Honors Chemistry Everett Study Guide Final Exam

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A sample of 35.1 g of methane gas has a volume of 3.11 L at a pressure of 2.70 atm. Calculate the temperature.

46.8 K

A mixture is prepared from 15.0 L of ammonia and 15.0 L chlorine measured at the same conditions; these compounds react according to the following equation: 2NH3(g) + 3Cl2(g) --> N2(g) + 6HCl(g) When the reaction is completed, what is the volume of each gas (NH3, Cl2, N2, and HCl, respectively)? Assume the final volumes are measured under identical conditions.

5.00 L, 0.00 L, 5.00 L, 30.0 L

A gaseous mixture containing 1.5 mol Ar and 3.5 mol CO2 has a total pressure of 7.3 atm. What is the partial pressure of CO2?

5.1 atm

CH4(g) + 4Cl2(g) --> CCl4(g) + 4HCl(g), DH = -434 kJ Based on the above reaction, what energy change occurs when 1.2 moles of methane (CH4) reacts?

5.2 x 10^5 J are released

What is the kinetic energy of a 1.56-kg object moving at 94.0 km/hr?

5.32 x 10^2 kJ

What mass of NaOH is required to react exactly with 25.0 mL of 2.7 M H2SO4?

5.4 g

Calculate the work associated with the compression of a gas from 121.0 L to 80.0 L at a constant pressure of 13.1 atm.

537 L atm

Consider the reaction: C2H5OH(l) + 3O2(g) --> 2CO2(g) + 3H2O(l), DH = -1.37 x 10^3 kJ When a 21.1-g sample of ethyl alcohol (molar mass = 46.07 g/mol) is burned, how much energy is released as heat?

6.27 x 10^2 kJ

Consider a sample of gas in a container on a comfortable spring day. The Celsius temperature suddenly doubles, and you transfer the gas to a container with twice the volume of the first container. If the original pressure was 12 atm, what is a good estimate for the new pressure?

6.4 atm

An excess of sodium hydroxide is treated with 26.5 L of dry hydrogen chloride gas measured at STP. What is the mass of sodium chloride formed?

69.1 g

The valve between a 5-L tank containing a gas at 9 atm and a 10-L tank containing a gas at 6 atm is opened. Calculate the final pressure in the tanks.

7 atm

Which of the following statements is(are) true? Oxidation and reduction

A, C, and D

Calculate the density of nitrogen at STP.

1.25 g/L

If all of the chloride in a 3.734-g sample of an unknown metal chloride is precipitated as AgCl with 70.90 mL of 0.2010 M AgNO3, what is the percentage of chloride in the sample?

13.53%

Mercury vapor contains Hg atoms. What is the volume of 201 g of mercury vapor at 822 K and 0.512 atm?

132 L

What volume of H2O(g) measured at STP is produced by the combustion of 6.27 g of natural gas (CH4) according to the following equation? CH4(g) + 2O2(g) --> CO2 + H2O(g)

17.5 L

Which of the following is an incorrect designation for an atomic orbital?

The electron configuration for the carbon atom is:

1s2 2s2 2p2

The electron configuration for tin is

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p2

How many electrons can be contained in all of the orbitals with n = 4?

You take 295.5 g of a solid at 30.0°C and let it melt in 425 g of water. The water temperature decreases from 85.1°C to 30.0°C. Calculate the heat of fusion of this solid.

331 J/g

You fill a balloon with 2.50 moles of gas at 22°C at a pressure of 1.62 atm. What is the volume of the balloon?

37.4 L

A 7.94-g piece of solid CO2 (dry ice) is allowed to sublime in a balloon. The final volume of the balloon is 1.00 L at 301 K. What is the pressure of the gas?

4.46 atm

Given the equation S(s) + O2(g) --> SO2(g), DH = -296 kJ, which of the following statement(s) is (are) true? I. The reaction is exothermic. II. When 0.500 mole sulfur is reacted, 148 kJ of energy is released. III. When 32.0 g of sulfur are burned, 2.96 ´ 105 J of energy is released.

All are true

Four identical 1.0 L flasks contain the gases He, Cl2, CH4, and NH3, each at 0 C and 1 atm pressure. Which gas sample has the greatest number of molecules?

All gases the same

Which of the following lists of atoms are arranged in order of INCREASING first ionization energy?

Li<O<N<F

Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed?

Mg+2, SO4-2

Order the elements S, Cl, and F in terms of increasing ionization energy

S, Cl, F

Pressure is

defined as force per unit area

Fe has _____ that is (are) unpaired in its d orbitals

four electrons

Which conditions of P, T, and n, respectively, are most ideal?

low P, high T, low n

Gases generally have

low density

An element has the electron configuration [Kr] 5s2 4d10 5p2. The element is a(n)

metal

Gaseous chlorine is held in two separate containers at identical temperature and pressure. The volume of container 1 is 1.30 L, and it contains 6.70 mol of the gas. The volume of container 2 is 2.33 L. How many moles of the gas are in container 2?

