Chemistry a molecular approach canadian 2nd edition tro test bank

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Chemistry: A Molecular Approach, Second Cdn. Ed. (Tro) Chapter 6 Thermochemistry 6.1 Multiple Choice Questions 1) Energy that is associated with the position or composition of an object is called A) kinetic energy.

B) thermal energy.

C) potential energy.

D) chemical energy.

Answer: C Diff: 1 Type: MC Var: 1 Page Ref: 6.2 2) Which of the following signs on q and w represent a system that is doing work on the surroundings as well as losing heat to the surroundings?

A) q = - , w = B) q = +, w = + C) q = -, w = + D) q = +, w = E) None of these represent the system referenced above.

Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.3 3) Which of the following signs on q and w represent a system that is doing work on the surroundings as well as gaining heat from the surroundings?

A) q = +, w = B) q = -, w = + C) q = +, w = + D) q = -, w = E) None of these represent the system referenced above.

Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.3 4) Which of the following is TRUE if U = -95 J? A) The system is gaining 95 J, while the surroundings are losing 95 J. B) The system is losing 95 J, while the surroundings are gaining 95 J. C) Both the system and the surroundings are gaining 95 J. D) Both the system and the surroundings are losing 95 J. E) None of the above are true.

Answer: B Diff: 1 Type: MC Var: 1 Page Ref: 6.3

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5) Calculate the change in internal energy (ΔU) for a system that is giving off 45.0 kJ of heat and is performing 855 J of work on the surroundings.

A) 44.1 kJ B) -44.1 kJ C) -45.9 kJ D) 9.00 × 102 kJ E) -9.00 × 102 kJ Answer: C Diff: 1 Type: MC Var: 1 Page Ref: 6.3 6) For U to always be -, what must be true?

A) q = w B) +q > -w C) +w > -q D) -w > +q Answer: D Diff: 2 Type: MC Var: 1 Page Ref: 6.3 7) Define heat capacity.

A) the quantity of heat required to raise the temperature of 1 mol of a substance by 1 °C B) the quantity of heat required to change a system's temperature by 1 °C C) the quantity of heat required to raise the temperature of 1 g of a substance by 1 °C D) the quantity of heat required to raise the temperature of 1 g of a substance by 1 °F E) the quantity of heat required to raise the temperature of 1 L of a substance by 1 °C Answer: B Diff: 1 Type: MC Var: 1 Page Ref: 6.4 8) Define specific heat capacity.

A) the quantity of heat required to raise the temperature of 1 mol of a substance by 1 °C B) the quantity of heat required to change a system's temperature by 1 °C C) the quantity of heat required to raise the temperature of 1 g of a substance by 1 °C D) the quantity of heat required to raise the temperature of 1 g of a substance by 1 °F E) the quantity of heat required to raise the temperature of 1 L of a substance by 1 °C Answer: C Diff: 1 Type: MC Var: 1 Page Ref: 6.4 9) Define molar heat capacity.

A) the quantity of heat required to raise the temperature of 1 mol of a substance by 1 °C B) the quantity of heat required to change a system's temperature by 1 °C C) the quantity of heat required to raise the temperature of 1 g of a substance by 1 °C D) the quantity of heat required to raise the temperature of 1 g of a substance by 1 °F E) the quantity of heat required to raise the temperature of 1 L of a substance by 1 °C Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.4

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10) Identify the unit of heat capacity.

A) J °C-1 B) J g-1 °C-1 C) J mol-1 °C-1 D) g °C-1 E) mol °C-1 Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.4 11) Identify the unit of specific heat capacity.

A) °C-1 B) J g-1 °C-1 C) J mol-1 °C-1 D) g °C-1 E) mol °C-1 Answer: B Diff: 1 Type: MC Var: 1 Page Ref: 6.4 12) A piece of iron (C = 0.449 J g-1 °C-1 and a piece of gold (C = 0.128 J g-1 °C-1) have identical masses. If the iron has an initial temperature of 498 K and the gold has an initial temperature of 298 K, which of the following statements is TRUE of the outcome when the two metals are placed in contact with one another? Assume no heat is lost to the surroundings.

A) Since the two metals have the same mass, the final temperature of the two metals will be 398 K, exactly halfway between the two initial temperatures.

B) Since the two metals have the same mass, but the specific heat capacity of gold is much smaller than that of iron, the final temperature of the two metals will be closer to 298 K than to 498 K. C) Since the two metals have the same mass, the thermal energy contained in the iron and gold after reaching thermal equilibrium will be the same.

D) Since the two metals have the same mass, the thermal energy contained in each metal after equilibrium will be the same.

E) None of the above is true.

Answer: D Diff: 1 Type: MC Var: 1 Page Ref: 6.4 13) Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat?

A) 10.0 g Ag, CAg = 0.235 J g-1 °C-1 B) 10.0 g H2O, = 4.184 J g-1 °C-1 C) 10.0 g ethanol, Cethanol = 2.42 J g-1 °C-1 D) 10.0 g Fe, CFe = 0.449 J g-1 °C-1 E) 10.0 g Au, CAu = 0.128 J g-1 °C-1 Answer: E Diff: 2 Type: MC Var: 1 Page Ref: 6.4 3 Copyright © 2017 Pearson Canada, Inc.

14) Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat?

A) 50.0 g Al, CAl = 0.903 J g-1 °C-1 B) 50.0 g Cu, CCu = 0.385 J g-1 °C-1 C) 25.0 g granite, Cgranite = 0.79 J g-1 °C-1 D) 25.0 g Au, CAu = 0.128 J g-1 °C-1 E) 25.0 g Ag, CAg = 0.235 J g-1 °C-1 Answer: A Diff: 2 Type: MC Var: 1 Page Ref: 6.4 15) Calculate the amount of heat (in kJ) required to raise the temperature of a 79.0 g sample of ethanol from 298.0 K to 385.0 K. The specific heat capacity of ethanol is 2.42 J g-1 °C-1.

A) 57.0 kJ B) 16.6 kJ C) 73.6 kJ D) 28.4 kJ E) 12.9 kJ Answer: B Diff: 2 Type: MC Var: 1 Page Ref: 6.4 16) Calculate the amount of heat (in kJ) necessary to raise the temperature of 47.8 g benzene by 57.0 K. The specific heat capacity of benzene is 1.05 J g-1 °C-1.

A) 1.61 kJ B) 16.6 kJ C) 2.59 kJ D) 2.86 kJ E) 3.85 kJ Answer: D Diff: 2 Type: MC Var: 1 Page Ref: 6.4 17) Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K. A) 4.38 J °C-1 B) 2.29 J °C-1 C) 3.95 J °C-1 D) 2.53 J °C-1 E) 1.87 J °C-1 Answer: C Diff: 2 Type: MC Var: 1 Page Ref: 6.4

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18) A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0 °C. Determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J g-1 °C-1.

A) 1.51 kg B) 6.62 kg C) 1.26 kg D) 7.94 kg E) 3.64 kg Answer: A Diff: 2 Type: MC Var: 1 Page Ref: 6.4 19) Determine the final temperature of a gold nugget (mass = 376 g) that starts at 398 K and loses 4.85 kJ of heat to a snowbank when it is lost. The specific heat capacity of gold is 0.128 J g-1 °C-1.

A) 133 K B) 398 K C) 187 K D) 297 K E) 377 K Answer: D Diff: 3 Type: MC Var: 1 Page Ref: 6.4 20) A balloon is inflated from 0.0100 L to 0.500 L against an external pressure of 10.00 bar.

How much work is done in joules? (100 J = 1 L bar) A) -49.0J B) 49.0 J C) 0.490 J D) -0.490 J E) -490 J Answer: E Diff: 3 Type: MC Var: 1 Page Ref: 6.4 21) Identify what a bomb calorimeter measures.

