

B) +4

What is the oxidation number of the oxygen atom in Rb2O2? A) -2 B) -1 C) +1 D) +2

B) -1

What is the oxidation number change for the bromine atom in the following unbalanced reduction half reaction: BrO3-(aq) + H+(aq) → Br-(aq) + H2O(l)? A) -7 B) -6 C) +6 D) +7

B) -6

Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution. A) 0.0297 M B) 0.0337 M C) 0.0936 M D) 0.0107 M E) 0.0651 M

B) 0.0337 M

How many moles are there in 3.00 g of ethanol, CH3CH2OH? A) 0.00725 mol B) 0.0652 mol C) 15.3 mol D) 138 mol

B) 0.0652 mol

What is the concentration of FeCl3 in a solution prepared by dissolving 20.0 g of FeCl3 in enough water to make 275 mL of solution? A) 4.48 × 10-4 M B) 0.448 M C) 2.23 M D) 2.23 × 103 M

B) 0.448 M

What volume of a 0.540 M NaOH solution contains 11.5 g of NaOH? A) 0.155 L B) 0.532 L C) 1.88 L D) 6.44 L

B) 0.532 L

If 100. mL of 0.400 M Na2SO4 is added to 200. mL of 0.600 M NaCl, what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive. A) 0.534 M B) 0.667 M C) 1.00 M D) 1.40 M

B) 0.667 M

How many moles of NaCl are required to make 250 mL of a 3.00 M solution? A) 750 moles B) 0.750 moles C) 3 moles D) 0.250 moles

B) 0.750 moles

What is the mass of a sample of water (H2O) containing 3.00 × 1022 H2O molecules? A) 18.0 g B) 0.900 g C) 9.00 g D) 1.00 mol

B) 0.900 g

What mass of carbon dioxide, CO2, contains the same number of molecules as 3.00 g of trichlorofluoromethane, CCl3F? A) 0.106 g B) 0.961 g C) 1.04 g D) 9.37 g

B) 0.961 g

Which of the following is the greatest mass? A) 1000 μg B) 1.000 × 10-4 kg C) 1.000 × 10-4 cg D) 1.000 × 10-8 mg

B) 1.000 × 10-4 kg

The mass of a single zinc atom is 1.086 × 10-22 g. This is the same mass as A) 1.086 × 10-16 mg. B) 1.086 × 10-25 kg. C) 1.086 × 10-28 μg. D) 1.086 × 10-31 ng.

B) 1.086 × 10-25 kg.

How many cations are there in 10.0 g of sodium phosphate? A) 3.67 × 1022 cations B) 1.10 × 1023 cations C) 9.87 × 1024 cations D) 2.96 × 1025 cations

B) 1.10 × 1023 cations

How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride? CaCl2(aq) + K2CO3(aq) → 2 KCl(aq) + CaCO3(aq) A) 0.896 g B) 1.12 g C) 2.23 g D) 4.47 g

B) 1.12 g

The average distance between nitrogen and oxygen atoms is 115 pm in a compound called nitric oxide. What is this distance in millimeters? A) 1.15 × 10-8 mm B) 1.15 × 10-7 mm C) 1.15 × 1013 mm D) 1.15 × 1017 mm

B) 1.15 × 10-7 mm

How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3 mL of 0.140 M sucrose solution? A) 8.29 × 1022 molecules C12H22O11 B) 1.21 × 1021 molecules C12H22O11 C) 6.15 × 1022 molecules C12H22O11 D) 1.63 × 1023 molecules C12H22O11 E) 5.90 × 1024 molecules C12H22O11

B) 1.21 × 1021 molecules C12H22O11

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of oxygen are formed when 10.0 g of dinitrogen monoxide decomposes? A) 0.275 g B) 3.64 g C) 7.27 g D) 14.5 g

B) 3.64 g

Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO2(g) + H2O(l) → HNO3(l) + NO(g) Suppose that 4 mol NO2 and 2 H2O mol combine and react completely. How many moles of NO are produced after the reaction has completed? A) 2 B) 1.33 C) 3 D) 4

B) 1.33

How many anions are there in 2.50 g of MgBr2? A) 8.18 × 1021 anions B) 1.64 × 1022 anions C) 4.43 × 1025 anions D) 8.87 × 1025 anions

B) 1.64 × 1022 anions

Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum. ____ Al(s) + ____ I2(s) → ____ Al2I6(s) A) 0.741 mol B) 1.67 mol C) 2.22 mol D) 3.33 mol

B) 1.67 mol

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen? A) 0.30 B) 1.8 C) 0.20 D) 0.40 E) 3.6

B) 1.8

A fishing boat accidentally spills 3.0 barrels of diesel oil into the ocean. Each barrel contains 42 gallons. If the oil film on the ocean is 2.5 × 102 nm thick, how many square meters will the oil slick cover? A) 1.9 × 10-3 m2 B) 1.9 × 106 m2 C) 1.9 × 107 m2 D) none of these

B) 1.9 × 106 m2

How many electrons does the Al3+ ion possess? A) 16 B) 10 C) 6 D) 0 E) 13

B) 10

Which of the following contains the most atoms? You shouldn't need to do a calculation here. A) 10.0 g Ne B) 10.0 g He C) 10.0 g Ar D) 10.0 g Kr E) 10.0 g Mg

B) 10.0 g He

A sample of pure lithium nitrate contains 10.1% lithium by mass. What is the % lithium by mass in a sample of pure lithium nitrate that has twice the mass of the first sample? A) 5.05% B) 10.1% C) 20.2% D) 40.4%

B) 10.1%

According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H2O? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g) A) 5.44 moles H2O B) 10.9 moles H2O C) 21.8 moles H2O D) 2.72 moles H2O E) 1.36 moles H2O

B) 10.9 moles H2O

The atomic mass for cadmium is ________. A) 48 B) 112.41 C) 40.08 D) 20

B) 112.41

Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 45.00 mL of 0.00150 M calcium hydroxide. ____ Ca(OH)2(aq) + ____ H3PO4(aq) → ____ Ca3(PO4)2(aq) + ____ H2O(l) A) 3.04 mL B) 15.0 mL C) 22.5 mL D) 33.8 mL

B) 15.0 mL

Calculate the mass percent composition of lithium in Li3PO4. A) 26.75% B) 17.98% C) 30.72% D) 55.27% E) 20.82%

B) 17.98%

How many electrons are in the ion, P3-? A) 12 B) 18 C) 28 D) 34

B) 18

Aluminum metal reacts with aqueous iron(II) chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients? A) 1 B) 2 C) 3 D) 4

B) 2

Which of the following is an acid base reaction? A) C(s) + O2(g) → CO2(g) B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq) C) Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq) D) MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s) E) None of the above are acid base reactions.

B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq)

Which of the following elements is classified as a semimetal? A) calcium B) boron C) fluorine D) uranium

B) boron

How many silver atoms are contained in 3.75 moles of silver? A) 6.23 × 1024 silver atoms B) 2.26 × 1024 silver atoms C) 1.61 × 1023 silver atoms D) 2.44 × 1026 silver atoms E) 6.50 × 1025 silver atoms

B) 2.26 × 1024 silver atoms

How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen. 6 Li(s) + N2(g) → 2 Li3N(s) A) 18.3 g Li3N B) 20.3 g Li3N C) 58.3 g Li3N D) 61.0 g Li3N E) 15.1 g Li3N

B) 20.3 g Li3N

How many moles of PCl3 contain 3.68 × 1025 chlorine atoms? A) 61.1 moles PCl3 B) 20.4 moles PCl3 C) 16.4 moles PCl3 D) 54.5 moles PCl3 E) 49.1 moles PCl3

B) 20.4 moles PCl3

Calculate the molar mass of Al(C2H3O2)3. A) 86.03 g/mol B) 204.13 g/mol C) 56.00 g/mol D) 258.09 g/mol E) 139.99 g/mol

B) 204.13 g/mol

How many milliliters of a stock solution of 11.1 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3? A) 0.0444 mL B) 22.5 mL C) 2.78 mL D) 44.4 mL E) 0.0225 mL

B) 22.5 mL

When 11.0 g of calcium metal is reacted with water, 5.00 g of calcium hydroxide is produced. Using the following balanced equation, calculate the percent yield for the reaction? Ca(s) + 2 H2O(l) → Ca(OH)2(aq) + H2(g) A) 12.3% B) 24.6% C) 45.5% D) 84.0%

B) 24.6%

Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O A) 20.00% B) 25.00% C) 88.90% D) 22.20%

B) 25.00%

A FeCl3 solution is 0.175 M. How many mL of a 0.175 M FeCl3 solution are needed to make 450. mL of a solution that is 0.300 M in Cl- ion? A) 0.771 mL B) 257 mL C) 771 mL D) It is not possible to make a more concentrated solution from a less concentrated solution.

B) 257 mL

What is the molar mass of nitrogen gas? A) 14.0 g/mol B) 28.0 g/mol C) 6.02 × 1023 g/mol D) 1.20 × 1023 g/mol

B) 28.0 g/mol

The U.S. Mint produced pure silver quarter commemorative coins in 1992, each coin weighing 5.67 g. How many silver atoms are present in each coin? A) 6.02 × 1023 B) 3.15 × 1022 C) 1.14 × 1023 D) 1.14 × 10-23

B) 3.15 × 1022

The width, length, and height of a large, custom-made shipping crate are 1.22 m, 3.22 m, and 0.83 m, respectively. The volume of the box using the correct number of significant figures is ________ m3. A) 3.26057 B) 3.3 C) 3.26 D) 3.261 E) 3.2606

B) 3.3

Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g) A) 1.55 moles O2 B) 3.50 moles O2 C) 2.33 moles O2 D) 4.14 moles O2 E) 6.21 moles O2

B) 3.50 moles O2

According to the following reaction, what mass of PbCl2 can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO3)2. 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) A) 7.19 g B) 3.59 g C) 1.80 g D) 5.94 g E) 1.30 g

B) 3.59 g

How many electrons are in a neutral atom of bromine-81? A) 1 B) 35 C) 36 D) 81

B) 35

The atomic number of an atom of 80Br is ________. A) 115 B) 35 C) 45 D) 73 E) 80

B) 35

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: Pb2+(aq) + 2I-(aq) → PbI2(s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 0.700 mol of Pb(NO3)2(aq) to completely precipitate the lead? A) 2.54 × 10-3 mL B) 394 mL C) 197 mL D) 0.197 mL E) 0.394 mL