12.0 mol

A sample of helium gas occupies 14.7 L at 23°C and 0.956 atm. What volume will it occupy at 40°C and 1.20 atm?

12.4 L

For the complete combustion of 1.000 mole of butane gas at 298 K and 1 atm pressure, DH° = -2877 kJ/mol. What will be the heat released when 2.43 g of butane is combusted under these conditions?

121 kJ

The mass of 1.12 liters of gas Y at STP is found to be 6.23 g. The molar mass of gas Y is

125 g/mol

How much heat is required to raise the temperature of a 5.75 g sample of iron (specific heat = 0.450 J/g C) from 25.0 C to 79.8 C?

142 J

Consider the following processes: 2A --> (1/2)B + C DH1 = 5 kJ/mol (3/2)B + 4C --> 2A + C + 3D DH2 = -15 kJ/mol E + 4A --> C DH3 = 10 kJ/mol Calculate DH for: C --> E + 3D

-10 kJ/mol

At 25°C, the following heats of reaction are known: 2ClF + O2 --> Cl2O + F2O 167.4 kJ/mol 2ClF3 + 2O2 --> Cl2O + 3F2O 341.4 kJ/mol 2F2 + O2 --> 2F2O -43.4 kJ/mol At the same temperature, calculate DeltaH for the reaction: ClF + F2 --> ClF3

-108.7 kJ/mol

Given: Cu2O(s) + mc201-1.jpgO2(g) --> 2CuO(s) DH° = -144 kJ Cu2O(s) --> Cu(s) + CuO(s) DH° = +11 kJ Calculate the standard enthalpy of formation of CuO(s).

-155 kJ

Calculate DH° for the reaction C4H4(g) + 2H2(g) --> C4H8(g), using the following data: DH°combustion for C4H4(g) = -2341 kJ/mol DH°combustion for H2(g) = -286 kJ/mol DH°combustion for C4H8(g) = -2755 kJ/mol

-158 kJ

Consider the following processes: 3B --> 2C + D -125 kJ/mol (1/2)A --> B 150 kJ/mol E + A --> D 350 kJ/mol Calculate DeltaH for B --> E + 2C

-175 kJ/mol

Using the following thermochemical data, calculate delta hf of Tm2O3(s). 2TmCl3(s) + 3H2O(l) --> Tm2O3(s) + 6HCl(g) DH° = 388.1 kJ/mol 2Tm(s) + 3Cl2(g) --> 2TmCl3(s) DH° = -1973.2 kJ/mol 4HCl(g) + O2(g) --> 2Cl2(g) + 2H2O(l) DH° = -202.4 kJ/mol

-1888.7 kJ/mol

Calculate the work for the expansion of CO2 from 1.0 to 4.7 liters against a pressure of 1.0 atm at constant temperature.

-3.7 L atm

Calculate the work associated with the expansion of a gas from 42.0 L to 79.0 L at a constant pressure of 14.0 atm.

-518 L atm

The standard temperature for gases is

0 C

A student weighs out 0.512 g of KHP (molar mass = 204.22 g/mol) and titrates to the equivalence point with 36.78 mL of a stock NaOH solution. What is the concentration of the stock NaOH solution? KHP is an acid with one acidic portion.

0.0682 M

A gas sample is heated from -20.0°C to 57.0°C and the volume is increased from 2.00 L to 4.50 L. If the initial pressure is 0.140 atm, what is the final pressure?

0.0811 atm

Sulfamic acid, HSO3NH2 (molar mass = 97.1 g/mol), is a strong monoprotic acid that can be used to standardize a strong base: HSO3NH2(aq) + KOH(aq) --> KSO2NH2(aq) + H2O(l) A 0.165-g sample of HSO3NH2 required 19.4 mL of an aqueous solution of KOH for a complete reaction. What is the molarity of the KOH solution?

0.0876 M

Given reaction N2 + 3H2 --> 2NH3, you mix 1 mol each of nitrogen and hydrogen gases under the same conditions in a container fitted with a piston. Calculate the ratio of volumes of the container (Vfinal/Vinitial).

0.67

You carry out the reaction represented by the following balanced equation: N2(g) + 3H2(g) --> 2NH3(g) You add an equal number of moles of nitrogen and hydrogen gases in a balloon. The volume of the balloon is 1.00 L before any reaction occurs. Determine the volume of the balloon after the reaction is complete. Assume constant temperature.