A) measures ΔH for aqueous solutions B) measures ΔU for combustion reactions C) measures ΔH for oxidation solutions D) measures ΔT for hydrolysis solutions E) measures ΔU for reduction reactions Answer: B Diff: 1 Type: MC Var: 1 Page Ref: 6.5

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22) Calculate the change in internal energy (ΔU) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 bar. (Remember that 100 J = 1 L bar) A) +25.9 kJ B) -16.0 kJ C) -25.9 kJ D) -24.1 kJ E) 937 kJ Answer: D Diff: 2 Type: MC Var: 1 Page Ref: 6.5 23) Calculate the change in internal energy (ΔU) for a system that is absorbing 35.8 kJ of heat and is expanding from 8.00 to 24.0 L in volume at 1.00 bar. (Remember that 100 J = 1 L bar) A) +51.8 kJ B) -15.8 kJ C) -16.6 kJ D) -29.3 kJ E) +34.2 kJ Answer: E Diff: 2 Type: MC Var: 1 Page Ref: 6.5 24) A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g ) was combusted in a bomb calorimeter. If the temperature rose by 32.9 °C, use the information below to determine the heat capacity of the calorimeter.

4C6H5NH2(l) + 35O2(g) → 24CO2(g) + 14H2O(g) + 4NO2(g) DrU= -3.20 × 103 kJ mol-1 A) 97.3 kJ B) 38.9 kJ C) 5.94 kJ D) 6.84 kJ E) 12.8 kJ Answer: D Diff: 3 Type: MC

Var: 1

Page Ref: 6.5

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25) Calculate the internal energy change, ΔrU, for the combustion of 29.3 g of vitamin C (C6H8O6, molar mass = 176.124 g mol-1) if the combustion inside a bomb calorimeter, Ccal = 8.31 kJ °C-1, causes a temperature change from 21.5 °C to 68.3 °C. A) -1.78 × 103 kJ mol-1 B) -2.34 × 103 kJ mol-1 C) -6.03 × 103 kJ mol-1 D) -9.19 × 102 kJ mol-1 E) -1.67 × 102 kJ mol-1 Answer: B Diff: 3 Type: MC Var: 1 Page Ref: 6.5 26) Calculate the internal energy change, ΔrU, for the combustion of 9.467 g of L-alanine (C3H7NO2, molar mass = 89.094 g mol-1) if the combustion inside a bomb calorimeter, Ccal = 7.83 kJ °C-1, causes a temperature change from 24.7 °C to 46.1 °C. A) -1.58 × 103 kJ mol-1 B) 6.14 × 103 kJ mol-1 C) -3.48 × 103 kJ mol-1 D) -8.60 × 102 kJ mol-1 E) 3.84 × 103 kJ mol-1 Answer: A Diff: 3 Type: MC Var: 1 Page Ref: 6.5 27) Calculate the internal energy change, ΔrU, for the combustion of 6.9261 g of diethylene glycol (C4H10O3, molar mass = 106.120 g mol-1) if the combustion inside a bomb calorimeter, Ccal = 13.84 kJ °C-1, causes a temperature change from 22.8 °C to 34.0 °C. A) -4.39 × 103 kJ mol-1 B) -9.16 × 102 kJ mol-1 C) -2.37 × 103 kJ mol-1 D) 4.39 × 103 kJ mol-1 E) 1.18 × 103 kJ mol-1 Answer: C Diff: 3 Type: MC Var: 1 Page Ref: 6.5

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28) A chemist wishes to calibrate a bomb calorimeter, so he combusts 7.529 g of D-galactose, ΔcombustionU = -15.48 kJ g-1, which causes a temperature change from 26.38 °C to 34.60 °C. What should the chemist report for the value of Ccal?

A) 24.34 kJ °C-1 B) 8.009 kJ °C-1 C) 14.18 kJ °C-1 D) 16.67 kJ °C-1 E) 9.170 kJ °C-1 Answer: C Diff: 3 Type: MC Var: 1 Page Ref: 6.5 29) A chemist wishes to calibrate a bomb calorimeter, so she combusts 5.58 g of 4-pentenoic acid, ΔcombustionU = -26.77 kJ g-1, which causes a temperature change from 23.4 °C to 38.9 °C. What should the chemist report for the value of Ccal?

A) 6.10 kJ °C-1 B) 17.5 kJ °C-1 C) 28.7 kJ °C-1 D) 9.64 kJ °C-1 E) 7.61 kJ °C-1 Answer: D Diff: 3 Type: MC Var: 1 Page Ref: 6.5 30) A 21.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter according to the following reaction. If the temperature rises from 25.0 °C to 62.3 °C, determine the heat capacity of the calorimeter. The molar mass of ethanol is 46.07 g .

C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g) A) 4.99 kJ °C-1 B) 5.65 kJ °C-1 C) 63.7 kJ °C-1 D) 33.1 kJ °C-1 E) 15.7 kJ °C-1 Answer: E Diff: 3 Type: MC

Var: 1

U = -1235 kJ mol-1

Page Ref: 6.5

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31) A 4.98 g sample of aniline (C6H5NH2, molar mass = 93.13 g ) was combusted in a bomb calorimeter with a heat capacity of 4.25 kJ . If the temperature rose from 29.5 °C to 69.8 °C, determine the value of U for the combustion of aniline.

A) +7.81 × 103 kJ mol-1 B) -3.20 × 103 kJ mol-1 C) +1.71 × 103 kJ mol-1 D) -1.71 × 103 kJ mol-1 E) -7.81 × 103 kJ mol-1 Answer: B Diff: 3 Type: MC Var: 1 Page Ref: 6.5 32) A 2.38 g sample of phenol (C6H6O, molar mass = 94.11 g ) was combusted in a bomb calorimeter with a heat capacity of 6.65 kJ . If the temperature increased from 23.8 °C to 35.4 °C, determine U for the combustion of phenol.

A) -8.19 × 103 kJ mol-1 B) -5.81 × 103 kJ mol-1 C) 4.87 × 103 kJ mol-1 D) -3.05 × 103 kJ mol-1 E) 2.41 × 103 kJ mol-1 Answer: D Diff: 3 Type: MC Var: 1 Page Ref: 6.5 33) An 8.21 g sample of glycerol (C3H8O3, molar mass = 92.0938 g ) was combusted in a bomb calorimeter with a heat capacity of 10.61 kJ . If the temperature increased from 22.1 °C to 36.0 °C, determine U for the combustion of glycerol.

A) -4.38 × 103 kJ mol-1 B) 3.65 × 103 kJ mol-1 C) 2.18 × 103 kJ mol-1 D) -2.18 × 103 kJ mol-1 E) -1.65 × 103 kJ mol-1 Answer: E Diff: 3 Type: MC Var: 1 Page Ref: 6.5 34) Calculate the amount (mass) of acetic acid (C2H4O2, molar mass = 60.052 g mol-1) that causes a bomb calorimeter with a heat capacity of 8.43 kJ °C-1 to have a temperature increase from 24.5 °C to 36.8 °C. The DrU for the combustion of acetic acid is -874.2 kJ mol-1.

A) 6.18 g B) 7.12 g C) 2.18 g D) 9.66 g E) 8.68 g Answer: B Diff: 3 Type: MC Var: 1 Page Ref: 6.5 9 Copyright © 2017 Pearson Canada, Inc.

35) Calculate the amount (mass) of acetaldehyde (C2H4O, molar mass = 44.0526 g mol-1) that causes a bomb calorimeter with a heat capacity of 12.91 kJ °C-1 to have a temperature increase from 27.8 °C to 41.7 °C. The DrU for the combustion of acetaldehyde is -1166.9 kJ mol-1.

A) 6.77 g B) 8.67 g C) 4.29 g D) 7.30 g E) 5.55 g Answer: A Diff: 3 Type: MC Var: 1 Page Ref: 6.5 36) A bomb calorimeter with a heat capacity of 13.9 kJ °C-1 has an initial temperature of 21.9 °C. If 5.00 g of propanal (C3H6O, molar mass = 58.0791 g mol-1, DrU = -1822.7 kJ mol-1 for combustion) is combusted, calculate the final temperature of the calorimeter.

