Chapter 13 Energy And Thermochemistry Test Bank Docx - Chemistry 3 4e | Test Bank Burrows by Andrew Burrows. DOCX document preview.
Chapter 13: Energy and Thermochemistry
Test Bank
Type: true-false
Title: Chapter 13 Question 01
1) Thermodynamics is the study of systems on the microscopic scale. It explains the interrelation of energy and chemistry and relies on information about individual molecular properties to do this.
a. True
Section reference: 13.1
b. False
Section reference: 13.1
Type: fill-in-blank
Title: Chapter 13 Question 02
2) Energy generated by a chemical reaction can be transferred as a result of motion against an opposing force as ____. .
Section reference: 13.1
a. work
Type: matching question
Title: Chapter 13 Question 03
3) Match the system name to its short description.
Section reference: 13.1
a. Both matter and energy can be exchanged with its surroundings = Open
b. Only energy can be exchanged with its surroundings = Closed
c. Neither energy or matter can be exchanged with its surroundings = Isolated
Type: multiple choice question
Title: Chapter 13 Question 04
4) What type of system is the Earth and its atmosphere?
a. Open.
Section reference: 13.1
b. Closed.
Section reference: 13.1
c. Isolated.
Section reference: 13.1
d. Not possible to define as a system.
Section reference: 13.1
Type: multiple choice question
Title: Chapter 13 Question 05
5) What type of system is the Atlantic ocean?
a. Open.
Section reference: 13.1
b. Closed.
Section reference: 13.1
c. Isolated.
Section reference: 13.1
d. Not possible to define as a system.
Section reference: 13.1
Type: matching question
Title: Chapter 13 Question 06
6) The term heat capacity, C, is used to quantify heat changes; it can be defined in different ways. Match the short definition with the correct heat capacity symbol.
Section reference: 13.1
a. Specific heat capacity is the heat needed to raise the temperature of 1 gram of substance by 1 K = Cs
b. Molar heat capacity is the heat needed to raise the temperature of 1 mol of substance by 1 K = Cm
c. Molar heat capacity is the heat needed to raise the temperature of 1 mol of substance by 1 K, for a gas, measured at constant pressure = Cp
d. Molar heat capacity is the heat needed to raise the temperature of 1 mol of substance by 1 K, for a gas, measured at constant volume = Cv
Type: multiple choice question
Title: Chapter 13 Question 07
7) The molar heat capacity, Cm of gold (Au(s)) is 25.4 J K-1 mol-1. Calculate the energy (in J) required to heat a 100 g bar of gold from 25 °C to 75 °C?
a. Not possible to calculate.
Section reference: 13.1
b. 645.
Section reference: 13.1
c. 127000.
Section reference: 13.1
d. 1.
Section reference: 13.1
Type: multiple choice question
Title: Chapter 13 Question 08
8) The specific heat capacity of liquid water is 4.18 J K-1 g-1. Calculate the temperature rise (in K) when 1050 J of heat is transferred to 5 mol of water.
a. 2.79
Section reference: 13.1
b. 50.24
Section reference: 13.1
c. 48.73
Section reference: 13.1
d. 2.79 × 10-3.
Section reference: 13.1
Type: multiple choice question
Title: Chapter 13 Question 09
9) Which of the following is the definition of molar heat capacity?
a. The amount of heat energy needed to raise the temperature of 1 mol of substance by 1 K.
Section reference: 13.1
b. The amount of heat energy needed to raise the temperature of 1 g of substance by 1 K.
Section reference: 13.1
c. The amount of heat energy needed to raise the temperature of 1 kg of substance by 1 K.
Section reference: 13.1
d. The amount of heat energy needed to raise the temperature of 1 g of water by 1 K.
Section reference: 13.1
Type: multiple choice question
Title: Chapter 13 Question 10
10) The specific heat capacity of Cu (s) is 0.38 J K-1 g-1 and that of Au (s) is 0.129 J K-1 g-1. When 100 J of heat is added to 100 g of sample of each of these substances, will one experience a larger increase in temperature?
a. Yes, gold.
Section reference: 13.1
b. No.
Section reference: 13.1
c. Yes, copper.
Section reference: 13.1
d. Not enough energy to increase the temperature of either substance.
Section reference: 13.1
Type: multiple choice question
Title: Chapter 13 Question 11
11) The specific heat capacity of iron (Fe(s)) is 0.45 J K-1 g-1, how much energy ( in J) must be added to raise the temperature of a 250 g iron bar by 30 ° C?
a. 34.104.
Section reference: 13.1
b. 34104.
Section reference: 13.1
c. 3375.
Section reference: 13.1
d. 6 × 10-5.