B) 394 mL

Convert 4 μm to meters. A) 4 × 10-9 m B) 4 × 10-6 m C) 4 × 10-3 m D) 4 × 106 m

B) 4 × 10-6 m

How many moles of Cs are contained in 595 kg of Cs? A) 2.23 × 102 moles Cs B) 4.48 × 103 moles Cs C) 7.91 × 104 moles Cs D) 1.26 × 103 moles Cs E) 5.39 × 102 moles Cs

B) 4.48 × 103 moles Cs

How many milliliters of a 0.266 M LiNO3 solution are required to make 150.0 mL of 0.075 M LiNO3 solution? A) 53.2 mL B) 42.3 mL C) 18.8 mL D) 23.6 mL E) 35.1 mL

B) 42.3 mL

How many milliliters of a 0.266 M NaNO3 solution are required to make 150.0 mL of 0.075 M NaNO3 solution? A) 53.2 mL B) 42.3 mL C) 18.8 mL D) 23.6 mL E) 35.1 mL

B) 42.3 mL

What is the mass, in kg, of 6.89 × 1025 molecules of CO2? The molar mass of CO2 is 44.01 g/mol. A) 3.85 kg B) 5.04 kg C) 2.60 kg D) 3.03 kg E) 6.39 kg

B) 5.04 kg

What is the concentration of HCl in the final solution when 65 mL of a 12 M HCl solution is diluted with pure water to a total volume of 0.15 L? A) 2.8 × 10-2 M B) 5.2 M C) 28 M D) 5.2 × 103 M

B) 5.2 M

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl3). If it is the only product, what mass of PCl3 is formed? A) 30.15 g B) 54.93 g C) 140.01 g D) 79.71 g E) 91.86 g

B) 54.93 g

Which of the following is the lowest temperature? A) 42°C B) 57°F C) 318 K D) All of these temperatures are all equal.

B) 57°F

What is the mass of a single fluorine molecule, F2? A) 3.155 × 10-23 g B) 6.310 × 10-23 g C) 19.00 g D) 38.00 g

B) 6.310 × 10-23 g

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O2(g) → 2MgO(s) When 4.00 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g. A) 4.00 B) 6.63 C) 0.165 D) 3.32 E) 13.3

B) 6.63

What is the mass of 0.500 mol of dichlorodifluoromethane, CCl2F2? A) 4.14 × 10-3 g B) 60.5 g C) 121 g D) 242 g

B) 60.5 g

How many Fe(II) ions are there in 20.0 g of FeSO4? A) 2.19 × 10-25 iron(II) ions B) 7.92 × 1022 iron(II) ions C) 4.57 × 1024 iron(II) ions D) 1.82 × 1027 iron(II) ions

B) 7.92 × 1022 iron(II) ions

Give the mass percent of carbon in C14H19NO2. A) 38.89% B) 72.07% C) 5.17% D) 2.78%

B) 72.07%

How many molecules of H2S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO2. 2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l) A) 1.48 × 1024 molecules H2S B) 9.89 × 1023 molecules H2S C) 5.06 × 1025 molecules H2S D) 3.17 × 1025 molecules H2S E) 2.44 × 1023 molecules H2S

B) 9.89 × 1023 molecules H2S

If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed to produce 15.0 g of CO2 according to the following chemical equation? C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) A) 6.19 mL B) 9.95 mL C) 19.9 mL D) 39.8 mL

B) 9.95 mL

Which of the following represent isotopes? A: 32/15X B: 32/16X C: 31/15X D: 34/17X A) A and B B) A and C C) A and D D) C and D

B) A and C

What is the net ionic reaction for the following reaction in aqueous solutions: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) A) AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) B) Ag+(aq) + Cl-(aq) → AgCl(s) C) Ag+(aq) +NO3-(aq) +Na+(aq) + Cl- (aq) → Ag+(aq) +NO3-(aq) + Na+(aq) + Cl- (aq) D) Ag+(aq) +NO3-(aq) +Na+(aq) + Cl- (aq) → AgCl(s) +Na+(aq) + NO3-(aq)

B) Ag+(aq) + Cl-(aq) → AgCl(s)

What precipitate is most likely formed from a solution containing Ba+2, Na+1, OH-1, and CO3-2. A) NaOH B) BaCO3 C) Na2CO3 D) Ba(OH)2

B) BaCO3

Combustion analysis of an unknown compound containing only carbon and hydrogen produced 0.2845 g of CO2 and 0.1451 g of H2O. What is the empirical formula of the compound? A) CH2 B) C2H5 C) C4H10 D) C5H2

B) C2H5

Which substance is oxidized in the following reaction? 5C2O42- + 2MnO4- + 16H+ → 10 CO2 + 2Mn2+ + 4H2O) A) 2MnO4- B) C2O42- C) H+ D) none

B) C2O42-

Which of the compounds C4H10, BaCl2, Ni(NO3)2, SF6 are expected to exist as molecular compounds? A) only C4H10 B) C4H10 and SF6 C) C4H10, Ni(NO3)2, and SF6 D) BaCl2 and Ni(NO3)2

B) C4H10 and SF6

Determine the molecular formula of a compound that has a molar mass of 183.2 g/mol and an empirical formula of C2H5O2. A) C2H5O2 B) C6H15O6 C) C3H7O3 D) C4H10O4 E) C8H20O8

B) C6H15O6

Which of the following compounds is not an Arrhenius acid? A) CH3CO2H B) CH3CH2NH2 C) HNO2 D) H2SO4

B) CH3CH2NH2

What species is represented by the following information? p+ = 17 n° = 18 e- = 18 A) Cl B) Cl- C) Ar D) Ar+ E) Kr

B) Cl-

Which of the following elements is a metalloid? A) Al B) Ge C) C D) Sn

B) Ge

The chemical formula for nitrous acid is A) H3N(aq). B) H NO2(aq). C) H NO3(aq). D) H2N2O6(aq).

B) H NO2(aq).

Which of the compounds of H2C2O4, Ca(OH)2, KOH, and HI, behave as acids when they are dissolved in water? A) Ca(OH)2 and KOH B) H2C2O4 and HI C) only HI D) only KOH

B) H2C2O4 and HI

Write a balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite. A) H2SO4(aq) + LiOH(aq) → H2O(l) + Li2SO4(aq) B) H2SO3(aq) + 2 LiOH(aq) → 2 H2O(l) + Li2SO3(aq) C) HSO3(aq) + LiOH(aq) → H2O(l) + LiSO3(aq) D) HSO4(aq) + LiOH(aq) → H2O(l) + LiSO4(aq) E) H2S(aq) + 2 LiOH(aq) → 2 H2O(l) + Li2S(aq)

B) H2SO3(aq) + 2 LiOH(aq) → 2 H2O(l) + Li2SO3(aq)

Which of the following pairs of aqueous solutions will react to produce a precipitate? A) NH4NO3 + Li2CO3 B) Hg2(NO3)2 + LiI C) NaCl + Li3PO4 D) AgC2H3O2 + Cu(NO3)2 E) None of the above solution pairs will produce a precipitate.

B) Hg2(NO3)2 + LiI

What is the empirical formula for Hg2(NO3)2? A) Hg2(NO3)2 B) HgNO3 C) Hg(NO3)2 D) Hg2NO3 E) Hg4(NO3)4

B) HgNO3

Identify the spectator ions in the following molecular equation. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq) A) Ag+ & Br- B) K+ & NO3- C) K+ & Br- D) Ag+ & NO3- E) There are no spectator ions in this reaction.

B) K+ & NO3-

Which of the following is an ionic compound? A) SCl2 B) Mg3(PO4)2 C) Cl2O D) CH2O E) PF5

B) Mg3(PO4)2

The solid compound, Na4SiO4, contains A) Na+, Si4+, and O2- ions. B) Na+ and SiO44- ions. C) Na4+ and SiO44- ions. D) Na4SiO4 molecules.

B) Na+ and SiO44- ions.

Which of the following elements is a lanthinide? A) U B) Pm C) Rf D) Po

B) Pm

You are given three solid compounds (A, B, C) with melting temperatures 700°C, 150°C and 800°C respectively. Which of these is a molecular solid? A) Solid A B) Solid B C) Solid C D) Solids A, B, C

B) Solid B

In which set do all elements tend to form cations in binary ionic compounds? A) K, Ga, O B) Sr, Ni, Hg C) N, P, Bi D) O, Br, I

B) Sr, Ni, Hg

Which of the following statements is false? A) Halogens are very reactive elements. B) The alkali metals are fairly unreactive. C) Sulfur is a main group element. D) Noble gases do not usually form ions. E) Zn is a transition metal.

B) The alkali metals are fairly unreactive.

What is the chemical symbol for titanium? A) Th B) Ti C) Tl D) Tm

B) Ti

Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain three times as much Cl-35 as Cl-37. B) Two different compounds formed from carbon and oxygen have the following mass ratios: 1.33 g O: 1 g C and 2.66 g O: 1 g C. C) Two different samples of table salt are found to have the same ratio of sodium to chlorine. D) The atomic mass of bromine is found to be 79.90 amu. E) Nitrogen dioxide always has a mass ratio of 2.28 g O: 1 g N.

B) Two different compounds formed from carbon and oxygen have the following mass ratios: 1.33 g O: 1 g C and 2.66 g O: 1 g C.

Barium belongs to the ________ group of the periodic table. A) alkali metal B) alkaline earth metal C) halogen D) noble gas

B) alkaline earth metal

Identify an anion. A) an atom that has lost an electron B) an atom that has gained an electron C) an atom that has lost a neutron and a proton D) an atom that has gained a neutron

B) an atom that has gained an electron

Which are isotopes? An atom that has an atomic number of 20 and a mass number of 42 is an isotope of an atom that has A) an atomic number of 21 and a mass number of 42. B) an atomic number of 20 and a mass number of 40. C) 22 neutrons and 20 protons. D) 22 protons and 20 neutrons.

B) an atomic number of 20 and a mass number of 40.

When 280. mL of 1.50 × 10-4 M hydrochloric acid is added to 135 mL of 1.75 × 10-4 M Mg(OH)2, the resulting solution will be A) acidic. B) basic C) neutral. D) It is impossible to tell from the information given.

B) basic

The ion, IO2-, is named A) iodate ion. B) iodite ion. C) iodine dioxide ion. D) iodine(II) oxide ion.

B) iodite ion.