A) 26.1 °C B) 16.7 °C C) 33.2 °C D) 43.1 °C E) 34.0 °C Answer: C Diff: 3 Type: MC Var: 1 Page Ref: 6.5 37) The temperature rises from 25.00 °C to 29.00 °C when 3.50 g of sucrose undergoes combustion in a bomb calorimeter. Calculate U for the combustion of sucrose in kJ sucrose. The heat capacity of the calorimeter is 4.90 kJ . The molar mass of sugar is 342.3 g .

A) -1.92 × 103 kJ mol-1 B) 1.92 × 103 kJ mol-1 C) -1.23 × 103 kJ mol-1 D) 2.35 × 104 kJ mol-1 Answer: A Diff: 3 Type: MC Var: 1 Page Ref: 6.5

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38) A 12.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ . Using the information below, determine the final temperature of the calorimeter if the initial temperature is 25.0°C. The molar mass of ethanol is 46.07 g .

C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g) A) 53.4 °C B) 28.1 °C C) 111 °C D) 85.7 °C E) 74.2 °C Answer: D Diff: 3 Type: MC

Var: 1

U = -1235 kJ

Page Ref: 6.5

39) A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter according to the following reaction. If the temperature rose from 35.0 °C to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ , what is the value of U°? The molar mass of ethanol is 46.07 g .

C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g) A) -1.24 × 103 kJ mol-1 B) +1.24 × 103 kJ mol-1 C) -8.09 × 103 kJ mol-1 D) -9.55 × 103 kJ mol-1 E) +9.55 × 103 kJ mol-1 Answer: A Diff: 3 Type: MC Var: 1

U° = ?

Page Ref: 6.5

40) A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g ) was combusted in a bomb calorimeter with a heat capacity of 14.25 kJ . If the initial temperature was 32.9 °C, use the information below to determine the value of the final temperature of the calorimeter.

4C6H5NH2(l) + 35O2(g) → 24CO2(g) + 14H2O(g) + 4NO2(g) U° = -1.28 × 104 kJ A) 257 °C B) 46.6 °C C) 96.1 °C D) 41.9 °C E) 931 °C Answer: C Diff: 3 Type: MC

Var: 1

Page Ref: 6.5 11 Copyright © 2017 Pearson Canada, Inc.

41) Given w = 0, an endothermic reaction has which of the following properties?

A) +ΔH and -ΔU B) -ΔH and +ΔU C) +ΔH and +ΔU D) -ΔH and -ΔU Answer: C Diff: 1 Type: MC Var: 1 Page Ref: 6.6 42) Which of the following processes is endothermic?

A) the freezing of water B) the combustion of propane C) a hot cup of coffee (system) cools on a countertop D) the chemical reaction in a "hot pack" often used to treat sore muscles E) the vaporization of rubbing alcohol Answer: E Diff: 1 Type: MC Var: 1 Page Ref: 6.6 43) Which of the following processes is exothermic?

A) the formation of dew in the morning B) the melting of ice C) the chemical reaction in a "cold pack" often used to treat injuries D) the vaporization of water E) None of the above is exothermic.

Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.6 44) Which of the following processes is endothermic?

A) an atom emits a photon B) the condensation of water C) an atom absorbs a photon D) the electron affinity of a fluorine atom E) None of the above processes is endothermic.

Answer: C Diff: 1 Type: MC Var: 1 Page Ref: 6.6

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45) Using the following equation for the combustion of octane, calculate the heat of reaction for 100.0 g of octane. The molar mass of octane is 114.33 g .

2C8H18 + 25O2 → 16CO2 + 18H2O A) 4.82 × 103 kJ B) 4.82 kJ C) 9.64 × 103 kJ D) 1.26 × 104 kJ Answer: A Diff: 3 Type: MC

Var: 1

H° = -11018 kJ

Page Ref: 6.6

46) How much energy is required to decompose 765 g of PCl3 according to the reaction below?

The molar mass of PCl3 is 137.32 g and may be useful.

4PCl3(g) → P4(s) + 6Cl2(g) A) 2.31 × 103 kJ B) 4.33 × 103 kJ C) 6.72 × 103 kJ D) 1.68 × 103 kJ E) 5.95 × 103 kJ Answer: D Diff: 3 Type: MC

Var: 1

H° = +1207 kJ

Page Ref: 6.6

47) How much energy is evolved during the reaction of 48.7 g of Al according to the reaction below? Assume that there is excess Fe2O3.

Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(s) A) 415 kJ B) 207 kJ C) 241 kJ D) 130 kJ E) 769 kJ Answer: E Diff: 3 Type: MC

Var: 1

H° = -852 kJ

Page Ref: 6.6

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48) How much energy is evolved during the formation of 98.7 g of Fe according to the reaction below?

Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(s) A) 753 kJ B) 1.51 × 103 kJ C) 4.20 × 103 kJ D) 482 kJ E) 241 kJ Answer: A Diff: 3 Type: MC

Var: 1

H° = -852 kJ

Page Ref: 6.6

49) According to the following reaction, how much energy is required to decompose 55.0 kg of Fe3O4? The molar mass of Fe3O4 is 231.55 g .

Fe3O4(s) → 3Fe(s) + 2O2(g) A) 1.10 × 106 kJ B) 2.38 × 102 kJ C) 2.66 × 105 kJ D) 1.12 × 103 kJ E) 3.44 × 104 kJ Answer: C Diff: 3 Type: MC

Var: 1

H° = +1118 kJ

Page Ref: 6.6

50) Using the following thermochemical equation, determine the amount of heat produced per kg of CO2 formed during the combustion of benzene (C6H6).

2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(g) A) 1.43 × 105 kJ (kg CO2)-1 B) 2.30 × 104 kJ (kg CO2)-1 C) 4.34 × 104 kJ (kg CO2)-1 D) 1.19 × 104 kJ (kg CO2)-1 E) 8.40 × 105 kJ (kg CO2)-1 Answer: D Diff: 3 Type: MC Var: 1

H° = -6278 kJ

Page Ref: 6.6

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51) Using the following thermochemical equation, determine the amount of heat produced from the combustion of 24.3 g benzene (C6H6). The molar mass of benzene is 78.11 g 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(g) A) 3910 kJ C6H6 B) 1950 kJ C6H6 C) 977 kJ C6H6 D) 40.1 kJ C6H6 E) 0.302 kJ C6H6 Answer: C Diff: 3 Type: MC

Var: 1

H° = -6278 kJ

Page Ref: 6.6

52) Using the following equation for the combustion of octane, calculate the amount of moles of carbon dioxide formed from 100.0 g of octane. The molar mass of octane is 114.33 g . The molar mass of carbon dioxide is 44.0095 g .

2C8H18 + 25O2 → 16CO2 + 18H2O A) 18.18 moles B) 6.997 moles C) 14.00 moles D) 8.000 moles E) 10.93 moles Answer: B Diff: 3 Type: MC

Var: 1

H° = -11018 kJ

Page Ref: 6.6

53) Using the following equation for the combustion of octane, calculate the amount of moles of oxygen that reacts with 100.0 g of octane. The molar mass of octane is 114.33 g . The molar mass of carbon dioxide is 44.0095 g .

2C8H18 + 25O2 → 16CO2 + 18H2O A) 18.18 moles B) 6.997 moles C) 14.00 moles D) 8.000 moles E) 10.93 moles Answer: E Diff: 3 Type: MC

Var: 1

H° = -11018 kJ

Page Ref: 6.6

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54) According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6 and 72.5 g Cl2? The molar mass of B2H6 is 27.67 g .

B2H6(g) + 6Cl2(g) → 2BCl3(g) + 6HCl(g) A) 1640 kJ B) 238 kJ C) 1430 kJ D) 3070 kJ E) 429 kJ Answer: B Diff: 3 Type: MC

Var: 1

H° = -1396 kJ

Page Ref: 6.6

55) According to the following reaction, how much energy is evolved during the reaction of 2.50 L B2H6 and 5.65 L Cl2 (both gases are initially at STP)? The molar mass of B2H6 is 27.67 g .