0.670 L

A glass column is filled with mercury and inverted in a pool of mercury. The mercury column stabilizes at a height of 729 mm above the pool of mercury. What is the pressure of the atmosphere?

0.959 atm

The number of unpaired electrons in the outer shell of a Cl atom is

Standard pressure for gases is

1 atm

Air has an average molar mass of 29.0 g/mol. The density of air at 0.97 atm and 30.0 C is:

1.13 g/L

You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 1.88 M solution of AgNO3(aq). Calculate the concentration of NO3-1 after the two solutions are mixed together.

1.18 M

A line in the spectrum of atomic mercury has a wavelength of 254 nm. When mercury emits a photon of light at this wavelength, the frequency of this light is

1.18 x 10^15 s^-1

Given the equation: 2KClO3(s) --> 2KCl(s) + 3O2(g) A 3.00-g sample of KClO3 is decomposed and the oxygen at 24.0°C and 0.717 atm is collected. What volume of oxygen gas will be collected assuming 100% yield?

1.25 x 10^3 mL

Given reaction 2NH3(g) + 3Cl2(g) --> N2(g) + 6HCl(g), you react 5.0 L of NH3 with 5.0 L of Cl2 measured at the same conditions in a closed container. Calculate the ratio of pressures in the container (Pfinal/Pinitial).

1.33

A 36.2 g piece of metal is heated to 81°C and dropped into a calorimeter containing 50.0 g of water (specific heat capacity of water is 4.18 J/g°C) initially at 21.7°C. The empty calorimeter has a heat capacity of 125 J/K. The final temperature of the water is 29.7°C. Ignoring significant figures, calculate the specific heat of the metal.

1.439 J/gK

What is the specific heat capacity of a metal if it requires 178.1 J to change the temperature of 15.0 g of the metal from 25.00°C to 32.00°C?

1.70 J/gC

You have a 400 mL container containing 55.0% He and 45.0% Ar by mass at 25 C and 1.5 atm total pressure. You heat the container to 100 C. Calculate the total pressure.

1.88 atm

Body temperature is about 309 K. On a cold day, what volume of air at 276 K must a person with a lung capacity of 2.2 L breathe in to fill the lungs?

1.97 L

Given the reaction 2MnO4- + 5H2O2 + 6H+ ---> 2Mn+2 + 8H2O + 5O2, determine the number of electrons involved in this reaction

A physics experiment is conducted at a pressure of 14.4 kPa. What is this pressure in mmHg?

108 mmHg

Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate. Write and balance the equation for this reaction to answer the following question.What is the sum of the coefficients when the molecular equation is balanced in standard form?

You are holding two balloons, an orange balloon and a blue balloon. The orange balloon is filled with neon (Ne) gas and the blue balloon is filled with argon (Ar) gas. The orange balloon has twice the volume of the blue balloon. Which of the following best represents the mass ratio of Ne:Ar in the balloons?

1:1

All alkaline earths have the following number of valence electrons

Balance the following oxidation-reduction reaction using the oxidation number method: Fe3+ + I- --> Fe2+ + I2 In the balanced equation, the coefficient of Fe2+ is

Consider the following unbalanced oxidation-reduction reaction: Fe+2 + Br2 --> Fe+3 + Br-1 In the balanced equation, the number of electrons transferred is

How many of the following are oxidation-reduction reactions? NaOH + HCl --> NaCl + H2O Cu + 2AgNO3 --> 2Ag + Cu(NO3)2 Mg(OH)2 --> MgO + H2O N2 + 3H2 --> 2NH3

How many unpaired electrons are there in an atom of sulfur in its ground state?

How may of the following electron configurations for the species in their ground state are correct? I. Ca: 1s22s22p63s23p64s2 II. Mg: 1s22s22p63s1 III. V: [Ar]3s23d3 IV. As: [Ar]4s23d104p3 V. P: 1s22s22p63p5

For a gas, which two variables are directly proportional to one another? 1. T and n 2. V and n 3. V and T

2 and 3 only

For an ideal gas, which factors are inversely proportional to each other (if all other conditions remain constant)?

2 only

You have 88.6 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 2.50 M solution of AgNO3(aq). Calculate the concentration of Na+ after the two solutions are mixed together.

2.07 M

A vessel with a volume of 26.9 L contains 2.80 g of nitrogen gas, 0.605 g of hydrogen gas, and 79.9 g of argon gas. At 25 C, what is the pressure in the vessel?

2.18 atm

The purity of a sample containing zinc and weighing 0.312 g is determined by measuring the amount of hydrogen formed when the sample reacts with an excess of hydrochloric acid. The determination shows the sample to be 84.0% zinc. What amount of hydrogen (measured at STP) was obtained?

