Complete Test Bank Entropy And Gibbs Energy Ch.14

Chapter 14: Entropy and Gibbs Energy

Test Bank

Type: true-false

Title: Chapter 14 Question 01

1) The following substances are ordered with increasing entropy: neon gas < liquid water < a gold bar.

a. True

Section reference: 14.2

b. False

Section reference: 14.2

Type: true-false

Title: Chapter 14 Question 02

2) The entropy change for the following reaction will be negative:

C₁₁H₂₂O₁₁ (s) + 12 O₂ (g) → 12 CO₂ (g) + 11 H₂O (l)

a. True

Section reference: 14.1

b. False

Section reference: 14.1

Type: true-false

Title: Chapter 14 Question 03

3) The entropy change for the following reaction will be positive:

N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)

a. True

Section reference: 14.1

b. False

Section reference: 14.1

Type: fill-in-blank

Title: Chapter 14 Question 04

4) Entropy is identified with the amount of ________ in the system.

Section reference: 14.1, 14.2

a. disorder

Type: multiple choice question

Title: Chapter 14 Question 05

5) Calculate the entropy change (, J K^-1 mol^-1) when 1.00 mol of ethanol at its boiling point (T_b =78.45 °C) vaporizes (in the process the temperature does not change, for ethanol is + 43.5 kJ mol^-1).

a. + 124.

Section reference: 14.2

b. - 124.

Section reference: 14.2

c. + 554.

Section reference: 14.2

d. + 0.12.

Section reference: 14.2

Type: multiple choice question

Title: Chapter 14 Question 06

6) Calculate the entropy change (, J K^-1 mol^-1) when 1.00 mol of mercury at its boiling point (T_b = 356.55 °C) vaporizes (in the process the temperature does not change, for mercury is + 59.3 kJ mol^-1).

a. - 94.

Section reference: 14.2

b. + 94.

Section reference: 14.2

c. + 166.

Section reference: 14.2

d. + 0.09.

Section reference: 14.2

Type: multiple choice question

Title: Chapter 14 Question 07

7) Calculate the entropy change (, J K^-1 mol^-1) when 1.00 mol of methane at its melting point (T_m = - 182.05 °C) freezes (in the process the temperature does not change and for methane is + 0.94 kJ mol^-1).

a. - 10.3.

Section reference: 14.2

b. - 0.01.

Section reference: 14.2

c. + 10.3.

Section reference: 14.2

d. - 5.2.

Section reference: 14.2

Type: true-false

Title: Chapter 14 Question 08

8) For water = + 109 J K^-1 mol^-1 whilst = + 22 J K^-1 mol^-1. The entropy change for vaporization is larger than the entropy change for fusion because it is measured at a higher temperature.

a. True

Section reference: 14.2

b. False

Section reference: 14.2

Type: matching question

Title: Chapter 14 Question 09

9) Whether the total entropy change (ΔS_(total)) of a process is positive, negative, or equal to zero defines whether the process is spontaneous. Match the (ΔS_(total)) condition with its description.

Section reference: 14.2

a. ΔS_(total) > 0 = spontaneous process

b. ΔS_(total) < 0 = non-spontaneous process

c. ΔS_(total) = 0 = process at equilibrium

Type: multiple choice question

Title: Chapter 14 Question 10

10) Calculate the change of entropy (in J K^-1 mol^-1) when 1 mol of methanol is heated at constant pressure from 5 °C to 35 °C, the molar heat capacity, C_p, of methanol is 81.6 J K^-1 mol^-1, assume that the molar heat capacity, C_p is constant over this temperature range.

a. + 8.36.

Section reference: 14.2

b. - 8.36.

Section reference: 14.2

c. - 158.79.

Section reference: 14.2

d. + 158.79.

Section reference: 14.2

Type: multiple choice question

Title: Chapter 14 Question 11

11) Calculate the change of entropy (in J K^-1 mol^-1) when 1 mol of ethanol is cooled at constant pressure from 25 °C to 10 °C, the molar heat capacity, C_p, of ethanol is 111.5 J K^-1 mol^-1 and assume that C_p is constant over this temperature range.

a. + 5.8.

Section reference: 14.2

b. - 5.8.

Section reference: 14.2

c. - 102.2.

Section reference: 14.2

d. + 102.2.