B2H6(g) + 6Cl2(g) → 2BCl3(g) + 6HCl(g) A) 57.8 kJ B) 156 kJ C) 215 kJ D) 352 kJ E) 508 kJ Answer: A Diff: 3 Type: MC

Var: 1

H° = -1396 kJ

Page Ref: 6.6

56) According to the following thermochemical equation, what mass of HF (in g) must react to produce 345 kJ of energy? Assume excess SiO2.

SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(l) A) 42.7 g B) 37.5 g C) 150. g D) 107 g E) 173 g Answer: C Diff: 3 Type: MC

Var: 1

H° = -184 kJ

Page Ref: 6.6

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57) According to the following thermochemical equation, what mass of H2O (in g) must form to produce 975 kJ of energy?

SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(l) A) 68.0 g B) 102 g C) 54.1 g D) 191 g E) 95.5 g Answer: D Diff: 3 Type: MC

Var: 1

H° = -184 kJ

Page Ref: 6.6

58) Using the following equation for the combustion of octane, calculate the amount of grams of carbon dioxide formed from 100.0 g of octane. The molar mass of octane is 114.33 g mol-1. The molar mass of carbon dioxide is 44.0095 g mol-1.

2C8H18 + 25O2 → 16CO2 + 18H2O A) 800.1 g B) 307.9 g C) 260.1 g D) 792.3 g Answer: B Diff: 3 Type: MC

Var: 1

H° = -11018 kJ

Page Ref: 6.6

59) What volume of benzene (C6H6, d = 0.88 g mL-1, molar mass = 78.11 g mol-1) is required to produce 1.5 × 103 kJ of heat according to the following reaction?

2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(g) A) 75 mL B) 37 mL C) 21 mL D) 19 mL E) 42 mL Answer: E Diff: 3 Type: MC

Var: 1

H° = -6278 kJ

Page Ref: 6.6

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60) Identify what a coffee cup calorimeter measures.

A) measures ΔH for aqueous solutions B) measures ΔU for combustion reactions C) measures ΔH for oxidation solutions D) measures ΔT for hydrolysis solutions E) measures ΔU for reduction reactions Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.7 61) Which of the following statements is TRUE? A) State functions do not depend on the path taken to arrive at a particular state.

B) U can be determined using constant volume calorimetry.

C) Energy is neither created nor destroyed, excluding nuclear reactions.

D) H can be determined using constant pressure calorimetry.

E) All of the above are true.

Answer: E Diff: 1 Type: MC Var: 1 Page Ref: 6.7 62) Two aqueous solutions are both at room temperature and are then mixed in a coffee cup calorimeter. The reaction causes the temperature of the resulting solution to fall below room temperature. Which of the following statements is TRUE? A) The products have a lower potential energy than the reactants.

B) This type of experiment will provide data to calculate U. C) The reaction is exothermic.

D) Energy is leaving the system during the reaction.

E) None of the above statements is true.

Answer: E Diff: 2 Type: MC Var: 1 Page Ref: 6.7 63) Calculate the heat transfer, in J, when 5.00 g of chromium (specific heat capacity = 0.449 J g-1 °C-1) at 0.00 °C is placed in 50.0 mL of water. The final temperature of the water is 23.8 °C. The chromium is defined as the system in this scenario.

A) -53 J B) 53 J C) 82 J D) -82 J E) 93 J Answer: B Diff: 2 Type: MC Var: 1 Page Ref: 6.7

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64) Calculate the heat transfer (J) when 3.15 g of platinum (specific heat capacity = 0.133 J g-1 °C-1) at 86.1 °C cools to room temperature, 24.3 °C. A) -26 J B) 26 J C) -60 J D) 60 J E) -17 J Answer: A Diff: 2 Type: MC Var: 1 Page Ref: 6.7 65) Calculate the heat transfer, in kJ, when 1.287 kg of chicken breast (specific heat capacity = 1.82 J g-1 °C-1) is removed from a freezer at -17.3 °C and allowed to warm up to 0.00 °C. You need not be concerned about melting of ice or any other phase changes.

A) -0.0405 kJ B) 0.0405 kJ C) -40.5 kJ D) 40.5 kJ E) 8.65 kJ Answer: D Diff: 2 Type: MC Var: 1 Page Ref: 6.7 66) Calculate the initial temperature of 648 g of cucumber (specific heat capacity = 1.88 J g-1 °C-1) that absorbs 19857 J of heat while warming up to room temperature, 24.8 °C. A) 9.62 °C B) 8.50 °C C) 10.3 °C D) 14.8 °C E) 3.41 °C Answer: B Diff: 2 Type: MC Var: 1 Page Ref: 6.7 67) Calculate the initial temperature of 448 g of grapes (specific heat capacity = 1.76 J g-1 °C-1) that absorb 17472 J of heat while warming up to room temperature, 23.1 °C. A) 3.15 °C B) 0.941 °C C) -13.5 °C D) 8.49 °C E) 5.23 °C Answer: B Diff: 2 Type: MC Var: 1 Page Ref: 6.7

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68) Calculate the initial temperature of 21.8 g of lithium (specific heat capacity = 3.582 J g-1 °C1) that absorbs 1642 J of energy from the surroundings and has a final temperature of 31.08 °C. A) 52.11 °C B) 38.04 °C C) 26.74 °C D) 10.05 °C E) 3.17 °C Answer: D Diff: 2 Type: MC Var: 1 Page Ref: 6.7 69) Calculate the final temperature of 82.1 g of molecular hydrogen (specific heat capacity = 14.304 J g-1 °C-1) initially at 5.48 °C that absorbs 57 kJ of energy from the surroundings.

A) 14 °C B) 24 °C C) 34 °C D) 44 °C E) 54 °C Answer: E Diff: 2 Type: MC Var: 1 Page Ref: 6.7 70) Calculate the final temperature of 68.4 g of molecular hydrogen (specific heat capacity = 14.304 J g-1 °C-1) initially at 8.24 °C that releases 25.3 kJ of energy into the surroundings.

A) 34.1 °C B) 17.6 °C C) -34.1 °C D) -17.6 °C E) -8.70 °C Answer: D Diff: 2 Type: MC Var: 1 Page Ref: 6.7 71) Calculate the final temperature of 6.84 g of praseodymium (specific heat capacity = 0.193 J g-1 °C-1) initially at 26.8 °C that releases 11.3 J of energy into the surroundings.

A) 14.3°C B) 18.2 °C C) 21.6 °C D) 23.8 °C E) 8.17 °C Answer: B Diff: 2 Type: MC Var: 1 Page Ref: 6.7

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72) Astatine is an extremely rare element with an estimated 28 g total on Earth. How much energy would be required to heat Earth's entire supply of astatine by 10.0 °C assuming it has a specific heat capacity similar to iodine, 0.214 J g-1 °C-1?

A) 60 J B) 24 J C) 130 J D) 14 J E) 250 J Answer: A Diff: 2 Type: MC Var: 1 Page Ref: 6.7 73) An unknown metal alloy, mass = 26.3 g, has a temperature increase of 8.31 °C after a heat transfer of 94.0 J. Calculate the specific heat capacity of the alloy.

A) 0.813 J g-1 °C-1 B) 0.517 J g-1 °C-1 C) 0.349 J g-1 °C-1 D) 0.288 J g-1 °C-1 E) 0.430 J g-1 °C-1 Answer: E Diff: 2 Type: MC Var: 1 Page Ref: 6.7 74) An unknown metal alloy, mass = 36.1 g, has a temperature change of 31.6 to 24.8 °C after a heat transfer of -103.0 J. Calculate the specific heat capacity of the alloy.