Which of the compounds, Li3N, NH3, C3H8, IF3 are ionic compounds? A) only C3H8 B) only Li3N C) Li3N and NH3 D) N H3, C3H8, and IF3

B) only Li3N

Determine the number of protons, neutrons and electrons in the following: 40/18X A) p+ = 18 n° = 18 e- = 22 B) p+ = 18 n° = 22 e- = 18 C) p+ = 22 n° = 18 e- = 18 D) p+ = 18 n° = 22 e- = 40 E) p+ = 40 n° = 22 e- = 18

B) p+ = 18 n° = 22 e- = 18

Rb2S is named A) rubidium disulfide. B) rubidium sulfide. C) rubidium(II) sulfide. D) rubidium sulfur.

B) rubidium sulfide.

Which element has the chemical symbol, Ru? A) rubidium B) ruthenium C) rutherfordium D) rhodium

B) ruthenium

Give the name for NaNO3. A) sodium nitrite B) sodium nitrate C) sodium pernitrate D) sodium hyponitrite E) sodium hyponitrate

B) sodium nitrate

An ionic bond is best described as A) the sharing of electrons. B) the transfer of electrons from one atom to another. C) the attraction that holds the atoms together in a polyatomic ion. D) the attraction between 2 nonmetal atoms. E) the attraction between 2 metal atoms.

B) the transfer of electrons from one atom to another.

Give the name for SnO. A) tin (I) oxide B) tin (II) oxide C) tin (III) oxide D) tin (IV) oxide

B) tin (II) oxide

Write the name for Sn(SO4)2. Remember that Sn forms several ions. A) tin (I) sulfite B) tin (IV) sulfate C) tin sulfide D) tin (II) sulfite E) tin (I) sulfate

B) tin (IV) sulfate

What is the oxidation number of the chromium atom in Na2CrO4? A) -2 B) +2 C) +6 D) +7

C) +6

Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M Ca(NO3)2 solution to 150.0 mL. A) 1.13 M B) 0.0887 M C) 0.0313 M D) 0.0199 M E) 0.0501 M

C) 0.0313 M

Which of the following solutions will have the highest concentration of chloride ions? A) 0.10 M NaCl B) 0.10 M MgCl2 C) 0.10 M AlCl3 D) 0.05 M CaCl2 E) All of these solutions have the same concentration of chloride ions.

C) 0.10 M AlCl3

The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M KOH solution. What is the concentration of the H3PO4 solution (in M)? A) 1.03 M B) 0.343 M C) 0.114 M D) 0.138 M E) 0.0461 M

C) 0.114 M

If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350. mL of solution? A) 0.0101 M B) 0.0404 M C) 0.162 M D) 0.323 M

C) 0.162 M

Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: Ag+(aq) + Cl-(aq) → AgCl(s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.366 M AgNO3 solution to completely precipitate the silver? A) 9.15 × 10-3 g B) 1.57 × 10-4 g C) 0.535 g D) 0.157 g E) 6.39 × 103 g

C) 0.535 g

A stock solution of HNO3 is prepared and found to contain 13.5 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M. A) 0.270 B) 1.48 C) 0.675 D) 675 E) 270

C) 0.675

Without using a calculator, solve the following problem: [(1x10^-8) x (1 x 10^5)]^2 / (1 x 10^6) A) 1 × 106 B) 1 × 100 C) 1 × 10-12 D) 1 × 10-18

C) 1 × 10-12

The diameter of an atom is approximately 1 × 10-10 m. What is the diameter in millimeters? A) 1 × 10-16 mm B) 1 × 10-13 mm C) 1 × 10-7 mm D) 1 × 10-4 mm

C) 1 × 10-7 mm

Without using a calculator, solve the following problem: [(1x10^4)x(1x10^3)]^2 / (1 x 10^-9) A) 1 × 10-4 B) 1 × 105 C) 1 × 1023 D) 1 × 1032

C) 1 × 1023

How many moles of C3H8 contain 4.95 × 1024 hydrogen atoms? A) 8.22 moles C3H8 B) 6.58 moles C3H8 C) 1.03 moles C3H8 D) 9.73 moles C3H8 E) 3.09 moles C3H8

C) 1.03 moles C3H8

Based on the balanced chemical equation shown below, determine the molarity of a solution containing Fe2+(aq), if 40.00 mL of the Fe2+(aq) solution is required to completely react with 30.00 mL of a 0.250 M potassium bromate, KBrO3(aq), solution. The chemical equation for the reaction is 6 Fe2+(aq) + BrO3-(aq) + 6 H+(aq) → 6 Fe3+(aq) + Br-(aq) + 3 H2O(l). A) 0.0312 M B) 0.188 M C) 1.12 M D) 2.00 M

C) 1.12 M

What is the concentration of ions in a 0.25 M Al2(CO3)3 solution? A) 0.25 M B) 1.00 M C) 1.25 M D) 0.50 M E) 0.75 M

C) 1.25 M

What is the molar concentration of sodium ions in a 0.450 M Na3PO4 solution? A) 0.150 M B) 0.450 M C) 1.35 M D) 1.80 M

C) 1.35 M

How many xenon atoms are contained in 2.36 moles of xenon? A) 3.92 × 1024 xenon atoms B) 2.55 × 1023 xenon atoms C) 1.42 × 1024 xenon atoms D) 7.91 × 1025 xenon atoms E) 1.87 × 1026 xenon atoms

C) 1.42 × 1024 xenon atoms

A piece of metal ore weighs 8.25 g. When a student places it into a graduated cylinder containing water, the liquid level rises from 21.25 mL to 26.47 mL. What is the density of the ore? A) 0.312 g/mL B) 0.633 g/mL C) 1.58 g/mL D) 3.21 g/mL

C) 1.58 g/mL

The mass of a proton is 1.67 × 10-27 kg. What is the mass of a proton in picograms? A) 1.67 × 10-18 pg B) 1.67 × 10-15 pg C) 1.67 × 10-12 pg D) 1.67 × 10-9 pg

C) 1.67 × 10-12 pg

How many moles of CuO can be produced from 0.900 mol of Cu2O in the following reaction? 2 Cu2O(s) + O2(g) → 4 CuO(s) A) 0.450 mol B) 0.900 mol C) 1.80 mol D) 3.60 mol

C) 1.80 mol

According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl2. FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq) A) 3.97 × 10-2 moles B) 2.52 × 10-2 moles C) 1.99 × 10-2 moles D) 5.03 × 10-2 moles E) 6.49 × 10-2 moles

C) 1.99 × 10-2 moles

According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H2O? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g) A) 2.72 moles H2O B) 16.7 moles H2O C) 10.9 moles H2O D) 8.33 moles H2O E) 4.87 moles H2O

C) 10.9 moles H2O

Vitamin E is a fat soluble vitamin with the formula C29H50O2 and a molar mass of 431 g/ mole. How many carbon atoms are in 30.0 mg? A) 15.0 × 1020 B) 4.10 × 1020 C) 12.1 × 1020 D) 4.20 × 1022

C) 12.1 × 1020

If the percent yield for the following reaction is 65.0%, how many grams of KClO3 are needed to produce 32.0 g of O2? 2 KClO3(s) → 2 KCl(s) + 3 O2(g) A) 53.1 g B) 81.7 g C) 126 g D) 283 g

C) 126 g

How many milliliters of a 9.0 M H2SO4 solution are needed to make 0.35 L of a 3.5 M solution? A) 0.14 mL B) 0.90 mL C) 140 mL D) 900 mL

C) 140 mL

A mass of mercury occupies 0.950 L. What volume would an equal mass of ethanol occupy? The density of mercury is 13.546 g/mL and the density of ethanol is 0.789 g/mL. A) 0.0553 L B) 0.0613 L C) 16.3 L D) 18.1 L

C) 16.3 L

The estimated costs for remodeling the interior of an apartment are: three 1-gallon cans of paint at $13.22 each, two paint brushes at $9.53 each, and $135 for a helper. The total estimated cost with the appropriate significant figures is $________. A) 193.72 B) 1.9 × 102 C) 194 D) 2 × 102 E) 193.7

C) 194

Write a balanced equation to show the reaction of gaseous ethane with gaseous oxygen to form carbon monoxide gas and water vapor. A) 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g) B) C2H6(g) + 5 O(g) → 2 CO(g) + 3 H2O(g) C) 2 C2H6(g) + 5 O2(g) → 4 CO(g) + 6 H2O(g) D) C2H6(g) + 7 O(g) → 2 CO2(g) + 3 H2O(g) E) 2 CH3(g) + 5 O(g) → 2 CO(g) + 3 H2O(g)

C) 2 C2H6(g) + 5 O2(g) → 4 CO(g) + 6 H2O(g)

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed. A) 2 H+(aq) + CO32-(aq) → H2CO3(s) B) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq) C) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g) D) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq) E) No reaction occurs.

C) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g)

Which of the following is a precipitation reaction? A) Zn(s) + 2 AgNO3(aq) → 2 Ag(s) + Zn(NO3)2(aq) B) NaCl(aq) + LiI(aq) → NaI(aq) + LiCl(aq) C) 2 LiI(aq) + Hg2(NO3)2(aq) → Hg2I2(s) + 2 LiNO3(aq) D) HCl(aq) + KOH(aq) → KCl(aq) + H2O(l) E) None of the above are precipitation reactions.