2.41 x 10^21 molecules

The valve between the 2.00 L bulb, in which the gas pressure is 1.80 atm, and the 3.00 L bulb, in which the gas pressure is 3.00 atm, is opened. What is the final pressure in the two bulbs, the temperature remaining constant?

2.52 atm

A chunk of lead at 91.6°C was added to 200.0 g of water at 15.5°C. The specific heat of lead is 0.129 J/g°C, and the specific heat of water is 4.18 J/g°C. When the temperature stabilized, the temperature of the mixture was 17.9°C. Assuming no heat was lost to the surroundings, what was the mass of lead added?

211 g

A 32.5 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 24.2°C. Ignoring significant figures, calculate the mass of water in the calorimeter.

212 g

What volume of carbon dioxide measured at STP will be formed by the reaction of 1.47 mol of oxygen with 0.900 mol of ethyl alcohol, CH3CH2OH?

22.0 L

An unknown diprotic acid requires 44.39 mL of 0.111 M NaOH to completely neutralize a 0.580-g sample. Calculate the approximate molar mass of the acid.

235 g/mol

A 0.307-g sample of an unknown triprotic acid is titrated to the third equivalence point using 35.2 mL of 0.106 M NaOH. Calculate the molar mass of the acid.

247 g/mol

An automobile tire is filled with air at a pressure of 27.0 lb/in^2 at 25 C. A cold front moves through and the temperature drops to 5 C. Assuming no change in volume, what is the new tire pressure?

25.2 lb/in^2

With what volume of 5.00 M HF will 4.72 g of calcium hydroxide react completely, according to the following reaction? 2HF + Ca(OH)2 --> CaF2 + 2H2O

25.5 mL

A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6 C. Determine the temperature at which the volume of the gas is 3.42 L.

278 K

You have 41.6 g of O2 gas in a container with twice the volume as one with CO2 gas. The pressure and temperature of both containers are the same. Calculate the mass of carbon dioxide gas you have in the container.

28.6 g

Calcium hydride combines with water according to the equation: CaH2(s) + 2H2O(l) --> 2H2(g) + Ca(OH)2(s) Beginning with 84.0 g of CaH2 and 42.0 g of H2O, what volume of H2 will be produced at 273 K and a pressure of 1327 torr?

29.9 L

30.0 mL of pure water at 282 K is mixed with 50.0 mL of pure water at 306 K. What is the final temperature of the mixture?

297 K

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The balanced complete ionic equation contains which of the following terms?

2Ag+(aq)

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The balanced molecular equation contains which one of the following terms?

2AgCl(s)

When sodium chloride and lead (II) nitrate react in an aqueous solution, which of the following terms will be present in the balanced molecular equation?

2NaNO3(aq)

A given set of p orbitals contains ______ orbitals

Green light can have a wavelength of 543 nm. The energy of a photon of this light is

3.66 x 10^-19 J

Gaseous C2H4 reacts with O2 according to the following equation: C2H4(g) + 3O2(g) --> 2CO2 + H2O(g) What volume of oxygen gas at STP is needed to react with 5.75 mol of C2H4?

3.86 x 10^2

The deltaH value for the reaction 1/2O2(g) + Hg(l) --> HgO(s) is -90.8 kJ. How much heat is released when 66.9 g Hg is reacted with oxygen?

30.3 kJ

What volume does 40.5 g of N2 occupy at STP?

32.4 L

A sample of gas is in a 50.0 mL container at a pressure of 645 torr and a temperature of 25 C. The entire sample is heated to a temperature of 35 C and transferred to a new container whose volume in 98.7 mL. The pressure of the gas in the second container is about

338 torr

A mixture of KCl and KClO3 weighing 1.34 grams was heated; the dry O2 generated occupied 143 mL at STP. What percent of the original mixture was KClO3, which decomposes as follows: 2KClO3(s) --> 2KCl(s) + 3O2(g)

38.9%

When solutions of phosphoric acid and iron (III) nitrate react, which of the following terms will be present in the balanced molecular equation?

3HNO3(aq)

The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species?

3OH-(aq)

Which of the following is the highest energy orbital to a silicon atom?

An atom of fluorine contains nine electrons. How many of these electrons are in s orbitals?

If n=2, how many orbitals are possible?

Which of the following frequencies corresponds to light with the longest wavelength?

4.12 x 10^5 s^-1

What is the energy of a photon of blue light that has a wavelength of 453 nm?

4.39 x 10^-19 J

A sample of oxygen has a volume of 1.72 L at 27 C and 800.0 torr. How many oxygen molecules does it contain?

4.43 x 10^22

A 41.1-g sample of Ne gas exerts a certain pressure in a container of fixed volume. What mass of Ar is required to exert half the pressure at the same conditions of volume and temperature?