A) 0.500 J g-1 °C-1 B) 0.384 J g-1 °C-1 C) 0.579 J g-1 °C-1 D) 0.420 J g-1 °C-1 E) 1.85 J g-1 °C-1 Answer: D Diff: 2 Type: MC Var: 1 Page Ref: 6.7 75) An unknown metal alloy, specific heat capacity = 0.613 J g-1 °C-1, has a temperature change of 31.02 to 24.77 °C after a heat transfer of -106.4 J. Calculate the mass of the alloy in question.

A) 16.8 g B) 12.7 g C) 38.3 g D) 27.8 g E) 9.17 g Answer: D Diff: 2 Type: MC Var: 1 Page Ref: 6.7

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76) An unknown metal alloy, specific heat capacity = 0.372 J g-1 °C-1, has a temperature change of +21.7 °C after a heat transfer of 216.4 J. Calculate the mass of the alloy in question.

A) 14.8 g B) 19.0 g C) 36.2 g D) 21.5 g E) 26.8 g Answer: E Diff: 2 Type: MC Var: 1 Page Ref: 6.7 77) A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J °C-1 and water = 4.184 J °C-1.

A) 348 K B) 308 K C) 287 K D) 325 K E) 388 K Answer: B Diff: 3 Type: MC Var: 1 Page Ref: 6.7 78) A student is preparing to perform a series of calorimetry experiments. She first wishes to determine the calorimeter constant (Ccal) for her coffee cup calorimeter. She pours a 50.0 mL sample of water at 345 K into the calorimeter containing a 50.0 mL sample of water at 298 K. She carefully records the final temperature of the water as 317 K. What is the value of Ccal for the calorimeter?

A) 19 J K-1 B) 28 J K-1 C) 99 J K-1 D) 21 J K-1 E) 76 J K-1 Answer: C Diff: 3 Type: MC Var: 1 Page Ref: 6.7

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79) A 100.0 mL sample of 0.300 mol L-1 NaOH is mixed with a 100.0 mL sample of 0.300 mol L-1 HNO3 in a coffee cup calorimeter. If both solutions were initially at 35.00 °C and the temperature of the resulting solution was recorded as 37.00 °C, determine the H° (in units of kJ ) for the neutralization reaction between aqueous NaOH and HNO3 . Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2) that the density and the heat capacity of the resulting solution are the same as water.

A) -55.7 kJ mol-1 B) -169 kJ mol-1 C) -16.7 kJ mol-1 D) -27.9 kJ mol-1 E) -34.4 kJ mol-1 Answer: A Diff: 3 Type: MC Var: 1 Page Ref: 6.7 80) Calculate the enthalpy of solution for the dissolution of sodium chloride, NaCl, molar mass = 58.443 g mol-1. When 6.93 g of NaCl is dissolved in a coffee cup calorimeter containing 100.0 mL of water the temperature dropped from 23.5 °C to 22.4 °C. The specific heat of water is 4.184 J g-1 °C-1, and assume the density of the solution is 1.00 g mL-1.

A) -2.8 kJ mol-1 B) 3.9 kJ mol-1 C) -6.4 kJ mol-1 D) 4.1 kJ mol-1 E) 6.3 kJ mol-1 Answer: B Diff: 3 Type: MC Var: 1 Page Ref: 6.7 81) Calculate the enthalpy of solution for the dissolution of lithium iodide, LiI, molar mass = 133.85 g mol-1. When 1.49 g of LiI is dissolved in a coffee cup calorimeter containing 75.0 mL of water the temperature increased from 23.5 °C to 25.7 °C. The specific heat of water is 4.184 J g-1 °C-1, and assume the density of the solution is 1.00 g mL-1.

A) 30 kJ mol-1 B) 18 kJ mol-1 C) -62 kJ mol-1 D) -39 kJ mol-1 E) -76 kJ mol-1 Answer: C Diff: 3 Type: MC Var: 1 Page Ref: 6.7

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82) Calculate the mass of NH4ClO4, molar mass = 117.49 g mol-1, required to create a temperature change of -1.0 °C in a coffee cup calorimeter containing 115 mL of water. The enthalpy of solution for NH4ClO4 is 33.47 kJ mol-1. The specific heat of water is 4.184 J g-1 °C-1, and assume the density of the solution is 1.00 g mL-1.

A) 1.7 g B) 3.2 g C) 2.8 g D) 4.0 g E) 0.83 g Answer: A Diff: 3 Type: MC Var: 1 Page Ref: 6.7 83) Calculate the mass of sodium cyanate (NaOCN, molar mass = 65.0066 g mol-1) required to lower the temperature from 24.1 °C to 23.0 °C in a coffee cup calorimeter containing 98 mL of water. The enthalpy of solution for NaOCN is 19.20 kJ mol-1. The specific heat of water is 4.184 J g-1 °C-1 and assume the density of the solution is 1.00 g mL-1.

A) 0.75 g B) 1.1 g C) 3.8 g D) 1.5 g E) 4.8 g Answer: D Diff: 3 Type: MC Var: 1 Page Ref: 6.7 84) 10.618 g of an unknown salt is dissolved in a coffee cup calorimeter that contains 50.0 mL of water. The measured temperature decreased from 23.8 °C to 22.7 °C. Identify the unknown salt.

The specific heat of water is 4.184 J g-1 °C-1, and assume the density of the solution is 1.00 g mL-1.

A) NaF, H = 0.91 kJ mol-1 B) NaBr, H = -0.60 kJ mol-1 C) NaNO3, D) LiNO3,

H = 20.50 kJ mol-1 H = -2.51 kJ mol-1

E) LiBr∙2H2O, H = -23.26 kJ mol-1 Answer: A Diff: 3 Type: MC Var: 1 Page Ref: 6.7

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85) 9.26 g of an unknown solid is dissolved in a coffee cup calorimeter that contains 62.0 mL of water. The measured temperature increased from 23.4 °C to 24.7 °C. The specific heat of water is 4.184 J g-1 °C-1, and assume the density of the solution is 1.00 g mL-1. Calculate the molecular weight of the unknown solid if the H was determined to be -2.51 kJ mol-1 via another experiment.

A) 69 g mol-1 B) 48 g mol-1 C) 76 g mol-1 D) 184 g mol-1 E) 93 g mol-1 Answer: A Diff: 3 Type: MC Var: 1 Page Ref: 6.7 86) A piece of gold with a mass of 21.0 g was heated to 100.0 °C and placed inside a coffee cup calorimeter. The temperature of the water inside the calorimeter increased from 23.8 °C to 25.5 °C. The specific heat capacity of water is 4.184 J g-1 °C-1 and the specific heat capacity of gold is 0.129 J g-1 °C-1. Calculate the mass of water contained inside the calorimeter.

A) 28.4 g B) 16.0 g C) 21.0 g D) 39.5 g E) 32.9 g Answer: A Diff: 3 Type: MC Var: 1 Page Ref: 6.7 87) A piece of uranium with a mass of 12.1 g and an initial temperature of 60.2 °C was placed inside a coffee cup calorimeter. The temperature of the water inside the calorimeter increased from 22.8 °C to 23.9 °C. The specific heat capacity of water is 4.184 J g-1 °C-1 and the specific heat capacity of uranium is 0.116 J g-1 °C-1. Calculate the mass of water contained inside the calorimeter.

A) 1.2 g B) 26 g C) 8.4 g D) 17 g E) 11 g Answer: E Diff: 3 Type: MC Var: 1 Page Ref: 6.7

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88) Calculate the final temperature of a 38.1 g piece of graphitic carbon, originally at 100.0 °C, placed inside a coffee cup calorimeter containing 68.0 mL of water at 24.6 °C. The specific heat capacity of water is 4.184 J g-1 °C-1, the specific heat capacity of graphitic carbon is 0.709 J g-1 °C-1, and the density of water is 1.00 g mL-1.