C) 2 LiI(aq) + Hg2(NO3)2(aq) → Hg2I2(s) + 2 LiNO3(aq)

What is the mass of 8.50 × 1022 molecules of NH3? A) 0.00829 g B) 0.417 g C) 2.40 g D) 121 g

C) 2.40 g

How many chloride ions are present in 65.5 mL of 0.210 M AlCl3 solution? A) 4.02 × 1023 chloride ions B) 5.79 × 1024 chloride ions C) 2.48 × 1022 chloride ions D) 8.28 × 1021 chloride ions E) 1.21 × 1022 chloride ions

C) 2.48 × 1022 chloride ions

Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O A) 0.640 moles B) 64.0 moles C) 2.56 moles D) 16.0 moles

C) 2.56 moles

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H2O(l) → Ca(OH)2(s) A 4.50-g sample of CaO is reacted with 4.34 g of H2O. How many grams of water remain after the reaction is complete? A) 0.00 B) 0.00892 C) 2.90 D) 1.04 E) 0.161

C) 2.90

If the melting point of vanadium metal is 1910°C, what is its melting point in Kelvin? A) 1029 K B) 1637 K C) 2183 K D) 3470 K

C) 2183 K

What mass of phosphorus pentafluoride, PF5, has the same number of fluorine atoms as 25.0 g of oxygen difluoride, OF2? A) 0.933 g B) 10.0 g C) 23.3 g D) 146 g

C) 23.3 g

Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq), is needed to completely react with 24.88 mL of 0.125 M KI3(aq), according to the chemical equation: 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq). A) 6.22 mL B) 12.4 mL C) 24.9 mL D) 99.5 mL

C) 24.9 mL

Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid. What is the coefficient for sulfuric acid when the equation is balanced using the lowest, whole-numbered coefficients? A) 1 B) 2 C) 3 D) none of these

C) 3

Calculate the molar mass of Ca3(PO4)2. A) 87.05 g/mol B) 215.21 g/mol C) 310.18 g/mol D) 279.21 g/mol E) 246.18 g/mol

C) 310.18 g/mol

Which of the following contains the fewest atoms? You shouldn't need to do a calculation here. A) 4.0 g Li B) 4.0 g Na C) 4.0 g Rb D) 4.0 g K E) 4.0 g Ca

C) 4.0 g Rb

Determine the name for H2CO3. A) carbonous acid B) dihydrogen carbonate C) carbonic acid D) hydrocarbonic acid E) hydrocarbide acid

C) carbonic acid

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s) → 2Na(s) + 3N2(g) How many moles of N2 are produced by the decomposition of 2.88 mol of sodium azide? A) 1.92 B) 8.64 C) 4.32 D) 0.960 E) 1.44

C) 4.32

The molecular weight of nitrous oxide (N2O), known as laughing gas, is ________ amu (rounded to one decimal place). A) 60.0 B) 30.0 C) 44.0 D) 3.0 E) 22.0

C) 44.0

How many grams of oxygen are formed when 6.21 moles of KOH are formed? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g) A) 19.9 g O2 B) 27.9 g O2 C) 49.7 g O2 D) 3.59 g O2 E) 11.7 g O2

C) 49.7 g O2

How many grams of AgNO3 are needed to make 250. mL of a solution that is 0.135 M? A) 0.0917 g B) 0.174 g C) 5.73 g D) 91.7 g

C) 5.73 g

How many milliliters of 0.550 M hydriodic acid are needed to react with 15.00 mL of 0.217 M CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H2O(l) A) 0.0263 mL B) 0.169 mL C) 5.92 mL D) 38.0 mL

C) 5.92 mL

How many grams of H2 gas can be produced by the reaction of 54.0 grams of Al(s) with an excess of dilute hydrochloric acid in the reaction shown below? 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g) A) 2.68 g B) 4.04 g C) 6.05 g D) 12.1 g

C) 6.05 g

How many milliliters of a 0.184 M NaNO3 solution contain 0.113 moles of NaNO3? A) 543 mL B) 163 mL C) 614 mL D) 885 mL E) 326 mL

C) 614 mL

An atom of 118Xe contains ________ neutrons. A) 54 B) 172 C) 64 D) 110 E) 118

C) 64

What is the mass of 9.44 × 1024 molecules of NO2? The molar mass of NO2 is 46.01 g/mol. A) 205 g B) 294 g C) 721 g D) 341 g E) 685 g

C) 721 g

Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kg of iodine were produced? A) 13.3 kg B) 22.5 kg C) 79.4 kg D) 44.4 kg E) 92.4 kg

C) 79.4 kg

How many Li atoms are contained in 97.9 g of Li? A) 5.90 × 1025 Li atoms B) 7.09 × 1021 Li atoms C) 8.49 × 1024 Li atoms D) 4.27 × 1022 Li atoms E) 4.18 × 1024 Li atoms

C) 8.49 × 1024 Li atoms

How many liters of wine can be held in a wine barrel whose capacity is 26.0 gal? 1 gal = 4 qt = 3.7854 L. A) 1.46 × 10-4 B) 0.146 C) 98.4 D) 6.87 × 103 E) 6.87

C) 98.4

Which statement is true? A) All chemical bonds share electrons between atoms. B) A covalent bond involves transfer of electrons from a metal atom to a nonmetal atom. C) An ionic bond involves transfer of electrons from a metal atom to a nonmetal atom. D) An ionic bond is formed by sharing a pair of electrons.

C) An ionic bond involves transfer of electrons from a metal atom to a nonmetal atom.

What element is defined by the following information? p+ = 17 n° = 20 e- = 17 A) calcium B) rubidium C) chlorine D) neon E) oxygen

C) chlorine

What element is undergoing oxidation (if any) in the following reaction? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) A) O B) H C) C D) both C and H E) None of the elements is undergoing oxidation.

C) C

Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO2 and 59.38 mg of H2O. What is the empirical formula for the compound? A) C5H2O B) CHO C) C3H6O D) C3H7O E) C6HO3

C) C3H6O

Which one of the following contains 39% carbon by mass? A) C2H2 B) CH4 C) CH3NH2 D) CO2

C) CH3NH2

The chemical formula for calcium nitride is A) Ca(NO3)2. B) Ca(NO2)2. C) Ca3N2. D) CaN2.

C) Ca3N2.

What is the chemical symbol for copper? A) Co B) Cr C) Cu D) C

C) Cu

Which one of the following compounds behaves as an acid when dissolved in water? A) RaO B) C4H10 C) HI D) RbOH

C) HI

What is the chemical symbol for mercury? A) Ag B) Au C) Hg D) Pb

C) Hg

Write the formula for the compound formed between potassium and sulfur. A) KS B) KS2 C) K2S D) K2SO3 E) K3S2

C) K2S

The mixing of which pair of reactants will result in a precipitation reaction? A) CsI(aq) + NaOH(aq) B) HCl(aq) + Ca(OH)2(aq) C) K2SO4(aq) + Hg2(NO3)2(aq) D) NaNO3(aq) + NH4Cl(aq)

C) K2SO4(aq) + Hg2(NO3)2(aq)

Which of the following elements has the least tendency to form an ion? A) Ca B) K C) Kr D) Se

C) Kr

18) Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N2O4 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol. N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) A) LR = N2H4, 59.0 g N2 formed B) LR = N2O4, 105 g N2 formed C) LR = N2O4, 45.7 g N2 formed D) LR = N2H4, 13.3 g N2 formed E) No LR, 45.0 g N2 formed

C) LR = N2O4, 45.7 g N2 formed

Which of the following elements is an alkaline earth metal? A) Cs B) Cu C) Mg D) Ti E) Br

C) Mg

Which of the following is not a strong electrolyte? A) LiOH B) CaCl2 C) MgCO3 D) NaC2H3O2 E) Li2SO4

C) MgCO3

Determine the molecular formula of a compound that has a molar mass of 92.0 g/mol and an empirical formula of NO2. A) N2O3 B) N3O6 C) N2O4 D) NO2 E) N2O5

C) N2O4

What are the spectator ions for the following reaction in aqueous solution: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) A) Ag+ B) Cl- C) Na+ & NO3- D) Na+ & Cl-

C) Na+ & NO3-

Give the formula for sodium chlorate. A) NaClO B) NaClO2 C) NaClO3 D) NaClO4

C) NaClO3

Which pair of compounds is soluble in water? A) Ag Cl and AgBr B) CoS and K2S C) NaI and Cu(NO3)2 D) NH4NO3 and BaCO3

C) NaI and Cu(NO3)2

Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 g of sodium hydroxide according to the following chemical equation: 2 S(s) + 3 O2(g) + 4 NaOH(aq) → 2 Na2SO4(aq) + 2 H2O(l) A) S(s) B) O2(g) C) NaOH(aq) D) None of these substances is the limiting reactant.

C) NaOH(aq)

Which one of the following compounds is insoluble in water? A) Ca Cl2 B) NaNO3 C) Pb Cl2 D) K2CO3

C) Pb Cl2

Which one of the following compounds is soluble in water? A) Cu3(PO4)2 B) CoS C) Pb(NO3)2 D) ZnCO3

C) Pb(NO3)2

Which of the following is a molecular element? A) Kr B) Ag C) S D) Mg E) Ti

C) S

The chemical formula for the sulfite ion is A) S-. B) S 2-. C) SO32-. D) SO42-.

C) SO32-.

Which of the following pairs of aqueous solutions will react to produce a precipitate? A) LiOH + Na2S B) (NH4)2SO4 + LiCl C) Sr(C2H3O2)2 + Na2SO4 D) KNO3 + NaOH E) None of the above solution pairs will produce a precipitate.

C) Sr(C2H3O2)2 + Na2SO4

Which of the following does not describe a metal? A) Good conductor of heat B) Good conductor of electricity C) Tends to gain electrons D) Forms ionic compounds with nonmetals E) Found on the left side of the periodic table

C) Tends to gain electrons

Which of the following elements is not a metal? A) Ba B) Mg C) Xe D) Pb E) G

C) Xe

Which of the following elements is not a solid at room temperature? A) Ag B) Al C) Xe D) Fe

C) Xe

When dissolved in water, KOH behaves as A) an acid that forms K+ and OH- ions. B) an acid that forms KO- and H+ ions. C) a base that forms K+ and OH- ions. D) a base that forms KO- and H+ ions.

C) a base that forms K+ and OH- ions.

Write the name for Ca3(PO4)2. A) calcium (III) phosphite B) calcium (II) phosphite C) calcium phosphate D) tricalcium phosphorustetraoxide E) calcium phosphite

C) calcium phosphate

Write the name for Sr3(PO4)2. A) strontium (III) phosphite B) strontium (II) phosphite C) strontium phosphate D) tristrontium phosphorustetraoxide E) strontium phosphite

C) strontium phosphate

Which element has the chemical symbol, S? A) selenium B) silicon C) sulfur D) scandium

C) sulfur

Identify the crystalline solid. A) plastic B) glass C) table salt D) water E) bleach

C) table salt

A certain alcohol contains only three elements, carbon, hydrogen, and oxygen. Combustion of a 50.00 gram sample of the alcohol produced 95.50 grams of CO2 and 58.70 grams of H2O. What is the empirical formula of the alcohol?