40.7 g Ar

A 3.00-g sample of an alloy (containing only Pb and Sn) was dissolved in nitric acid (HNO3). Sulfuric acid was added to this solution, which precipitated 2.37 g of PbSO4. Assuming that all of the lead was precipitated, what is the percentage of Sn in the sample? (molar mass of PbSO4 = 303.3 g/mol)

46.0% Sn

A 1.59-g sample of a metal chloride, MCl2, is dissolved in water and treated with excess aqueous silver nitrate. The silver chloride that formed weighed 3.60 g. Calculate the molar mass of M.

55.9 g/mol

The MnO4- is often used to analyze for the Fe2+ content of an aqueous solution via the reaction MnO4-(aq) + Fe2+(aq) + H+(aq) --> Fe3+(aq) + Mn2+(aq) + H2O(l) What is the ratio of Fe2+ : MnO4- in the balanced equation?

5:1

Balance the following oxidation-reduction reaction using the oxidation number method: Fe + Br2 --> Fe3+ + Br- In the balanced equation, the coefficient of Br- is

What is the wavelength of a photon of red light (in nm) whose frequency is 4.55 x 10^14 Hz?

659 nm

How many f orbitals have n = 6?

The enthalpy of fusion of ice is 6.020 kJ/mol. The heat capacity of liquid water is 75.4 J/mol C. What is the smallest number of ice cubes at 0 C, each containing one mole of water, necessary to cool 500 g of liquid water initially at 20 C and to 0 C

One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 8.93 liters against a constant external pressure of 1.00 atm. How much work (in joules) is performed on the surroundings? Ignore significant figures for this problem. (T = 300 K; 1 L·atm = 101.3 J)

803 J

The temperature of a specific amount of gas in a sealed container changes from 20.0°C to 40.0°C. If the volume remains constant, the pressure will change from 755 mmHg to

807 mmHg

A mixture contained no fluorine compound except methyl fluoroacetate, FCH2COOCH3 (molar mass = 92.07 g/mol). When chemically treated, all the fluorine was converted to CaF2 (molar mass = 78.08 g/mol). The mass of CaF2 obtained was 35.8 g. Find the mass of methyl fluoroacetate in the original mixture.

84.4 g

What is the wavelength of light that is emitted when an excited electron in the hydrogen atom falls from n=5 to n=1?

9.50 x 10^-8 m

Four identical 1.0 L flasks contain the gases He, Cl2, CH4, and NH3, each at 0 C and 1 atm pressure. For which gas are the collisions elastic?

all gases the same

Four identical 1.0 L flasks contain the gases He, Cl2, CH4, and NH3, each at 0 C and 1 atm pressure. For which gas do the molecules have the smallest average kinetic energy?

all gases the same

You have separate solutions of HCl and H2SO4 with the same concentrations in terms of molarity. You wish to neutralize a solution of NaOH. Which acid solution would require more volume (in mL) to neutralize the base?

The HCl Solution

Consider the ionization energy (IE) of the magnesium atom. Which of the following is not true?

The IE of Mg is lower than that of sodium

Which statement is true of a process in which one mole of a gas is expanded from State A to State B?

The amount of heat released in the process will depend on the path taken

In the lab, you mix two solutions (each originally at the same temperature) and the temperature of the resulting solution decreases. Which of the following is true?

The chemical reaction is absorbing energy

You mix 275.0 mL of 1.20 M lead(II) nitrate with 300.0 mL of 1.85 M potassium iodide. The lead(II) iodide is insoluble. Which of the following is false?

The final concentration of NO3- is 0.965 M

Which of the following statements is true?

The krypton 1s orbital is smaller than the helium 1s orbital because krypton's nuclear charge draws the electrons closer

Two metals of equal mass with different heat capacities are subjected to the same amount of heat. Which undergoes the smallest change in temperature?

The metal with the higher heat capacity

You have a certain mass of Helium gas (He) in a rigid steel container. You add the same mass of Neon gas (Ne) to this container. Which of the following best explains what happens? Assume the temperature is constant.

The pressure in the container increases but does not double.

On a cold winter day, a steel metal fence post feels colder than a wooden fence post of identical size because:

The specific heat capacity of steel is lower than the specific heat capacity of wood

For a particular process q = -17 kJ and w = 21kJ, which of the following statements is true?

The system does work on the surroundings

Which of the following statements is correct?

The system does work on the surroundings when an ideal gas expands against a constant external pressure.

Dalton's law of partial pressures states that:

The total pressure of a mixture of gases is the sum of the partial pressures of all of the gaseous compounds

Charles's law states that:

The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure

Boyle's law states that:

The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

1s2 2s2 2p6 3s2 3p6 4s2 3d2 is the correct electron configuration for which of the following atoms?