A) 14.7 °C B) 26.8 °C C) 31.1 °C D) 28.6 °C E) 34.0 °C Answer: C Diff: 3 Type: MC Var: 1 Page Ref: 6.7 89) Calculate the final temperature of a 63.7 g piece of palladium, originally at 100.0 °C, placed inside a coffee cup calorimeter containing 115.0 mL of water at 21.8 °C. The specific heat capacity of water is 4.184 J g-1 °C-1, the specific heat capacity of palladium is 0.246 J g-1 °C-1, and the density of water is 1.00 g mL-1.

A) 19.3 °C B) 26.0 °C C) 32.8 °C D) 24.3 °C E) 29.6 °C Answer: D Diff: 3 Type: MC

Var: 1

Page Ref: 6.7

90) Two solutions, initially at 24.60 °C, are mixed in a coffee cup calorimeter (Ccal = 15.5 J °C1). When a 100.0 mL volume of 0.100 mol L-1 AgNO3 solution is mixed with a 100.0 mL sample of 0.200 mol L-1 NaCl solution, the temperature in the calorimeter rises to 25.30 °C. Determine the DrH° for the reaction as written below. Assume that the density and specific heat capacity of the solutions is the same as that of water.

NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) DrH° = ?

A) -35 kJ mol-1 B) -59 kJ mol-1 C) -250 kJ mol-1 D) -16 kJ mol-1 E) -140 kJ mol-1 Answer: B Diff: 3 Type: MC

Var: 1

Page Ref: 6.7

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91) Two solutions, initially at 24.69 °C, are mixed in a coffee cup calorimeter (Ccal = 105.5 J °C-1). When a 200.0 mL volume of 0.100 mol L-1 AgNO3 solution is mixed with a 100.0 mL sample of 0.100 mol L-1 NaCl solution, the temperature in the calorimeter rises to 25.16 °C. Determine the H°, in units of kJ . Assume that the density and heat capacity of the solutions is the same as that of water.

Hint: Write a balanced reaction for the process.

A) -32 kJ mol-1 B) -78 kJ mol-1 C) -64 kJ mol-1 D) -25 kJ mol-1 E) -52 kJ mol-1 Answer: C Diff: 3 Type: MC

Var: 1

Page Ref: 6.7

92) Use the standard reaction enthalpies given below to determine reaction: P4(g) + 10Cl2(g) → 4PCl5(s)

H° = ?

PCl5(s) → PCl3(g) + Cl2(g)

H°= +157 kJ

P4(g) + 6Cl2(g) → 4PCl3(g)

H° = -1207 kJ

Given:

A) -1835 kJ mol-1 B) -1364 kJ mol-1 C) -1050 kJ mol-1 D) -1786 kJ mol-1 E) -2100 kJ mol-1 Answer: A Diff: 2 Type: MC

Var: 1

Page Ref: 6.8

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H° for the following

93) Use the standard reaction enthalpies given below to determine reaction: 2NO(g) + O2(g) → 2NO2(g)

H° = ?

N2(g) + O2(g) → 2NO(g)

H° = +183 kJ

1/2 N2(g) + O2(g) → NO2(g)

H° = +33 kJ

H° for the following

Given:

A) -150. kJ mol-1 B) -117 kJ mol-1 C) -333 kJ mol-1 D) +115 kJ mol-1 E) +238 kJ mol-1 Answer: B Diff: 2 Type: MC

Var: 1

Page Ref: 6.8

94) Use the standard reaction enthalpies given below to determine reaction: 2S(s) + 3O2(g) → 2SO3(g)

H° = ?

SO2(g) → S(s) + O2(g)

H° = +296.8 kJ

2SO2(g) + O2(g) → 2SO3(g)

H° = -197.8 kJ

Given:

A) -494.6 kJ mol-1 B) -692.4 kJ mol-1 C) -791.4 kJ mol-1 D) 1583 kJ mol-1 E) -293.0 kJ mol-1 Answer: C Diff: 2 Type: MC

Var: 1

Page Ref: 6.8

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H° for the following

95) Use the standard reaction enthalpies given below to determine reaction: 4SO3(g) → 4S(s) + 6O2(g)

H° = ?

SO2(g) → S(s) + O2(g)

H° = +296.8 kJ

2SO2(g) + O2(g) → 2SO3(g)

H° = -197.8 kJ

Given:

A) -494.6 kJ mol-1 B) -692.4 kJ mol-1 C) -791.4 kJ mol-1 D) 1583 kJ mol-1 E) -293.0 kJ mol-1 Answer: D Diff: 2 Type: MC

Var: 1

Page Ref: 6.8

96) Which of the following is in a non-standard state?

A) a solid at 25 °F B) a liquid at 25 °C C) a solution at 1 bar D) a solution at 1 mol L-1 E) a liquid at 1 bar Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.9 97) Identify a substance that is not in its standard state.

A) CO(s) B) Ba(s) C) H2(g) D) O2(g) E) Ni(s) Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.9 98) Identify a substance that is in a non-standard state.

A) O2 B) Ca C) H D) Zn E) Ne Answer: C Diff: 1 Type: MC Var: 1 Page Ref: 6.9 29 Copyright © 2017 Pearson Canada, Inc.

H° for the following

99) Which of the following processes is exothermic?

A) the ionization of a lithium atom B) the breaking of a Cl-Cl bond C) the sublimation of dry ice (CO2(s)) D) the reaction associated with H° for an ionic compound Answer: D Diff: 1 Type: MC Var: 1 Page Ref: 6.9 100) Choose the reaction that illustrates H° for Ca(NO3)2.

A) Ca(s) + N2(g) + 3O2(g) → Ca(NO3)2(s) B) Ca2+(aq) + 2NO3-(aq) → Ca(NO3)2(aq) C) Ca(s) + 2N(g) + 6O(g) → Ca(NO3)2(s) D) Ca(NO3)2(aq) → Ca2+(aq) + 2NO3-(aq) E) Ca(NO3)2(s) → Ca(s) + N2(g) + 3O2(g) Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.9 101) Choose the reaction that illustrates H° for NaHCO3.

A) Na(s) + H2(g) + C(s) + O2(g) → NaHCO3 (s) B) Na+(aq) + HCO3 -1 (aq) → NaHCO3 (s) C) Na+(aq) + H2O (l) + CO2 (g) → NaHCO3(s) D) Na(s) + 1/2 H2(g) + C(s) + 3/2 O2(g) → NaHCO3 (s) E) Na(s) + 2 H(g) + C(s) + 3 O(g) → NaHCO3(s) Answer: D Diff: 1 Type: MC Var: 1 Page Ref: 6.9 102) Choose the thermochemical equation that illustrates A) 2Li+(aq) + SO42-(aq) → Li2SO4(aq) B) 2Li(s) + 1/8 S8(s, rhombic) + 2O2(g) → Li2SO4(s) C) Li2SO4(aq) → 2Li+(aq) + SO42-(aq) D) 8Li2SO4(s) → 16Li(s) + S8(s, rhombic) + 16O2(g) E) 16Li(s) + S8(s, rhombic) + 16O2(g) → 8Li2SO4(s) Answer: B Diff: 1 Type: MC Var: 1 Page Ref: 6.9

H° for Li2SO4.

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103) Use the

H° information provided to calculate

H° (kJ ) SO2Cl2(g) -364 H2O(l) -286 HCl(g) 92 H2SO4(l) -814 A) -256 kJ mol-1 B) +161 kJ mol-1 C) -62 kJ mol-1 D) +800. kJ mol-1 E) -422 kJ mol-1 Answer: C Diff: 2 Type: MC 104) Use the

IF7(g) IF5(g)

H° (kJ -941 -840

)

A) 101 kJ mol-1 B) -146 kJ mol-1 C) -190. kJ mol-1 D) -95 kJ mol-1 E) 24 kJ mol-1 Answer: D Diff: 2 Type: MC 105) Use the

A) -792 kJ mol-1 B) -248 kJ mol-1 C) -495 kJ mol-1 D) -578 kJ mol-1 E) -396 kJ mol-1 Answer: E Diff: 2 Type: MC

)

H° = ?