C2H6O

Which of the following has the smallest mass? A) 3.50 × 1023 molecules of I2 B) 85.0 g of Cl2 C) 2.50 mol of F2 D) 0.050 kg of Br2

D) 0.050 kg of Br2

A student dissolved 4.00 g of Co(NO3)2 in enough water to make 100. mL of stock solution. He took 4.00 mL of the stock solution and then diluted it with water to give 275. mL of a final solution. How many grams of NO3- ion are there in the final solution? A) 0.0197 g B) 0.0394 g C) 0.0542 g D) 0.108 g

D) 0.108 g

Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 × 1023 atoms of Fe according to the following reaction. 2 HCl(aq) + Fe(s) → H2(g) + FeCl2(aq) A) 0.374 g B) 1.33 g C) 1.14 g D) 0.187 g E) 1.51 g

D) 0.187 g

Calculate the moles of Fe in 16.0 g of Fe2O3. A) 10.0 mol B) 0.10 mol C) 16.0 mol D) 0.200 mol

D) 0.200 mol

What is the concentration of nitrate ions in a 0.125 M Mg(NO3)2 solution? A) 0.125 M B) 0.0625 M C) 0.375 M D) 0.250 M E) 0.160 M

D) 0.250 M

What mass, in kg, does 5.84 moles of titanium (Ti) have? A) 0.352 kg B) 0.122 kg C) 0.820 kg D) 0.280 kg E) 0.632 kg

D) 0.280 kg

Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 10.00 mL of glacial acetic acid at 25°C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25°C is 1.05 g/mL. A) 1.26 × 103 M B) 21.0 M C) 0.0210 M D) 0.350 M E) 3.50 × 10-4 M

D) 0.350 M

How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g) A) 23.2 mol O2 B) 0.580 mol O2 C) 18.5 mol O2 D) 0.724 mol O2 E) 1.73 mol O2

D) 0.724 mol O2

What decimal power does the abbreviation pico represent? A) 1 × 106 B) 1 × 109 C) 1 × 10-1 D) 1 × 10-12 E) 1 × 10-15

D) 1 × 10-12

What decimal power does the abbreviation f represent? A) 1 × 106 B) 1 × 103 C) 1 × 10-1 D) 1 × 10-15 E) 1 × 10-12

D) 1 × 10-15

Predict the charge of the most stable ion of bromine. A) 2+ B) 1+ C) 3+ D) 1- E) 2-

D) 1-

What is the concentration of NO3- ions in a solution prepared by dissolving 25.0 g of Ca(NO3)2 in enough water to produce 300. mL of solution? A) 0.254 M B) 0.508 M C) 0.672 M D) 1.02 M

D) 1.02 M

How many atoms of oxygen are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3 is 233.99 g/mol. A) 1.23 × 1023 O atoms B) 2.96 × 1024 O atoms C) 2.87 × 1025 O atoms D) 1.10 × 1024 O atoms E) 3.19 × 1024 O atoms

D) 1.10 × 1024 O atoms

How many oxygen atoms are there in 7.00 g of sodium dichromate, Na2Cr2O7? A) 0.187 oxygen atoms B) 2.30 × 1021 oxygen atoms C) 1.60 × 1022 oxygen atoms D) 1.13 × 1023 oxygen atoms

D) 1.13 × 1023 oxygen atoms

Which has the least number of atoms? A) 1mol O2 B) 1mol H2O C) 4.0 g He D) 1.2 g C

D) 1.2 g C

How many molecules are contained in 25.0 mL of butane? The density of butane is 0.6011 g/mL and the molar mass is 58.12 g/mol. A) 2.59 × 1023 molecules butane B) 1.46 × 1027 molecules butane C) 6.87 × 1023 molecules butane D) 1.56 × 1023 molecules butane E) 7.14 × 1025 molecules butane

D) 1.56 × 1023 molecules butane

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) A) 38.0 g H2O B) 21.7 g H2O C) 43.4 g H2O D) 10.9 g H2O E) 26.5 g H2O

D) 10.9 g H2O

How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 1.38 g of Fe2S3 if the percent yield for the reaction is 65.0%? 3 Na2S(aq) + 2 FeCl3(aq) → Fe2S3(s) + 6 NaCl(aq) A) 25.5 mL B) 43.1 mL C) 51.1 mL D) 102 mL

D) 102 mL

The mass number of an atom of 128Xe is ________. A) 54 B) 182 C) 74 D) 128 E) 120

D) 128

Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of MgSO3 and HI are mixed. A) 2 H+(aq) + SO32-(aq) → H2SO3(s) B) Mg2+(aq) + 2 I-(aq) → MgI2(s) C) 2 H+(aq) + SO32-(aq) + Mg2+(aq) + 2 I-(aq) → H2SO3(s) + MgI2(aq) D) 2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g) E) No reaction occurs.

D) 2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g)

Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide and copper (II) nitrate are mixed. A) Li+(aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq) B) Li+(aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq) C) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s) D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq) E) No reaction occurs.

D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq)

Predict the charge that a calcium ion would have. A) 6- B) 2- C) 3+ D) 2+ E) 1+

D) 2+

Round the following number to four significant figures and express the result in standard exponential notation: 229.613 A) 0.2296 × 103 B) 229.6 C) 2.296 × 10-2 D) 2.296 × 102 E) 22.96 × 10-1

D) 2.296 × 102

How many liters of a 0.0550 M KCl solution contain 0.163 moles of KCl? A) 3.37 L B) 1.48 L C) 8.97 L D) 2.96 L E) 1.12 L

D) 2.96 L

A sample of pure calcium fluoride with a mass of 15.0 g contains 7.70 g of calcium. How much calcium is contained in 40.0 g of calcium fluoride? A) 2.27 g B) 7.70 g C) 15.0 g D) 20.5 g

D) 20.5 g

How many of the following compounds are soluble in water? Cu(OH)2 LiNO3 NH4Br K2S A) 0 B) 1 C) 2 D) 3 E) 4

D) 3

What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients? _____ C2H6O(l) + _____ O2(g) → _____ CO2(g) + _____ H2O(l) A) 9 B) 7 C) 5 D) 3

D) 3

A student weighed 30.00 μg of sulfur in the lab. This is the same mass as A) 3.000 × 10-8 g. B) 3.000 × 10-5 kg. C) 3.000 × 10-5 mg. D) 3.000 × 104 ng.

D) 3.000 × 104 ng.

Convert 35 m3 to liters. A) 3.5 × 10-2 L B) 3.5 L C) 3.5 × 102 L D) 3.5 × 104 L

D) 3.5 × 104 L

How many iron atoms are contained in 354 g of iron? A) 2.62 × 1025 Fe atoms B) 2.13 × 1026 Fe atoms C) 4.69 × 1024 Fe atoms D) 3.82 × 1024 Fe atoms E) 9.50 × 1022 Fe atoms

D) 3.82 × 1024 Fe atoms

The recommended adult dose of Elixophyllin, a drug used to treat asthma, is 6.00 mg/kg of body mass. Calculate the dose in milligrams for a 115-lb person. 1 lb = 453.59 g. A) 24 B) 1,521 C) 1.5 D) 313 E) 3.1 × 105

D) 313

Based on the balanced chemical equation shown below, determine the mass percent of Fe3+ in a 0.7450 g sample of iron ore, if 22.40 mL of a 0.1000 M stannous chloride, SnCl2(aq), solution is required to completely react with the Fe3+ present in the ore sample. The chemical equation for the reaction is 2 Fe3+(aq) + Sn2+(aq) → 2 Fe2+(aq) + Sn4+(aq). A) 5.365% B) 8.396% C) 16.79% D) 33.58%

D) 33.58%

How many grams of NaCl are required to make 250.0 mL of a 3.000 M solution? A) 58.40 g B) 175.3 g C) 14.60 g D) 43.83 g

D) 43.83 g

What mass of N2 will be produced from the reaction of 50.0 g N2O4 with 45.0 g N2H4? N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) A) 59.0 g B) 118 g C) 152 g D) 45.7 g

D) 45.7 g

Calculate the number of grams of solute in 500.0 mL of 0.189 M KOH. A) 148 B) 1.68 C) 5.30 × 103 D) 5.30 E) 1.68 × 10-3

D) 5.30

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) In a particular experiment, 3.50 g samples of each reagent are reacted. The theoretical yield of lithium nitride is ________ g. A) 3.52 B) 2.93 C) 17.6 D) 5.85 E) 8.7

D) 5.85

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s) → 2Na(s) + 3N2(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen? A) 1.77 B) 0.785 C) 76.6 D) 51.1 E) 114.9

D) 51.1

Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction. A possibly useful molar mass is BCl3 = 117.16 g/mol. BCl3(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g) A) 75.9 g HCl B) 132 g HCl C) 187 g HCl D) 56.0 g HCl E) 25.3 g HCl

D) 56.0 g HCl

What volume (in mL) of 0.0887 M MgF2 solution is needed to make 275.0 mL of 0.0224 M MgF2 solution? A) 72.3 mL B) 91.8 mL C) 10.9 mL D) 69.4 mL E) 14.4 mL

D) 69.4 mL

Balance the chemical equation given below, and determine the number of grams of MgO are needed to produce 10.0 g of Fe2O3 . ____ MgO(s) + ____ Fe(s) → ____ Fe2O3(s) +_____ Mg(s) A) 0.312 g B) 0.841 g C) 2.52 g D) 7.57 g

D) 7.57 g

How many millimoles of Ca(NO3)2 contain 4.78 × 1022 formula units of Ca(NO3)2? The molar mass of Ca(NO3)2 is 164.10 g/mol. A) 12.6 mmol Ca(NO3)2 B) 13.0 mmol Ca(NO3)2 C) 20.7 mmol Ca(NO3)2 D) 79.4 mmol Ca(NO3)2 E) 57.0 mmol Ca(NO3)2

D) 79.4 mmol Ca(NO3)2

Give the number of electrons for carbon-14, with a -2 charge. A) 7 B) 4 C) 6 D) 8

D) 8

How many chloride ions are there in 4.50 mol of aluminum chloride? A) 3.00 chloride ions B) 13.5 chloride ions C) 2.71 × 1024 chloride ions D) 8.13 × 1024 chloride ions

D) 8.13 × 1024 chloride ions

How many aluminum ions are present in 65.5 mL of 0.210 M AlF3 solution? A) 4.02 × 1023 aluminum ions B) 5.79 × 1024 aluminum ions C) 2.48 × 1022 aluminum ions D) 8.28 × 1021 aluminum ions E) 1.21 × 1022 aluminum ions

D) 8.28 × 1021 aluminum ions

According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution? 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) A) 97.4 mL B) 116 mL C) 43.0 mL D) 86.1 mL E) 58.1 mL

D) 86.1 mL

Round off 00907506 to four significant figures. A) 0091 B) 9076 C) 9100 D) 9.075 × 105

D) 9.075 × 105

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H2O(l) → Ca(OH)2(s) In a particular experiment, a 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH)2 is recovered. What is the percent yield in this experiment? A) 122 B) 1.22 C) 7.19 D) 92.5 E) 81.9

D) 92.5

What element is undergoing reduction (if any) in the following reaction? Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s) A) Zn B) N C) O D) Ag E) This is not an oxidation-reduction reaction.