A reducing agent is an electron donor

True

Which of the following types of radiation has the shortest wavelength, the greatest energy, and the highest frequency?

Ultraviolet Radiation

Which of the following statements is not true?

When two nonmetals react, the compound formed is ionic

Select the correct electron configuration for Cu.

[Ar] 4s1 3d10

The electron configuration for the barium atom is

[Xe]6s2

The statement that the first ionization energy for an oxygen atom is lower than the first ionization energy for a nitrogen atom is

inconsistent with the general trend relating changes in ionization energy across a period from left to right and due to the fact that oxygen has one doubly occupied 2p orbital and nitrogen does not.

When a strontium salt is ignited, it burns with a red flame. The frequency of the light given off by this flame is greater than

infrared light

A 142-mL sample of gas is collected over water at 22°C and 753 torr. What is the volume of the dry gas at STP? (The vapor pressure of water at 22°C = 20. torr)

none of these

In which group do all the elements have the same number of valence electrons?

none of these

When solutions of carbonic acid and copper(II) hydroxide react, which of the following are spectator ions?

none of these

204 Nitrogen has five valence electrons. Consider the following electron arrangements. 2s 2p a) ¯ b) ¯ ¯ c) d) ¯ e) ¯ ¯ Which represents the ground state for N?

option a

Nitrogen has five valence electrons. Consider the following electron arrangements. Which represents the ground state for the N- ion?

option e

The SI unit of pressure is the

pascal

In the reaction P4(s) + 10Cl2(g) --> 4PCl5(s), the reducing agent is

phosphorous

Which of the following statements correctly describes the signs of q and w for the following exothermic process at P = 1 atm and T = 370 K? H2O(g) --> H2O(l)

q is negative, w is positive

Which form of electromagnetic radiation has the longest wavelength?

radio waves

In the reaction N2(g) + 3H2(g) --> 2NH3(g), N2 is

reduced

If 5.0 kJ of energy is added to a 15.5 g sample of water at 10 C, the water is

still a liquid

In the reaction 2Cs(s) + Cl2(g) --> 2CsCl(s), Cl2 is

the oxidizing agent

In the reaction C(s) + O2(g) --> CO2(g), carbon is ______.

the reducing agent

An element with the electron configuration [Xe] 6s2 4f14 5d7 would belong to which class on the periodic table?

transition elements

Germanium has ________ in its 4p orbitals

two electrons

Ti has ___ in its d orbitals.

two electrons

When ignited, a uranium compound burns with a green flame. The wavelength of the light given off by this flame is greater than that of

ultraviolet light

Which has these types of electromagnetic radiation arranged in order of increasing wavelength?

ultraviolet, visible, infared

Which has these types of electromagnetic radiation in order of decreasing energy?

ultraviolet, visible, infared

Which has these types of electromagnetic radiation arranged in order of decreasing frequency?

ultraviolet, visible, infrared

Which of the following are incorrectly paired?

x-rays - shortest wavelength

In the reaction Zn + H2SO4 --> ZnSO4 + H2, which, if any, element is oxidized?

zinc

What is the specific heat capacity of silver if it requires 86.3 J to raise the temperature of 15 grams of silver by 25°C?

0.23 J/ g C

You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 2.01 M solution of AgNO3(aq). Calculate the concentration of CrO4-2 after the two solutions are mixed together.

0.309 M

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. The net ionic equation contains which of the following terms?

Ag+(aq)

Which of the following reactions does not involve oxidation-reduction?

All are oxidation-reactions

Exactly 123.7 J will raise the temperature of 10.0 g of a metal from 25.0°C to 60.0°C. What is the specific heat capacity of the metal?

0.353 J/g C

The partial pressures of CH4, N2, and O2 in a sample of gas were found to be 135 mmHg, 508 mmHg, and 571 mmHg, respectively. Calculate the mole fraction of Nitrogen.

0.418

Consider three 1 L flasks at STP. Flask A contains NH3 gas, Flask B contains NO2 gas, and Flask 3 contains N2 gas. Which contains the largest number of molecules?

All are the same

The oxidation state of chlorine in ClO- is

The oxidation state of iodine in IO3- is:

How many f orbitals have the value n = 3?

What volume is occupied by 21.0 g of methane (CH4) at 27°C and 1.25 atm?

25.8 L

Consider 3 1 L flasks at STP. Flask A contains NH3 gas, Flask B contains NO2 gas, and Flack C contains N2 gas. In which flask do the molecules have the highest average velocity?