Section reference: 14.2

Type: true-false

Title: Chapter 14 Question 12

12) When 1 mol of trichloromethane is heated from 5 °C to 20 °C at constant pressure, the change of entropy is + 6.00 J K^-1 mol^-1. When the solvent is heated further from 20 °C to 35 °C, the change in entropy will also be + 6.00 J K^-1 mol^-1.

a. True

Section reference: 14.2

b. False

Section reference: 14.2

Type: true-false

Title: Chapter 14 Question 13

13) When 1 mol of water is heated from 10 °C to 25 °C at constant pressure, the change in entropy is + 3.89 J K^-1 mol^-1. When 1 mol of methanol is heated from 10 °C to 25 °C at constant pressure, the change in entropy will be smaller.

a. True

Section reference: 14.2

b. False

Section reference: 14.2

Type: fill-in-blank

Title: Chapter 14 Question 14

14) At zero kelvin the entropy of a perfect crystal is ____.

Section reference: 14.3

a. zero

Type: multiple choice question

Title: Chapter 14 Question 15

15) Calculate the standard entropy of 1 mol of water at 20 °C and 1 bar. The molar heat capacity, C_p, of water is 75.3 J K^-1 mol^-1 and is 69.9 J K^-1 mol^-1.

a. 69.9.

Section reference: 14.3

b. - 133.5.

Section reference: 14.3

c. 68.7.

Section reference: 14.3

d. 71.1.

Section reference: 14.3

Type: true-false

Title: Chapter 14 Question 16

16) The standard entropy of ethanol, at 1 bar, is 159.9 J K^-1 mol^-1. At 315 K, its standard entropy will be larger.

a. True

Section reference: 14.3

b. False

Section reference: 14.3

Type: true-false

Title: Chapter 14 Question 17

17) The standard entropy change for the following reaction will be large and positive. CS₂ (l) + 3O₂ (g) → CO₂ (g) + 2SO₂ (g)

a. True

Section reference: 14.5

b. False

Section reference: 14.5

Type: multiple choice question

Title: Chapter 14 Question 18

18) Using data in Appendix 7, (p. 1350), calculate the standard entropy change of reaction ( in J K^-1 mol^-1) for the following reaction: CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O (l)

a. + 243.0.

Section reference: 14.5

b. - 243.0.

Section reference: 14.5

c. - 107.8.

Section reference: 14.5

d. + 107.8.

Section reference: 14.5

Type: multiple choice question

Title: Chapter 14 Question 19

19) Using data in Appendix 7, (p. 1350), calculate the standard entropy change of reaction (in J K^-1 mol^-1) for the following reaction:

NH₃ (g) + HNO₃ (l) → NH₄NO₃ (s)

a. - 197.

Section reference: 14.5

b. + 197.

Section reference: 14.5

c. -151.1.

Section reference: 14.5

d. +151.1.

Section reference: 14.5

Type: multiple choice question

Title: Chapter 14 Question 20

20) The standard entropy change, for the following reaction is:

–198.7 J K^-1 mol^-1.

N₂ (g) + 3 H₂ (g) → 2 NH₃ (g) Calculate the standard entropy change of reaction (in J K^-1 mol^-1) at 550 K.

a. - 226.

Section reference: 14.4

b. - 171.

Section reference: 14.4

c. + 226.

Section reference: 14.4

d. + 171.

Section reference: 14.4

Type: multiple choice question

Title: Chapter 14 Question 21

21) The standard entropy change, for the following reaction is: + 511.9 J K^-1 mol^-1.

C₁₂H₂₂O₁₁ (s) + 12 O₂ (g) → 12 CO₂ (g) + 11 H₂O (l) Calculate the standard entropy change of reaction (in J K^-1 mol^-1) at 390 116.85 °C.

a. + 511.9.

Section reference: 14.4

b. + 48.3.

Section reference: 14.4

c. + 379.

Section reference: 14.4

d. + 645.

Section reference: 14.4

Type: true-false

Title: Chapter 14 Question 22

22) The standard entropy change, is: – 198.7 J K^-1 mol^-1, for the following reaction: N₂ (g) + 3 H₂ (g) → 2 NH₃ (g) This violates the Second Law of thermodynamics.

a. True

Section reference: 14.2, 14.4

b. False

Section reference: 14.2, 14.4

Type: matching question

Title: Chapter 14 Question 23

23) Whether Gibbs energy change (ΔG) of a process is positive, negative, or equal to zero defines whether the process is spontaneous. Match the situation with its description.