Page Ref: 6.9

H° information provided to calculate

H° for IF:

IF7(g) + I2(g) → IF5(g) + 2IF(g)

H° = -89 kJ

Var: 1

H° and

H° (kJ SO2(g) -297

SO2Cl2 (g) + 2H2O(l)→ 2HCl(g) + H2SO4(l)

Var: 1

H° and

H° for the following:

Page Ref: 6.9

H° information provided to calculate 2SO2(g) + O2(g) → 2SO3(g)

Var: 1

H° for SO3(g):

H° = -198 kJ

Page Ref: 6.9 31 Copyright © 2017 Pearson Canada, Inc.

106) Use the information provided to determine H°(kJ CH4(g) CCl4(g) HCl(g)

)

CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g) -75 -96

H° = ?

-92

A) -389 kJ mol-1 B) -113 kJ mol-1 C) +113 kJ mol-1 D) -71 kJ mol-1 E) +79 kJ mol-1 Answer: A Diff: 2 Type: MC

Var: 1

Page Ref: 6.9

107) Use the information provided to determine H° (kJ CH4(g) CHCl3(l) HCl(g)

H° for the following reaction:

)

H° for the following reaction:

CH4(g) + 3Cl2(g) → CHCl3(l) + 3HCl(g) -75

-134 -92

A) -151 kJ mol-1 B) -335 kJ mol-1 C) +662 kJ mol-1 D) +117 kJ mol-1 E) -217 kJ mol-1 Answer: B Diff: 2 Type: MC

Var: 1

Page Ref: 6.9

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H° = ?

108) Use the information provided to determine H° (kJ ) Fe2O3(s) -824 Fe3O4(s) -1118 CO(g) -111 CO2(g) A) +277 kJ mol-1 B) -577 kJ mol-1 C) -47 kJ mol-1 D) +144 kJ mol-1 E) -111 kJ mol-1 Answer: C Diff: 2 Type: MC

H° for the following reaction:

3Fe2O3(s) + CO(g) → 2Fe3O4(s) + CO2(g) H° = ?

-394

Var: 1

Page Ref: 6.9

109) Which of the following is not a major contributor to energy consumption?

A) residential B) commercial C) transportation D) industrial E) atmospheric Answer: E Diff: 1 Type: MC Var: 1 Page Ref: 6.10 110) Identify the greatest source of energy worldwide.

A) petroleum B) natural gas C) wood D) coal E) nuclear power Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.10 111) Identify the major greenhouse gas.

A) CO2 B) O2 C) CO D) NO E) NO2 Answer: A Diff: 1 Type: MC Var: 1 Page Ref: 6.10

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112) Identify an energy source that is non-renewable.

A) solar B) hydroelectric C) coal D) wind E) sun Answer: C Diff: 1 Type: MC Var: 1 Page Ref: 6.10 6.2 Algorithmic Questions 1) For a process at constant pressure, 62,000 calories of heat are absorbed. This quantity of heat is equivalent to A) 3.85 × 10-6 J. B) 1.48 × 104 J. C) 6.21 × 104 J. D) 2.59 × 105 J. Answer: D Diff: 2 Type: MC Var: 5 Page Ref: 6.1 2) Calculate the kinetic energy of a 150 g baseball moving at a speed of 39. m A) 5.8 J B) 1.1 × 102 J C) 5.8 × 103 J D) 1.1 × 105 J Answer: B Diff: 2 Type: MC Var: 5 Page Ref: 6.2

(87 mph).

3) Calculate the work, w, gained or lost by the system when a gas expands from 15 L to 40 L against a constant external pressure of 1.5199 bar.

A) -6.1 kJ B) -3.8 kJ C) +3.8 kJ D) +6.1 kJ Answer: B Diff: 2 Type: MC Var: 5 Page Ref: 6.4

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4) The specific heat capacity of liquid mercury is 0.14 J . How many joules of heat are needed to raise the temperature of 4.00 g of mercury from 19.0°C to 39.5°C? A) 5.9 × 102 J B) 33 J C) 0.72 J D) 0.0017 J E) 11 J Answer: E Diff: 3 Type: MC Var: 5 Page Ref: 6.4 5) The specific heat capacity of solid copper metal is 0.385 J . How many joules of heat are needed to raise the temperature of a 1.55 kg block of copper from 33.0°C to 77.5°C? A) 6.59 × 104 J B) 5.58 × 10-6 J C) 0.00558 J D) 1.79 × 105 J E) 2.66 × 104 J Answer: E Diff: 3 Type: MC Var: 5 Page Ref: 6.4 6) A 5.00 g sample of liquid water at 25.0 °C is heated by the addition of 145 J of energy. The final temperature of the water is ________ °C. The specific heat capacity of liquid water is A) 25.9 B) 146 C) 6.93 D) -18.1 E) 31.9 Answer: E Diff: 3 Type: MC

Var: 5

Page Ref: 6.4

7) A 6.00 g sample of copper metal at 25.0 °C is heated by the addition of 97.0 J of energy. The final temperature of the copper is ________°C. The specific heat capacity of copper is A) 26.5 B) 98.5 C) 42.5 D) 17.5 E) 67.5 Answer: E Diff: 3 Type: MC

Var: 5

Page Ref: 6.4

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8) The specific heat capacity of liquid water is 4.184 J . How many joules of heat are needed to raise the temperature of 7.00 g of water from 33.0 °C to 76.0 °C? A) 3.19 × 103 J B) 25.7 J C) 1.39 × 10-2 J D) 71.9 J E) 1.26 × 103 J Answer: E Diff: 3 Type: MC Var: 5 Page Ref: 6.4 9) The specific heat capacity of methane gas is 2.20 J . How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0 °C to 75.0 °C? A) 17.2 J B) 0.0113 J C) 88.6 J D) 1.22 × 103 J E) 429 J Answer: E Diff: 3 Type: MC Var: 4 Page Ref: 6.4 10) The specific heat of copper is 0.385 J . If 34.2 g of copper, initially at 21.0 °C, absorbs 4.689 kJ, what will be the final temperature of the copper?

A) 21.4 °C B) 23.8 °C C) 356 °C D) 377 °C Answer: D Diff: 3 Type: MC Var: 5 Page Ref: 6.4 11) A 50.0 g sample of liquid water at 25.0 °C is mixed with 19.0 g of water at 87.0 °C. The final temperature of the water is ________°C. A) 93.6 B) 13.0 C) 62.0 D) 36.1 E) 42.1 Answer: E Diff: 3 Type: MC Var: 5 Page Ref: 6.4

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12) What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g by 10.2 °C? (The specific heat of the solution is 3.733 J .)

A) -7.43 kJ B) -12.51 kJ C) 8.20 kJ D) -11.9 kJ E) 6.51 kJ Answer: D Diff: 3 Type: MC Var: 10 Page Ref: 6.4 13) The combustion of titanium with oxygen produces titanium dioxide: Ti(s) +

(g) →

(s)

When 2.090 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 91.30 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ . The heat of reaction for the combustion of a mole of Ti in this calorimeter is ________ kJ .

A) 14.9 B) 652 C) -3.40 D) -28.5 E) -1.49 × Answer: E Diff: 3 Type: MC Var: 5 Page Ref: 6.4 14) For a particular process that is carried out at constant pressure, q = 145 kJ and w = -35 kJ. Therefore, A) ΔU = 110 kJ and ΔH = 145 kJ. B) ΔU = 145 kJ and ΔH = 110 kJ. C) ΔU = 145 kJ and ΔH = 180 kJ. D) ΔU = 180 kJ and ΔH = 145 kJ. Answer: A Diff: 2 Type: MC Var: 5 Page Ref: 6.6 15) 8.000 moles of H2(g) reacts with 4.000 mol of O2(g) to form 8.000 mol of H2O(l) at 25 °C and a constant pressure of 1.0133 bar. If 546.4 kJ of heat are released during this reaction, and PΔV is equal to -29.60 kJ, then A) ΔH° = +546.4 kJ and ΔU° = +576.06 kJ. B) ΔH° = +546.4 kJ and ΔU° = +516.8 kJ. C) ΔH° = -546.4 kJ and ΔU° = -516.8 kJ. D) ΔH° = -546.4 kJ and ΔU° = -576.0 kJ. Answer: C Diff: 3 Type: MC Var: 5 Page Ref: 6.6 37 Copyright © 2017 Pearson Canada, Inc.