D) Ag

Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate. A) Al(C2H3O2)2(aq) + (NH4)2PO4(aq) → AlPO4(s) + 2 NH4C2H3O2(aq) B) Al(C2H3O2)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3C2H3O2(aq) C) Al(CO3)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3CO3(aq) D) Al(C2H3O2)3(aq) + (NH4)3PO4(aq) → AlPO4(s) + 3 NH4C2H3O2(aq) E) Al(CO2)3(aq) + (NH4)3PO3(aq) → AlPO3(s) + 3 NH4CO2(aq)

D) Al(C2H3O2)3(aq) + (NH4)3PO4(aq) → AlPO4(s) + 3 NH4C2H3O2(aq)

Give the correct formula for aluminum sulfate. A) Al22SO4 B) Al(SO4)3 C) Al3(SO4)2 D) Al2(SO4)3

D) Al2(SO4)3

Which of the following is the correct chemical formula for a molecule of astatine? A) At B) At- C) At+ D) At2

D) At2

Write the formula for barium nitrite. A) Ba3N2 B) BaNO3 C) BN D) Ba(NO2)2 E) B(NO2)3

D) Ba(NO2)2

In which of the following sets do all species have the same number of protons? A) F-, Ne, Mg2+ B) Ge, Se2-, Br- C) K+, Rb+, Cs+ D) Br, Br-, Br+

D) Br, Br-, Br+

Which one of the following is not an empirical formula? A) CHO B) CH2O C) C2H4O D) C2H4O2

D) C2H4O2

Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen, and oxygen produced 2.086 g of CO2 and 1.134 g of H2O. What is the empirical formula of the compound? A) C2H5O B) C2H5O2 C) C2H10O3 D) C3H8O2

D) C3H8O2

Which of the following compounds is an Arrhenius base? A) C6H12O6 B) HOCl C) H2SO4 D) C6H5NH2

D) C6H5NH2

Which of the following is not a strong electrolyte? A) CaS B) LiSO4 C) NH4OH D) CH3CH2CH3 E) Na2CO3

D) CH3CH2CH3

Which of the following is a molecular compound? A) CuCl2 B) KCl C) NaNO3 D) CH3Cl E) RbBr

D) CH3Cl

What is the chemical formula for calcium hydroxide? A) CaH2 B) CaOH C) CaOH2 D) Ca(OH)2

D) Ca(OH)2

Which of the following compounds is an Arrhenius base? A) CH3OH B) CH3CO2H C) HOCl D) CsOH

D) CsOH

What is the chemical formula for iron(III) sulfate? A) Fe3S B) Fe3SO4 C) Fe2S3 D) Fe2(SO4)3

D) Fe2(SO4)3

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and Fe(NO3)2 are mixed. A) K+(aq) + NO3-(aq) → KNO3(s) B) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq) C) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s) D) Fe2+(aq) + S2-(aq) → FeS(s) E) No reaction occurs.

D) Fe2+(aq) + S2-(aq) → FeS(s)

Which of the following is a molecular element? A) Mg B) Ar C) Xe D) I E) Li

D) I

Which of the following elements is an alkali metal? A) Zn B) Xe C) F D) Li E) Ca

D) Li

Which statement is correct for the following redox reaction? 5 Fe2+ + MnO4- +8H+ → 5 Fe3+ +Mn2+ + 4H2O A) Fe2+ is reduced. B) MnO4- is oxidized. C) Fe2+ is the oxidizing agent. D) MnO4- is the oxidizing agent.

D) MnO4- is the oxidizing agent.

In which set do all elements tend to form anions in binary ionic compounds? A) C, S, Pb B) K, Fe, Br C) Li, Na, K D) N, O, I

D) N, O, I

Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass. A) NO B) N2O C) NO2 D) N2O3 E) NO3

D) N2O3

Which of the following is a gas-evolution reaction? A) 2 C2H6(l) + 7 O2(g) → 4 CO2(g) + 6 H2O(g) B) 2 H2(g) + O2(g) → 2 H2O(g) C) LiCl(aq) + NaNO3(aq) → LiNO3(aq) + NaCl(g) D) NH4Cl(aq) + KOH(aq) → KCl(aq) + NH3(g) + H2O(l) E) None of the above are gas-evolution reactions.

D) NH4Cl(aq) + KOH(aq) → KCl(aq) + NH3(g) + H2O(l)

Which of the following does not describe a nonmetal? A) Tend to gain electrons B) Found in the upper right hand corner of the periodic table. C) Poor conductor of electricity D) Nonmetals are generally unreactive. E) Poor conductor of heat

D) Nonmetals are generally unreactive.

Identify the chemical symbol of element Q in 80/34Q. A) Br B) Hg C) Pd D) Se

D) Se

Which of the following elements is a metal? A) As B) C C) I D) Sn E) Se

D) Sn

Which of the following statements is false? A) Anions are usually larger than their corresponding atom. B) Metals tend to form cations. C) Atoms are usually larger than their corresponding cation. D) The halogens tend to form 1+ ions. E) Nonmetals tend to gain electrons.

D) The halogens tend to form 1+ ions.

7.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below. Which one of the following statements is FALSE? N2(g) + 3 H2(g) → 2 NH3(g) A) 3.5 g of hydrogen are left over. B) Hydrogen is the excess reactant. C) Nitrogen is the limiting reactant. D) The theoretical yield of ammonia is 15 g.

D) The theoretical yield of ammonia is 15 g.

5.0 g of iron is reacted with 5.0 g of water according to the chemical equation shown below. Which one of the following statements is FALSE? 3 Fe(s) + 4 H2O(l) → Fe3O4(s) + 4 H2(g) A) 6.91 g of Fe3O4 are produced. B) 2.85 g of H2O are left over. C) Mass is conserved in this reaction. D) Water is the limiting reactant.

D) Water is the limiting reactant.

Which of the following elements is a good conductor of heat and electricity? A) carbon B) chlorine C) neon D) aluminum

D) aluminum

What does "X" represent in the following symbol? X A) mercury B) chlorine C) scandium D) bromine E) selenium

D) bromine

Determine the name for HClO3. A) hydrochloric acid B) hydrochlorus acid C) chlorate acid D) chloric acid E) perchloric acid

D) chloric acid

Determine the name for CoCl2∙6H2O. Remember that Co forms several ions. A) cobalt chloride hydrate B) cobalt (I) chloride heptahydrate C) cobalt (II) chloride heptahydrate D) cobalt (II) chloride hexahydrate E) cobalt (I) chloride

D) cobalt (II) chloride hexahydrate

The compound, Cu(N O2)2, is named A) copper nitrite(II). B) copper(I) nitrite. C) copper(I) nitrite(II). D) copper(II) nitrite.

D) copper(II) nitrite.

Determine the oxidation state of Cl in NaClO3. A) +6 B) +4 C) +3 D) +2 E) +5

E) +5

Lithium and nitrogen react to produce lithium nitride by the following reaction. 6Li(s) + N2(g) → 2Li3N(s) How many moles of N2 are needed to react with 0.500 mol of lithium? A) 3.00 B) 0.500 C) 0.167 D) 1.50 E) 0.0833

E) 0.0833

A solution is prepared by mixing 50.0 mL of 0.100 M HCl and 10.0 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution? A) 0.183 B) 8.57 C) 3.50 D) 0.0500 E) 0.117

E) 0.117

Consider the following balanced reaction. What mass (in g) of CO2 can be formed from 288 mg of O2? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g) A) 0.396 g CO2 B) 0.209 g CO2 C) 0.792 g CO2 D) 0.126 g CO2 E) 0.198 g CO2

E) 0.198 g CO2

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O2(g) → 2MgO(s) How many moles of O2 are consumed when 0.770 mol of magnesium burns in excess oxygen? A) 0.0317 B) 2.60 C) 0.770 D) 1.54 E) 0.385

E) 0.385

Predict the charge of the most stable ion of potassium. A) 3+ B) 1- C) 2+ D) 2- E) 1+

E) 1+

What mass, in mg, does 2.63 moles of nickel have? A) 44.8 mg B) 2.23 × 104 mg C) 129 mg D) 3.56 × 105 mg E) 1.54 × 105 mg

E) 1.54 × 105 mg

Determine the volume of hexane that contains 5.33 × 1022 molecules of hexane. The density of hexane is 0.6548 g/mL and its molar mass is 86.17 g/mol. A) 8.59 mL B) 13.5 mL C) 7.40 mL D) 12.4 mL E) 11.6 mL

E) 11.6 mL

Give the number of neutrons in Al3+. A) 10 B) 16 C) 17 D) 13 E) 14

E) 14

How many moles of C3H8 contain 9.25 × 1024 molecules of C3H8? A) 65.1 moles C3H8 B) 28.6 moles C3H8 C) 34.9 moles C3H8 D) 46.2 moles C3H8 E) 15.4 moles C3H8

E) 15.4 moles C3H8

According to the following reaction, what amount of Al2S3 remains when 20.00 g of Al2S3 and 2.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 = 150.17 g/mol, H2O = 18.02 g/mol. Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g) A) 28.33 g B) 14.00 g C) 8.33 g D) 19.78 g E) 17.22 g

E) 17.22 g

Predict the charge that an ion formed from sulfur would have. A) 1- B) 6+ C) 3- D) 4+ E) 2-

E) 2-

Determine the theoretical yield of H2S (in moles) if 4.0 mol Al2S3 and 4.0 mol H2O are reacted according to the following balanced reaction. A possibly useful molar mass is Al2S3 = 150.17 g/mol. Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g) A) 12 mol H2S B) 4.0 mol H2S C) 18 mol H2S D) 6.0 mol H2S E) 2.0 mol H2S

E) 2.0 mol H2S

What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution? Hint: you will want to write a balanced reaction. A) 581 mL B) 173 mL C) 345 mL D) 139 mL E) 278 mL

E) 278 mL

How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M NaOH? A) 0.521 B) 0.0120 C) 83.7 D) 0.0335 E) 29.9

E) 29.9

Predict the charge that an aluminum ion would have. A) 5- B) 1+ C) 1- D) 2+ E) 3+

E) 3+

How many protons does the Br- ion possess? A) 34 B) 36 C) 6 D) 8 E) 35

E) 35

How many N2O4 molecules are contained in 76.3 g N2O4? The molar mass of N2O4 is 92.02 g/mol. A) 5.54 × 1025 N2O4 molecules B) 7.26 × 1023 N2O4 molecules C) 1.38 × 1024 N2O4 molecules D) 4.59 × 1025 N2O4 molecules E) 4.99 × 1023 N2O4 molecules