Section reference: 13.1
Type: matching question
Title: Chapter 13 Question 12
12) Match the definition with the quantity it is describing.
Section reference: 13.2, 13.3
a. 
= Energy required to melt one mol of a pure substance at its melting point, Tm, at 1 bar pressure
b. 
= Energy required to vaporize one mole of a pure liquid at its boiling point, Tb, at 1 bar pressure
c. 
= Enthalpy change at 298 K when 1 mol of a compound is formed under standard conditions from its constituent elements in their standard states
d. 
= Enthalpy change when 1 mol of a substance reacts completely with oxygen gas at 1 bar pressure
Type: multiple choice question
Title: Chapter 13 Question 13
13) The standard enthalpy change of formation is the energy released when 1 mol of compound is formed from its constituent elements under which set of conditions?
a. Elements in their standard states and 1 bar pressure.
Section reference: 13.3
b. Elements in their standard states and 1 atm pressure.
Section reference: 13.3
c. Elements in their standard states at 101325 Pa pressure.
Section reference: 13.3
d. Elements in their standard states at any temperature and pressure.
Section reference: 13.3
Type: multiple choice question
Title: Chapter 13 Question 14
14) The standard enthalpy change of fusion and vaporization for water are +6.01 kJ mol-1 and +40.7 kJ mol-1 respectively. Why is the value for vaporization so much larger than fusion?
a. Because it is measured at a higher temperature.
Section reference: 13.2
b. Because the pressure has increased.
Section reference: 13.2
c. Because gas is released into the surroundings.
Section reference: 13.2
d. Because overcoming all intermolecular forces that hold a liquid together needs a lot of energy.
Section reference: 13.2
Type: multiple choice question
Title: Chapter 13 Question 15
15) The standard enthalpy change of vaporization of water is + 40.7 kJ mol-1. Calculate the enthalpy change (in kJ) when 15 g of water vaporizes at its boiling point at 1 bar.
a. 611.
Section reference: 13.2
b. 49.
Section reference: 13.2
c. + 34.
Section reference: 13.2
d. 3.
Section reference: 13.2
Type: multiple choice question
Title: Chapter 13 Question 16
16) Calculate the enthalpy change (in kJ mol-1) when 1 mol of solid ethanol is melted at 155.8 K and heated to 298 K. (Take the molar heat capacity of liquid ethanol to be 112 J K-1 mol-1), 
(ethanol) = + 4.60 kJ mol-1 and 
(ethanol) = + 43.5 kJ mol-1.
a. + 64.0
Section reference: 13.2
b. + 20.5
Section reference: 13.2
c. + 15.9
Section reference: 13.2
d. + 38
Section reference: 13.2
Type: multiple choice question
Title: Chapter 13 Question 17
17) Calculate the standard enthalpy change (in kJ mol-1) for the hydrogenation of propene to propane at 298 K. The standard enthalpy change at 298 K for reactions of graphite and hydrogen gas to form 1 mol of each of these compounds is + 20.4 kJ mol-1 and – 103.9 kJ mol-1 respectively.
a. + 83.5
Section reference: 13.3
b. + 124.3
Section reference: 13.3
c. - 83.5
Section reference: 13.3
d. - 124.3
Section reference: 13.3
Type: multiple choice question
Title: Chapter 13 Question 18
18) Calculate the standard enthalpy change (in kJ mol-1) for the hydrogenation of ethyne to ethene at 298 K. The standard enthalpy change at 298 K for reactions of graphite and hydrogen gas to form 1 mol of each of these compounds is + 226.7 kJ mol-1 and + 52.5 kJ mol-1 respectively.
a. + 279.2
Section reference: 13.3
b. - 279.2
Section reference: 13.3
c. + 174.2
Section reference: 13.3
d. - 174.2
Section reference: 13.3
Type: multiple choice question
Title: Chapter 13 Question 19
19) Calculate the enthalpy change at 298.15 K and 1 bar pressure for the following reaction, using 
data in Appendix 7:
SiCl4 (l) + 2H2O (l) → SiO2 (s) + 4 HCl (g)
a. + 30.4 kJ mol-1.
Section reference: 13.3
b. - 30.4 kJ mol-1.
Section reference: 13.3
c. + 21.5 kJ mol-1.
Section reference: 13.3
d. - 21.5 kJ mol-1.
Section reference: 13.3
Type: multiple choice question
Title: Chapter 13 Question 20
20) Calculate the enthalpy change at 298.15 K and 1 bar pressure for the following reaction, using data in Appendix 7:
CH4 (g) + Cl2 (g) → CH3Cl (g) + HCl (g)
a. - 101.2 kJ mol-1.
Section reference: 13.3
b. + 101.2 kJ mol-1.
Section reference: 13.3
c. - 250.8 kJ mol-1.