Flask A

Consider three 1-L flasks at STP. Flask A contains NH3 gas, flask B contains NO2 gas, and flask C contains N2 gas. In which flask are the molecules least polar and therefore most ideal in behavior?

Flask C

Which of the following is not a postulate of the kinetic molecular theory?

Gas particles have most of their mass concentrated in the center of the atom

You are holding four identical balloons each containing 10.0 g of a different gas. The balloon containing which gas is the largest balloon?

Four identical 1.0-L flasks contain the gases He, Cl2, CH4, and NH3, each at 0°C and 1 atm pressure. For which gas do the molecules have the highest average velocity?

Mendeleev is given the most credit for the concept of a periodic table of the elements because:

He emphasized its usefulness in predicting the existence and properties of unknown elements

Which of the following are oxidation-reduction reactions? I. PCl3 + Cl2 --> PCl5 II. Cu + 2AgNO3 --> Cu(NO3)2 + 2Ag III. CO2 + 2LiOH --> Li2CO3 + H2O IV. FeCl2 + 2NaOH --> Fe(OH)2 + 2NaCl

I and II

When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the net ionic equation?

I and III

When solutions of carbonic acid and aluminum hydroxide react, which of the following are NOT present in the net ionic equation? I. hydrogen ion II. carbonate ion III. aluminum ion IV. hydroxide ion

I and IV

C2H5OH(l) + 3O2(g) --> 2CO2(g) + 3H2O(l), Delta h = -1.37 x10^3 kJ For the combustion of ethyl alcohol as described in the above equation, which of the following is true?

I, II

Which of the following atoms or ions has three unpaired electrons?

A 3.54 gram sample of a certain diatomic gas occupies a volume of 3.30-L at 1.00 atm and a temperature of 45°C. Identify this gas.

In which of the following does nitrogen have an oxidation state of +4?

NO2

When solutions of carbonic acid and potassium hydroxide react, which of the following are NOT present in the complete ionic equation?

hydrogen ion

Consider the reaction between 15.0 mL of a 1.00 M aqueous solution of AgNO3 and 10.0 mL of a 1.00 M aqueous solution of K2CrO4. When these react, a precipitate is observed. What is present in the solution after the reaction is complete? Note: the solid is not considered to be in the solution.

NO3-, K+, CrO4-2, water

At 1000 C and 10. torr, the density of a certain element in the gaseous state is 2.9 x 10^-3 g/L. The element is:

Which of the following atoms would have the largest second ionization energy?

In the balanced molecular equation for the neutralization of sodium hydroxide with sulfuric acid, the products are:

Na2SO4 + 2H2O

A solution contains the ions Ag+, Pb2+, and Ni2+. Dilute solutions of NaCl, Na2SO4, and Na2S are available to separate the positive ions from each other. In order to effect separation, the solutions should be added in which order?

Na2SO4, NaCl, Na2S

Which of the following atoms has the largest ionization energy?

Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is correct?

No reaction will occur

According to the first law of thermodynamics, the energy of the universe is constant. Does this mean that DE is always equal to zero?

No, DE does not always equal zero because it refers to the system's internal energy, which is affected by heat and work.

Given a cylinder of fixed volume filled with 1 mol of argon gas, which of the following is correct? (Assume all gases obey the ideal gas law)

None of the above

Choose the element with the highest ionization energy

Of the following elements, which needs three electrons to complete its valence shell?

Which of the following statements is false?

A fluorine atom has a smaller first ionization energy than an oxygen atom.

Which of the following salts is insoluble in water?

All of these are soluble in water

A 1.00 g sample of a gaseous compound of boron and hydrogen occupies 0.820 L at 1.00 atm and 3 C. What could be the molecular formula for the compound?

B2H6

Of the following elements, which has occupied d orbitals in its ground-state neutral atoms?

Which of the following atoms has three electrons in p orbitals in its valence shell?

Which of the following processes represents the ionization energy of bromine?

Br(g) ---> Br+(g) + e-

Which of the following processes represents the ionization energy of bromine?

Br(g) --> Br+(g) + e-

When 0.72 g of a liquid is vaporized at 110°C and 0.967 atm, the gas occupies a volume of 0.559 L. The empirical formula of the gas is CH2. What is the molecular formula of the gas?

C3H6

in the reaction 2Ca(s) + O2(g) -->2CaO(s), which species is oxidized

Which of the following ions is most likely to form an insoluble sulfate?

Ca +2

Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate. What is the formula of the solid formed in the reaction?

Ca3(PO4)2

Of the following elements, which is most likely to form a negative ion with a charge of -1?

Four identical 1.0 L flasks contain the gases He, Cl2, CH4, and NH3, each at 0 C and 1 atm pressure. For which gas are the molecules diatomic?