E) 4.99 × 1023 N2O4 molecules

The density of air under ordinary conditions at 25°C is 1.19 g/L. How many kilograms of air are in a room that measures 11.0 ft × 11.0 ft and has a(n) 10.0 ft ceiling? 1 in. = 2.54 cm (exactly); 1 L = 103 cm3. A) 3.66 B) 0.152 C) 4.08 × 104 D) 0.0962 E) 40.8

E) 40.8

Calculate the mass, in g, of 1.9 × 1024 atoms of Pb. A) 3.9 × 102 g B) 2.4 × 102 g C) 3.2 × 102 g D) 1.5 × 102 g E) 6.5 × 102 g

E) 6.5 × 102 g

How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution? A) 1.31 × 10-3 mol B) 8.74 × 10-3 mol C) 1.14 × 10-3 mol D) 3.67 × 10-3 mol E) 7.65 × 10-3 mol

E) 7.65 × 10-3 mol

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react with excess Al according to the following reaction. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) A) 61.03% B) 28.65% C) 57.30% D) 20.02% E) 81.93%

E) 81.93%

How many sodium ions are contained in 99.6 mg of Na2SO3? The molar mass of Na2SO3 is 126.05 g/mol. A) 1.52 × 1027 sodium ions B) 4.76 × 1020 sodium ions C) 2.10 × 1021 sodium ions D) 1.05 × 1021 sodium ions E) 9.52 × 1020 sodium ions

E) 9.52 × 1020 sodium ions

Which of the following pairs of aqueous solutions will produce a precipitate when mixed? A) HCl + LiOH B) Li2S + HCl C) K2CO3 + HNO3 D) MgCl2 + KOH E) All of these solution pairs will produce a precipitate.

E) All of these solution pairs will produce a precipitate.

Which of the following statements is false according to Dalton's Atomic Theory? A) Atoms combine in simple whole number ratios to form compounds. B) All atoms of chlorine have identical properties that distinguish them from other elements. C) One carbon atom will combine with one oxygen atom to form a molecule of carbon monoxide. D) Atoms of sodium do not change into another element during chemical reaction with chlorine. E) An atom of nitrogen can be broken down into smaller particles that will still have the unique properties of nitrogen.

E) An atom of nitrogen can be broken down into smaller particles that will still have the unique properties of nitrogen.

What is the empirical formula of a compound that is 62.0% C, 10.4% H, and 27.5% O by mass? A) C3HO B) C6HO3 C) C6H12O2 D) C5H10O2 E) C3H6O

E) C3H6O

Write the formula for copper (II) sulfate pentahydrate. A) Cu2SO3∙H5 B) Cu2S∙H2O C) CuS∙5H2O D) (CuSO4)5 E) CuSO4∙5H2O

E) CuSO4∙5H2O

Determine the reducing agent in the following reaction. 2 Li(s) + Fe(C2H3O2)2(aq) → 2 LiC2H3O2(aq) + Fe(s) A) O B) H C) C D) Fe E) Li

E) Li

Which of the following is an atomic element? A) Br B) H C) N D) O E) Mg

E) Mg

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Al(C2H3O2)3 and LiNO3 are mixed. A) Al3+(aq) + 3 NO3-(aq) → Al(NO3)3(s) B) Li+(aq) + C2H3O2-(aq) → LiC2H3O2(s) C) Al3+(aq) + 3 NO3-(aq) + Li+(aq) + C2H3O2-(aq) → Al(NO3)3(aq) + LiC2H3O2(s) D) 3 Li+(aq) + (C2H3O2)33-(aq) → Li3(C2H3O2)3(s) E) No reaction occurs.

E) No reaction occurs.

Which of the following is a molecular compound? A) NaCN B) LiOH C) SrI2 D) ZnS E) P4O10

E) P4O10

Determine the empirical formula for a compound that is found to contain 10.15 mg P and 34.85 mg Cl. A) P3Cl B) PCl C) PCl2 D) P2Cl3 E) PCl3

E) PCl3

Which of the following statements about isotopes is true? A) Isotopes of the same element differ only in the number of electrons they contain. B) An isotope of an atom with a larger number of neutrons is larger than an isotope of the same atom that contains fewer neutrons. C) Isotopes of the same element have the same mass. D) Isotopes of the same element don't usually have the same properties. E) Some elements have 3 or more naturally occurring isotopes.

E) Some elements have 3 or more naturally occurring isotopes.

Determine the name for aqueous HBr. A) bromic acid B) bromous acid C) hydrobromous acid D) hydrogen bromate E) hydrobromic acid

E) hydrobromic acid

Determine the name for P4O10. A) phosphorus (IV) oxide B) diphosphorus pentoxide C) phosphorus oxide D) phosphorus (II) oxide E) tetraphosphorus decoxide

E) tetraphosphorus decoxide

What does "X" represent in the following symbol? 235/92X A) tin B) copper C) palladium D) niobium E) uranium

E) uranium

Define the law of the conservation of energy

Energy is neither created nor destroyed.

define precision

How close a series of measurements are to one another.

Describe the difference between ions and isotopes.

Ions have the loss or gain of electrons; isotopes differ in the number of neutrons.

Why do the isotopes of the same element have the same atomic size?

Isotopes only differ in the number of neutrons contained within the nucleus. Since the size of an atom is determined by the electrons, isotopes of the same element should be the same size.

List the spectator ions in the following reaction. Ba+2(aq) + 2 OH-(aq) + 2 Na +(aq) + CO3-2(aq) → 2 Na +(aq) + 2 OH-(aq) + BaCO3(s)

Na+ and OH-

Can you predict the chemical formula for a covalent compound between nitrogen and oxygen? Explain your answer.

No, since nitrogen and oxygen are both nonmetals, they combine by sharing electrons. This can be done in multiple different ways. Some possible compounds are N2O, N2O3, NO2.

A sample of liquid isopropyl alcohol is placed in a sealed container. Some of the volatile isopropyl alcohol vaporizes. Does the mass of the sealed container and its contents change during the vaporization? Explain.

No. The vaporized isopropyl alcohol is just in a different physical state. It still has mass and therefore the gas plus the remaining liquid and container have the same total mass after the vaporization of some of the isopropyl alcohol.

Why do elements in the same group tend to have similar chemical properties?

Since elements in the same group have the same number of valence electrons (similar electron configurations) they tend to have similar chemical reactivity, since chemical reactions typically involve valence electrons.

What happens to the density of a sample of iron metal as it is heated from room temperature to 100°C? (This is below the melting point of iron.)

Since the mass of the iron stays constant, but the volume increases as the temperature is raised, the density of the iron decreases upon heating.

Define atomic mass.

The atomic mass represents the average mass of the isotopes that compose that element weighted according to the natural abundance of each isotope.

Why doesn't a mass spectrum of silver have a peak at 107.9 amu?

The average atomic mass of silver is 107.9 amu, but there are no atoms of silver that weigh 107.9 amu. One isotope weighs more and another weighs less.

Why aren't prefixes used in naming ionic compounds?

The charges on the ions dictate how many must be present to form a neutral unit. Molecular compounds do not have such constraints and therefore must use prefixes to denote the number of atoms present.

What group of elements in the periodic table are the most unreactive and why?

The noble gases are the most unreactive since they do not combine with other elements to form compounds.

What is the oxidation number of the sulfur atom in Li2SO4? A) -2 B) +2 C) +4 D) +6

What is the oxidation number of the sulfur atom in Li2SO4? A) -2 B) +2 C) +4 D) +6

is a solution has a temperature of 355 K, what is the temperature in degrees C? a. 165 b. 628 c. 179 d. 79 e. 82

e. 82

how many kL does a 1.25 x 10^8 cL sample contain? a. 1.25 x 10^3 kL b. 1.25 x 10^13 kL c. 1.25 x 10^4 kL d. 1.25 x 10^12 kL e. 1.25 x 10^2 kL

a. 1.25 x 10^3 kL

how many significant figures are in the measurement 0.0005890? a. 4 b. 5 c. 6 d. 7 e. 8

a. 4

NaN is an example of A) a compound. B) an element. C) a heterogeneous mixture. D) a homogeneous mixture.

a. a compound

which of the following statements about crystalline and amorphous solids is true? a. a crystalline solid is composed of atoms or molecules arranged with long-range repeating order b. an example of crystalline solid is glass c. an example of an amorphous solid is table salt (NaCl) d. an amorphous solid has the well-ordered geometric arrangements of atoms

a. a crystalline solid is composed of atoms or molecules arranged with long-range repeating order

which of the following are examples of intensive properties a. density b. volume c. mass d. none of the above e. all of the above

a. density

which of the following is an example of physical change? a. dew forms on a blade of grass b. a halloween light stick glows after shaking c. an egg solidifies during cooking d. a hydrogen balloon explodes when contacted with a flame e. an iron pipe rusts in the yard

a. dew from on a blade of grass

A student performs an experiment to determine the density of a sugar solution . She obtains the following results: 4.71 g/mL, 4.67 g/mL , 4.69mL. If the actual value for the density is 4.40 g/mL, which statement below best describe her results? a. her results are precise, but not accurate b. her results are accurate, but not precise c. her results are both accurate and precise d. her results are neither accurate nor precise e. it isn't possible to determine with the information given

a. her results are precise, but not accurate

choose the homogeneous mixture from the list below a. kool-aid b. mud c. ice water d. salad dressing e. salsa

a. kool-aid

a chemical change a. occurs when methane gas is burned b. occurs when paper is shredded c. occurs when water is vaporized d. occurs when salt is dissolved in water e. occurs when kool-aid is stirred into water

a. occurs when methane gas is burned

choose the heterogeneous mixture from the list below a. sugar b. sea water c. air d. lemonade e. milk

a. sugar

the statement "in a chemical reaction, matter is neither created nor destroyed" is called a. the law of conservation of mass b. daltons atomic theory c. the scientific method d. the law of multiple proportions e. the law of definite proportions

a. the law of conservation of mass

what answer should be reported, with the correct number of significant figures for the following calculation? (433.621 - 333.9) x 11.900 a. 1.19 x 10^3 b. 1.187 x 10^3 c. 1.1868 x 10^3 d. 1.18680 x 10^3 e. 1.186799 x 10^3

b. 1.187 x 10^3

a person weighs 77.1 kg, what is their weight in pounds considering 1 kg = 2.2 pounds a. 154 pounds b. 170 pounds c. 35.0 pounds d. 162 pounds

b. 170 pounds

If the temperature is 25 degrees C, what is the temperature in K? a. 45 b. 298.15 c. 77 d. -3.89

b. 298.15

how many cm^3 are contained in 3.77 x 10^4 mm^3? a. 3.77 x 10^4 cm^3 b. 3.77 x 10^1 cm^3 c. 3.77 x 10^-10 cm^3 d. 3.77 x 10^20 cm^3 e. 3.77 x 10^6 cm^3

b. 3.77 x 10^1 cm^3

how many significant figures are in 3.408x10^4? a. 3 b. 4 c. 5 d. 7 e. 8

b. 4

what answer should be reported, with the correct number of significant figures for the following calculation? (249.362 + 41)/63.498 a. 4.6 b. 4.57 c. 4.573 d. 4.5728 e. 4.57277

b. 4.57

covert 15.0 km to miles a. 24.1 miles b. 9.32 miles c. 591 miles d. 33.1 miles

b. 9.32 miles

Which of the following elements is a halogen? A) Ne B) I C) O D) Mg E) K

b. I

choose the homogeneous mixture from the list below a. cola b. air c. concrete d. trail mix e. blood

b. air

Gold is an example of A) a compound. B) an element. C) a heterogeneous mixture. D) a homogeneous mixture.