Section reference: 13.3
d. 250.8 kJ mol-1.
Section reference: 13.3
Type: multiple choice question
Title: Chapter 13 Question 21
21) Calculate the enthalpy change at 298.15 K and 1 bar pressure for the following reaction, using data in Appendix 7:
2 Cl (g) → Cl2 (g) a. - 121.7 kJ mol-1.
Section reference: 13.3
b. 0 kJ mol-1.
Section reference: 13.3
c. - 243.4 kJ mol-1.
Section reference: 13.3
d. + 243.4 kJ mol-1.
Section reference: 13.3
Type: multiple choice question
Title: Chapter 13 Question 22
22) Calculate the enthalpy change 298.15 K and 1 bar pressure for the following reaction, using data in Appendix 7:
NH3 (g) + HNO3 (l) → NH4NO3 (s) a. + 585.8 kJ mol-1.
Section reference: 13.3
b. + 145.4 kJ mol-1.
Section reference: 13.3
c. - 585.8 kJ mol-1.
Section reference: 13.3
d. - 145.4 kJ mol-1.
Section reference: 13.3
Type: multiple response question
Title: Chapter 13 Question 23
23) The symbol 
conveys which of the following information? Select all that apply.
Section reference: 13.3
a. Standard enthalpy change of combustion.
b. Standard enthalpy change measured at 273.15 K.
c. Enthalpy change measured at 1 bar pressure.
d. Enthalpy change measured for 1 gram of substance.
Type: multiple choice question
Title: Chapter 13 Question 24
24) The combustion of glucose (C6H12O6) at 1 bar and 298 K releases 2802.5 kJ mol-1 of heat.
C6H12O6 (s) + 6 O2 (g) → 6 CO2 (g) + 6 H2O (l) Calculate the standard enthalpy change of formation of glucose (in kJ mol-1). Use 
data in Appendix 7.
a. + 2123.2
Section reference: 13.3
b. - 1273.3
Section reference: 13.3
c. + 1273.3
Section reference: 13.3
d. - 6878.3
Section reference: 13.3
Type: multiple choice question
Title: Chapter 13 Question 25
25) The combustion of ethanol (C2H5OH) at 1 bar and 298 K releases 1367 kJ mol-1 of heat.
C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (l) Calculate the standard enthalpy change of formation of ethanol (in kJ mol-1). Use data in Appendix 7.
a. - 277.4
Section reference: 13.3
b. + 277.4
Section reference: 13.3
c. - 3011.4
Section reference: 13.3
d. + 3011.4
Section reference: 13.3
Type: true-false
Title: Chapter 13 Question 26
26) Values of bond dissociation enthalpies D(A-B) are always positive because they are measured in the gas phase.
a. True
Section reference: 13.3
b. False
Section reference: 13.3
Type: multiple choice question
Title: Chapter 13 Question 27
27) Calculate 
for the following reaction:
C5H12 (g)+ 8 O2 (g)→ 5 CO2 (g) + 6 H2O (g), using the following bond enthalpies given (in kJ mol-1):
C-H = + 412
C=O = + 742
C-O = + 358
C-C = + 347
O=O = + 498
O-H = + 464
a. + 2325 kJ mol-1.
Section reference: 13.3
Section reference: 13.3
c. + 2672 kJ mol-1
Section reference: 13.3
d. - 2325 kJ mol-1.
Section reference: 13.3
Type: multiple choice question
Title: Chapter 13 Question 28
28) Calculate the enthalpy change for the following reaction :
C2H6O (g)+ 3 O2 (g)→ 2 CO2 (g) + 3 H2O (g), using the bond enthalpies given (in kJ mol-1):
C-H = + 412
C=O = + 742
C-O = + 358
C-C = + 347
O=O = + 498
O-H = + 464
a. - 1081 kJ mol-1.
Section reference: 13.3
b. + 1081 kJ mol-1.
Section reference: 13.3
c. + 1029 kJ mol-1.
Section reference: 13.3
d. - 1029 kJ mol-1.
Section reference: 13.3
Type: multiple choice question
Title: Chapter 13 Question 29
29) The enthalpy change for the complete combustion of 1 mol of methane at 1 bar and 298 K is – 890.3 kJ mol-1.
Calculate 
at 335 K.
Mean Cp / J K-1 mol-1: CH4 (g) 35.7; O2 (g) 29.4; CO2 (g) 37.1; H2O (l) 75.3.
a. – 890.3 kJ mol-1.
Section reference: 13.4
b. - 859.1 kJ mol-1.
Section reference: 13.4
c. - 888.8 kJ mol-1.
Section reference: 13.4
d. - 886.9 kJ mol-1.