16) At 1.0133 bar, the heat of sublimation of gallium is 277 kJ and the heat of vaporization is 271 kJ . To the correct number of significant figures, how much heat is required to melt 5.50 mol of gallium at 1.0133 bar?

A) 6 kJ B) 33 kJ C) 244 kJ D) 274 kJ Answer: B Diff: 3 Type: MC Var: 5 Page Ref: 6.6 17) How much heat is absorbed/released when 40.00 g of NH3(g) reacts in the presence of excess (g) to produce NO(g) and H2O(l) according to the following chemical equation?

4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l)

H° = 1168 kJ

A) 685.8 kJ of heat are absorbed.

B) 685.8 kJ of heat are released.

C) 2743 kJ of heat are absorbed.

D) 2743 kJ of heat are released.

Answer: A Diff: 3 Type: MC Var: 5 Page Ref: 6.6 18) How much heat is absorbed when 50.00 g of C(s) reacts in the presence of excess SO2(g) to produce CS2(l) and CO(g) according to the following chemical equation?

5C(s) + 2SO2(g) → CS2(l) + 4CO(g) H° = 239.9 kJ A) 199.7 kJ B) 239.9 kJ C) 998.3 kJ D) 2398 kJ Answer: A Diff: 3 Type: MC

Var: 5

Page Ref: 6.6

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19) At constant pressure, the combustion of 20.0 g of C2H6(g) releases 1036 kJ of heat. What is ΔH for the reaction given below?

2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l) A) -173 kJ B) -779 kJ C) -1560 kJ D) -3120 kJ Answer: D Diff: 3 Type: MC

Var: 5

Page Ref: 6.6

20) When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of ΔH for this reaction, as written.

2CH4(g) + 3Cl2(g) → 2CHCl3(l) + 3H2(g) A) -1420 kJ B) -708 kJ C) +708 kJ D) +1420 kJ Answer: A Diff: 3 Type: MC

Var: 5

H° = ?

Page Ref: 6.6

21) In the presence of excess oxygen, methane gas burns in a constant pressure system to yield carbon dioxide and water: (g) +

(g) →

(g) +

O (l)

H = -890.0 kJ

Calculate the value of q (kJ) in this exothermic reaction when 1.90 g of methane is combusted at constant pressure.

A) -0.00946 kJ B) 0.0342 kJ C) -1.06 × kJ D) 29.3 kJ E) -106 kJ Answer: E Diff: 3 Type: MC Var: 5 Page Ref: 6.7

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22) Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: (l) →

O(l) +

(g)

H = -196 kJ

Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure?

A) -0.0217 kJ B) 1.44 kJ C) -2.31 × kJ D) -23.1 kJ E) -11.5 kJ Answer: E Diff: 3 Type: MC Var: 5 Page Ref: 6.7 23) When 2.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00 °C to 40.32 °C. If the specific heat of the solution is 4.18 J , calculate for the reaction, as written.

Ba(s) + 2H2O(l) → Ba(OH)2(aq) + H2(g) A) -431 kJ B) -3.14 kJ C) +3.14 kJ D) +431 kJ Answer: A Diff: 3 Type: MC

Var: 5

=?

Page Ref: 6.7

24) Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below. When 0.015 mol of Na is added to 100.00 g of water, the temperature of the resulting solution rises from 25.00 °C to 31.45 °C. If the specific heat of the solution is 4.18 J , calculate ΔH for the reaction, as written.

2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g) A) -5.41 kJ B) -90.0 kJ C) -180 kJ D) -360 kJ Answer: D Diff: 3 Type: MC

Var: 5

H= ?

Page Ref: 6.7

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25) When 50.0 mL of 0.400 mol L-1 Ca(NO3)2 is added to 50.0 mL of 0.800 mol L-1 NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 24.0 °C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J , calculate the final temperature of the solution.

Ca2+(aq) + 2F-(aq) → CaF2(s) A) 23.45 °C B) 24.55 °C C) 25.10 °C D) 25.65 °C Answer: B Diff: 3 Type: MC

Var: 5

H = -11.5 kJ

Page Ref: 6.7

6.3 Matching Questions Match the following.

A) kinetic energy B) potential energy C) thermal energy D) chemical energy 1) energy associated with the motion of an object Diff: 1 Type: MA Var: 1 Page Ref: 6.2 2) energy associated with the temperature of an object Diff: 1 Type: MA Var: 1 Page Ref: 6.2 3) energy associated with the position of an object Diff: 1 Type: MA Var: 1 Page Ref: 6.2 4) energy associated with the relative positions of electrons and nuclei in atoms and molecules Diff: 1 Type: MA Var: 1 Page Ref: 6.2 Answers: 1) A 2) C 3) B 4) D

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Match the following.

A) the system loses thermal energy to the surroundings B) work done on the system by the surroundings C) energy flows into the system from the surroundings D) work done by the system on the surroundings E) the system gains thermal energy from the surroundings F) energy flows out of the system into the surroundings 5) -ΔU Diff: 1

Type: MA

Var: 1

Page Ref: 6.3

6) +ΔU Diff: 1 Type: MA

Var: 1

Page Ref: 6.3

7) -w Diff: 1

Type: MA

Var: 1

Page Ref: 6.3

8) +w Diff: 1

Type: MA

Var: 1

Page Ref: 6.3

9) -q Diff: 1

Type: MA

Var: 1

Page Ref: 6.3

10) + q Diff: 1

Type: MA

Var: 1

Page Ref: 6.3

Answers: 5) F 6) C 7) D 8) B 9) A 10) E 6.4 Short Answer Questions 1) Describe the energy changes that occur when a book is held 1 m off the floor and then dropped.

Answer: The book starts out with a certain amount of potential energy (stored energy due to position). When it begins to drop, that potential energy is then converted to kinetic energy (energy of motion).

Diff: 1 Type: SA Var: 1 Page Ref: 6.2 2) Define chemical energy.

Answer: Chemical energy is the energy associated with the relative positions of electrons and nuclei in atoms and molecules.

Diff: 1 Type: SA Var: 1 Page Ref: 6.2

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3) Where does the energy absorbed during an endothermic reaction go?

Answer: During an endothermic reaction, the products are higher in potential energy than the reactants. The thermal (kinetic) energy absorbed during reaction is used in forming products with a higher potential energy.

Diff: 1 Type: SA Var: 1 Page Ref: 6.6 4) Explain the difference between ΔH and ΔU. Answer: Change in enthalpy (ΔH) only tracks the exchange of heat between a system and its surroundings, at constant pressure. Internal energy change (ΔU) tracks both heat and work exchanged between a system and its surroundings.

Diff: 1 Type: SA Var: 1 Page Ref: 6.6 5) Give the temperature and pressure for the standard state for a liquid.

Answer: For the standard state of liquid, the temperature is 25 °C (298 K) and the pressure is 1 bar (1 atm).

Diff: 1 Type: SA Var: 1 Page Ref: 6.9 6) Why are the standard heats of formation for elements in their most stable form assigned a value of 0?

Answer: We can't measure absolute enthalpy, but we can measure changes in enthalpy.

Assigning all elements in their most stable form a value of 0 gives us a starting point from which to measure all other enthalpy changes.

Diff: 1 Type: SA Var: 1 Page Ref: 6.9 7) The standard state of sulfur is ________.

Answer: rhombic sulfur Diff: 1 Type: SA Var: 1 Page Ref: 6.9 8) The standard state of carbon is ________.

Answer: graphite Diff: 1 Type: SA Var: 1 Page Ref: 6.9

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