b. an element

a substance that can't be chemically broken down into simpler substances is considered to be a. a homogeneous mixture b. an element c. a heterogeneous mixture d. a compound e. an alloy

b. an element

identify a liquid a. definite volume and definite shape b. definite volume and no shape c. definite shape and no definite volume d. no definite shape and no definite volume

b. definite volume and no shape

all of the following are S1 units of measurement except a. meter b. gram c. second d. kelvin e. mole

b. gram

dalton's atomic theory states a. all elements have several isotopes b. matter is composed of small indestructible particles c. the properties of matter are determined by the properties of atoms d. energy is neither created nor destroyed during a chemical reaction e. an atom is predominately empty space

b. matter is composed of small indestructible particles

gas is sold for $1.399 per liter in Toronto, Canada. your car needs 12.00 gallons, how much will you be charged? a. $16.79 b. $67.15 c. $4.44 d. $63.54

d. $63.54

which of the following represents a physical property? a. sodium metal is extremely reactive with chlorine gas b. mercury is a silver liquid at room temperature c. the tendency of aluminum to "rust" d. the flammability of butane fuel e. the unreactive nature of argon gas

b. mercury is a silver liquid at room temperature

How many significant figures are there in the answer for the following problem? 56.4 + 0.8822 + 21 = ? A) one B) two C) three D) four

b. two

How many significant figures are there in the answer for the following problem? [(143.7-121) x 2.06] / 0.600= ? A) one B) two C) three D) four

b. two

determine the density of an object that has a mass of 149.8an displaces 12.1 mL water when places in a graduated cylinder a. 8.08 g/mL b. 1.38 g/mL c. 12.4 g/mL d. 18.1 g/mL e. 11.4 g/mL

c. 12.4 g/mL

if the walls in a room are 955 square feet in area, and a gallon of paint covers 15 square yards, how many gallons of paint are needed for the room? a. 47 gallons b. 21 gallons c. 7.1 gallons d. 24 gallons e. 2.3 gallons

c. 7.1 gallons

if the temperature is 25 degrees C, what is the temperature in F? a. 45 b. 298.15 c. 77 d. -3.89

c. 77

if an object has a density of 8.65 g/cm^3, what is its density in units of kg/m^3? a. 8.65 x 10^-3 kg/m^3 b. 8.65 x 10^-7 kg/m^3 c. 8.65 x 10^3 kg/m^3 d. 8.65 x 10^1 kg/m^3 e. 8.65 x 10^-1 kg/m^3

c. 8.65 x 10^3 kg/m^3

a substance composed of 2 or more elements in a fixed, definite proportion is a. a homogeneous mixture b. a heterogeneous mixture c. a compound d. a solution e. an alloy

c. a compound

Crude oil is an example of A) a compound. B) an element. C) a heterogeneous mixture. D) a homogeneous mixture.

c. a heterogeneous mixture

choose the pure substance from the list below a. tea b. a casserole c. carbon monoxide d. sugar water e. pomegranate juice

c. carbon monoxide

how many significant figures are in the measurement 463.090 m? a. 2 b. 3 c. 4 d. 5 e. 6

e. 6

Which of the following statements about the phases of matter is true? a. in both solids and liquids, the atoms or molecules are loosely packed b. solids are highly compressible c. gasses are highly compressible d. atoms in solids, liquids, and gasses can move freely e. liquids have a fixed volume

c. gasses are highly compressible

which of the following represents a chemical property of hydrogen gas? a. it is gaseous at room temperature b. it is less dense than air c. it reacts explosively with oxygen d. it is colorless e. it is tasteless

c. it reacts explosively with oxygen

The factor 1,000,000 corresponds to which prefix? A) deka B) deci C) mega D) milli

c. mega

The factor 10-3 corresponds to which prefix? A) deka B) deci C) milli D) centi

c. milli

which of the following is an example of a chemical change? a. coffee brewing b. water boiling c. nails rusting d. salt dissolving in water e. freezing of water

c. nails rusting

which of the following statements about energy is false a. energy can be converted from one type to another b. the total energy of a system remains constant c. thermal energy is the energy associated with its position or composition d. kinetic energy is the capacity to do work e. systems tend to change in order to lower their potential energy

c. thermal energy is the energy associated with its position or composition

How many of the following numbers contain 3 significant figures? 0.4089.0400.04009.05 × 1024 A) one B) two C) three D) four

c. three

How many significant figures are there in the answer to the following problem? (9.992 × 3.200) + 0.610 = ? A) one B) two C) three D) four

c. three

give the components of water a. two hydrogen atoms and two oxygen atoms b. one hydrogen atom and one oxygen atom c. two hydrogen atoms and one oxygen atom d. one hydrogen atom and two oxygen atoms

c. two hydrogen atoms and one oxygen atom

molecules can be described as a. a mixture of two or more substances b. a mixture of two or more elements that has a specific ratio between components c. two or more atoms chemically joined together d. a heterogeneous mixture e. a homogeneous mixture

c. two or more atoms chemically joined together

Identify the element that has an atomic number of 40. A) neon B) calcium C) zirconium D) bromine

c. zirconium

how many significant figures are in 1009.630 mL? a. 3 b. 4 c. 5 d. 6 e. 7

e. 7

what wavelength of light would you report in units of nm, if the light had a wavelength of 7.60 x 10^-10m? a. 7.60 x 10^-3 nm b. 7.60 x 10^-19 nm c. 1.32 nm d. 0.760 nm e. 760 nm

d. 0.760

if a room requires 25.4 square yards of carpeting, what is the area of the floor in units of ft^2? a. 76.3 ft^2 b. 8.47 ft^2 c. 282 ft^2 d. 229 ft^2 e. 68.6 ft^2

d. 229 ft^2

determine the volume of an object that has a mass of 45.6 g and a density of 19.3 g/cm3 a. 87.9 mL b. 42.4 mL c. 18.5 mL d. 23.6 ml e. 31.2 mL

d. 23.6 mL

the outside air temperature is 30 degrees F, what is the temperature in K? a. 303 b. 307 c. 274 d. 272

d. 272

How many significant figures are in the measurement 5.34 g? A) 1 B) 2 C) 4 D) 3 E) 5

d. 3

Give the number of neutrons for carbon-14, with a -2 charge. A) 7 B) 4 C) 6 D) 8

d. 8

if the temperature is 178 degrees F, what is the temperature in degrees C? a. 352 b. 451 c. 67 d. 81.1 e. 378

d. 81.1

Gasoline is an example of A) a compound. B) an element. C) a heterogeneous mixture. D) a homogeneous mixture.

d. a homogeneous mixture

two or more substances in a variable proportions, where the composition is constant throughout are considered a. a compound b. an element c. a heterogeneous mixture d. a homogeneous mixture e. a crystalline solid

d. a homogeneous mixture

which of the following is an example of chemical change a. copper building materials develop a green patina over time b. water vapor condenses on the window c. ethanol evaporates d. a mixture of hydrogen and oxygen gas explodes on ignition e. a helium balloon goes up in the air

d. a mixture of hydrogen and oxygen gas explodes on ignition

What symbol is used to represent the factor 10-1? A) M B) m C) μ D) d

d. d

A student performs an experiment to determine the density of a sugar solution. She obtains the following result: 4.11 g/mL, 4.81 g/mL 3.75 g/mL. If the actual value for the density of the sugar solution is 4.75 g/mL, which statement below best describes her results? a. her results are precise, but not accurate b. her results are accurate, but not precise c. her results are both accurate and precise d. her results are neither accurate nor precise e. it isn't possible to determine with the information given

d. her results are neither accurate nor precise

An acetylene molecule contains 2 atoms of carbon. The number 2 represents how many significant figures? A) one B) two C) three D) infinite

d. infinite

the scientific method a. is just a theory b. is a strict set of rules and procedures that lead to inarguable fact c. isn't used much in modern chemistry d. is based on continued observation and experiment e. is a framework for proving an argument you know to be true

d. is based on continued observation and experiment

a physical change a. occurs when iron rusts b. occurs when sugar. is heated into caramel c. occurs when glucose is converted into energy within your cells d. occurs when water is evaporated e. occurs when propane is burned for heat

d. occurs when water is evaporated

which of the following represents a hypothesis? a. sodium reacts with water to form sodium hydroxide and hydrogen gas b. nitrogen gas is a fairly inert substance c. nickel has a silvery sheen d. when a substance combusts, it combines with air e. when wood burns, heat is given off

d. when a substance combusts, it combines with air

what answer should be reported, with the correct number of significant figures for the following calculation? (965.43 x 3.911) + 9413.4136 a. 13189 b. 13189.2 c. 1.32 x 10^4 d. 1.3 x 10^4 e. 1.319 x 10^4

e. 1.319 x 10^4

how many mg does 433 kg sample contain? a. 4.33 x 10^-4 mg b. 4.33 x 10^7 c. 4.33 x 10^-3 d. 4.33 x 10^6 e. 4.33 x 10^8

e. 4.33 x 10^8

An atom of 131Xe contains ________ electrons. A) 131 B) 185 C) 77 D) 123 E) 54

e. 54

Give the name of the element whose symbol is Na.

sodium