Section reference: 13.4
Type: multiple choice question
Title: Chapter 13 Question 30
30) The enthalpy change for the complete combustion of 1 mol of hydrogen at 1 bar and 298 K is – 286 kJ mol-1.
Calculate 
at 323 K (in kJ mol-1).
Mean Cp / J K-1 mol-1: H2 (g) 28.8; O2 (g) 29.4; CO2 (g) 37.1; H2O (l) 75.3.
a. + 1304.
Section reference: 13.4
b. - 286.
Section reference: 13.4
c. - 284.
Section reference: 13.4
d. - 265.
Section reference: 13.4
Type: multiple response question
Title: Chapter 13 Question 31
31) When 1 mole of gas expands from a volume of 2.5 dm3 to 5 dm3 against a constant pressure of 1 atm, which of the following are true? Select all that apply.
Section reference: 13.5
a. Work is done by the system.
b. Work is done on the system.
c. Energy is gained by the system.
d. Energy is lost by the system.
Type: multiple choice question
Title: Chapter 13 Question 32
32) A reaction produces hydrogen gas. A balloon attached to the reaction vessel expands against a constant pressure of 1 atm and at the end of the reaction it is calculated that 1.5 dm3 of H2 (g) has been produced. Calculate the energy transferred as work, w, (in J).
a. - 152.
Section reference: 13.5
b. + 152.
Section reference: 13.5
c. - 1.5.
Section reference: 13.5
d. - 1.5 × 10-3.
Section reference: 13.5
Type: multiple choice question
Title: Chapter 13 Question 33
33) When 1 mol of gas expands from a volume of 2.5 dm3 to 5 dm3 against a constant pressure of 1 atm, calculate the energy transferred as work, w, (in J).
a. - 2.5 × 10-3.
Section reference: 13.5
b. + 253.
Section reference: 13.5
c. - 253.
Section reference: 13.5
d. - 2.5.
Section reference: 13.5
Type: fill-in-blank
Title: Chapter 13 Question 34
34) The First Law of thermodynamics states the principle of conservation of energy that the total quantity of energy in the Universe is ________.
Section reference: 13.5
a. constant
Type: multiple choice question
Title: Chapter 13 Question 35
35) One mole of gas is heated with 1.75 kJ of energy; it expands doing 250 J of work. Calculate the change in internal energy of the gas.
a. + 1500 J.
Section reference: 13.5
b. + 2000 J.
Section reference: 13.5
c. - 1500 J.
Section reference: 13.5
d. - 2000 J.
Section reference: 13.5
Type: multiple choice question
Title: Chapter 13 Question 36
36) For a reaction conducted at constant pressure and at 298 K the change in number of moles of gas (Δngas) is + 2. Calculate the difference (in kJ mol-1) between ΔH (enthalpy change) and ΔU (internal energy).
a. - 4.96
Section reference: 13.5
b. + 4.96.
Section reference: 13.5
c. + 2.
Section reference: 13.5
d. - 2.
Section reference: 13.5
Type: multiple choice question
Title: Chapter 13 Question 37
37) For a reaction conducted at constant pressure and at 298 K the change in number of moles of gas (Δngas) is - 1. Calculate the difference (in kJ mol-1) between ΔH (enthalpy change) and ΔU (internal energy).
a. + 2.48.
Section reference: 13.5
b. - 2.48.
Section reference: 13.5
c. + 1.
Section reference: 13.5
d. - 1.
Section reference: 13.5
Type: multiple choice question
Title: Chapter 13 Question 38
38) The combustion of ethanol (C2H5OH) at 1 bar and 298 K releases 1367 kJ mol-1 of heat.
C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (l) Calculate 
(in kJ mol-1) for ethanol.
a. + 1110.
Section reference: 13.5
b. - 3845.
Section reference: 13.5
c. - 1369.
Section reference: 13.5
Correct-
d. -1365.
Section reference: 13.5
Type: multiple response question
Title: Chapter 13 Question 39
39) Which of the following correctly characterise a bomb calorimeter? Select all that apply.
Section reference: 13.6
a. It measures the internal energy change of a reaction.
b. It measures the enthalpy change of a reaction.
c. It is a reaction chamber where the temperature is kept constant.
d. It can measure many different reactions.
Type: multiple choice question
Title: Chapter 13 Question 40
40) The calibration factor of a bomb calorimeter was calculated to be 10.27 kJ K-1. Calculate the internal energy change of combustion 
for glucose (Mr = 180.16) if the combustion at 298 K of 1.228 g caused a temperature rise of 1.847 K.
a. - 2783.
Section reference: 13.6
b. + 19.
Section reference: 13.6
c. - 19.
Section reference: 13.6
d. + 2783.
Section reference: 13.6