Cl2

Four identical 1.0-L flasks contain the gases He, Cl2, CH4, and NH3, each at 0°C and 1 atm pressure. Which gas has the highest density?

Cl2

When solutions of cobalt(II) chloride and carbonic acid react, which of the following terms will be present in the net ionic equation?

CoCO3(s)

One way to isolate metals from their ores is to react the metal oxide with carbon as shown in the following reaction: 2MO(s) + C(s) --> 2M(s) + CO2(g) If 34.08 g of a metal oxide reacted with excess carbon and 4.37 L of CO2 formed at 100°C and 1.50 atm, what is the identity of the metal?

When NH3(aq) is added to Cu2+(aq), a precipitate initially forms. Its formula is:

Cu(OH)2

Aqueous solutions of sodium sulfide and copper (II) chloride are mixed together. Which statement is correct?

CuS will precipitate from the solution

For a particular process q = 20 kJ and w = 15 kJ. Which of the following statements is true?

DeltaE = 35 kJ

Who was the first chemist to recognize patterns in chemical properties of the elements?

Dobereiner

An element E has the electron configuration [Kr] 5s2 4d10 5p2. The formula for the fluoride of E is most likely

EF4

Avogadro's law states that:

Equal amounts of gases occupy the same volume at constant temperature and pressure

Order the elements S, Cl, and F in terms of increasing atomic radii

F, Cl, S

Which of the following exhibits the correct orders for both atomic radius and ionization energy, respectively? (smallest to largest)

F, O, S and S, O, F

A chemical that changes color at the endpoint of a reaction is called a colorimeter

False

Oxidation is the gain of electrons

False

Which of the following statements are false? I. It takes less energy to add an electron to nitrogen than to carbon because nitrogen will be closer to achieving a noble gas configuration. II. It takes more energy to add an electron to fluorine than to oxygen because the radius of fluorine is smaller and more repulsion would occur in the p-orbitals. III. It takes more energy to add an electron to nitrogen than to carbon because of the extra repulsions that would occur in the 2p orbitals. IV. Less energy is released in adding an electron to iodine than to chlorine because the radius of iodine is larger and the electron is added at a distance further from the nucleus.

I, II

When a hydrogen electron makes a transition from n = 3 to n = 1, which of the following statements is true? I. Energy is emitted. II. Energy is absorbed. III. The electron loses energy. IV. The electron gains energy. V. The electron cannot make this transition.

I, III

Consider the following orderings. I. Na+ < Mg2+ < Al3+ < Si4+ II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Al < Si < P < Cl Which of these give(s) a correct trend in ionization energy?

I, III, IV

In the reaction below, which species is oxidized? 2NaI + Br2 --> 2NaBr + I2

I-

Consider the reaction: C2H5OH(l) + 3O2(g) -->2CO2(g) + 3H2O(l); DeltaH = -1.37 x 10^3 kJ Consider the following propositions: I. The reaction is endothermic II. The reaction is exothermic. III. The enthalpy term would be different if the water formed was gaseous. Which of these propositions is (are) true?

II, III

In the following reaction, which species is oxidized? 8NaI + 5H2SO4 --> 4I2 + H2S + 4Na2SO4 + 4H2O

Iodine

A 45.9 g sample of a metal is heated to 95.2°C and then placed in a calorimeter containing 120.0 g of water (c = 4.18 J/g°C) at 21.6°C. The final temperature of the water is 24.5°C. Which metal was used?

Iron (c = 0.45 J/g C)

Consider a gas in a 1.0 L bulb at STP that is connected via a valve to another bulb that is initially evacuated. Answer the following concerning what occurs when the valve between the two bulbs is opened. What is true about the value of DE?

It is equal to zero

Which of the following statements is true about the ionization energy of Mg+?

It will be equal and opposite in sign to the electron affinity of Mg +2

Which of the following compounds is soluble in water?

K3PO4

Consider the following specific heats of metals. Metal Specific Heat Zinc 0.387 J/(g°C) Magnesium 1.02 J/(g°C) Iron 0.450 J/(g°C) Silver 0.237 J/(g°C) Lead 0.127 J/(g°C) If the same amount of heat is added to 25.0 g of each of the metals, which are all at the same initial temperature, which metal will have the highest temperature?

Lead

Which of the following lists of atoms are arranged in order of DECREASING atomic radius?

Li > N > O > F

In writing the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of KOH and Mg(NO3)2 are mixed, which of the following would not be written as ionic species?

Mg(OH)2

Which of the following was not an elemental property usually predicted by Mendeleev for as-yet-unknown elements?

electron configuration

Sodium losing an electron is an ____ process and fluorine losing an electron is an _____ process

Honors Chemistry Everett Study Guide Final Exam

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