Section reference: 14.5

a. ΔG < 0 = the reaction or process is spontaneous

b. ΔG > 0 = the reaction or process is non-spontaneous

c. ΔG = 0 = the reaction or process is at equilibrium

Type: matching question

Title: Chapter 14 Question 24

24) Match the reaction description and whether it is spontaneous and under which conditions

Section reference: 14.5

a. ΔH > 0, ΔS < 0 = Never spontaneous

b. ΔH > 0, ΔS > 0 = Spontaneous on heating

c. ΔH < 0, ΔS > 0 = Always spontaneous

d. ΔH < 0, ΔS < 0 = Spontaneous on cooling

Type: multiple choice question

Title: Chapter 14 Question 25

25) An endothermic reaction has , and . Find the temperature, T(K), at which the reaction becomes spontaneous.

a. 298.

Section reference: 14.5

b. 783.

Section reference: 14.5

c. 0.78.

Section reference: 14.5

d. 1.28.

Section reference: 14.5

Type: multiple choice question

Title: Chapter 14 Question 26

26) Using and data given below:

Calculate the standard Gibbs energy change, (kJ mol^-1), for the following reaction:

2 NH₃ (g) → N₂ (g) + 3 H₂ (g) a. + 151.

Section reference: 14.5

b. - 151.

Section reference: 14.5

c. + 33.

Section reference: 14.5

d. - 59.

Section reference: 14.5

Type: multiple choice question

Title: Chapter 14 Question 27

27) Using and data given below:

Calculate the standard Gibbs energy change, (kJ mol^-1), for the following reaction:

CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O (l) a. - 818.

Section reference: 14.5

b. + 71.5.

Section reference: 14.5

c. + 963.

Section reference: 14.5

d. - 963.

Section reference: 14.5

Type: multiple choice question

Title: Chapter 14 Question 28

28) Using data given below:

Calculate the standard Gibbs energy change, (kJ mol^-1), for the following reaction:

CO (g) + 2 H₂ (g) → CH₃OH (g) a. - 299.2.

Section reference: 14.5

b. + 299.2.

Section reference: 14.5

c. + 24.8.

Section reference: 14.5

d. - 24.8.

Section reference: 14.5

Type: multiple choice question

Title: Chapter 14 Question 29

29) Using data given below:

calculate the standard Gibbs energy change, (kJ mol^-1), for the following reaction:

CO₂ (g) + CH₄ (g) → CH₃CO₂H (l) a. - 835.1

Section reference: 14.5

b. - 55.3.

Section reference: 14.5

c. + 835.1.

Section reference: 14.5

d. + 55.3.

Section reference: 14.5

Type: multiple choice question

Title: Chapter 14 Question 30

30) Using data given below:

calculate the standard Gibbs energy change, (kJ mol^-1), for the following reaction:

C₁₂H₂₂O₁₁ (s) + 12 O₂ (g) → 12 CO₂ (g) + 11 H₂O (l) a. + 911.5.

Section reference: 14.5

b. - 5797.9.

Section reference: 14.5

c. + 5797.9.

Section reference: 14.5

d. - 911.5.

Section reference: 14.5

Type: true-false

Title: Chapter 14 Question 31

31) An endothermic reaction with a positive entropy change will become spontaneous on cooling.

a. True

Section reference: 14.5

b. False

Section reference: 14.5

Type: multiple choice question

Title: Chapter 14 Question 32

32) Using the data given below estimate the value of the Gibbs energy change of reaction (kJ mol^-1) at 310 K, for the following reaction:

CH₃CH₂OH (l) + O₂ (g) → CH₃CO₂H (l) + H₂O (l)

a. - 450.2

Section reference: 14.5

b. - 451.8.

Section reference: 14.5

c. -41.7.

Section reference: 14.5

d. -533.8.

Section reference: 14.5

Type: multiple choice question

Title: Chapter 14 Question 33

33) Using the data given below estimate the value of the Gibbs energy change of reaction at 325 K, for the following reaction:

N₂ (g) + 2 O₂ (g) → 2 NO₂ (g)

a. + 26.1.

Section reference: 14.5

b. + 105.9.

Section reference: 14.5

c. + 102.6.

Section reference: 14.5

d. + 40.

Section reference: 14.5