Using $\Delta_{f} G_{298}^{\circ}$ data given below: $\begin{array}{|c|c|c|c|} \hline & \mathrm{CO}_{2}(\mathrm{~g}) & \mathrm{CH}_{4}(\mathrm{~g}) & \mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}(\mathrm{l}) \\ \hline \Delta_{\mathrm{f}} G_{298}^{\circ} / \mathrm{kJ} \mathrm{mol}^{-1} & -394.4 & -50.8 & -389.9 \\ \hline \end{array}$ calculate the standard Gibbs energy change, $\Delta _{T}G_{298}^{\circ}$ (kJ mol-1), for the following reaction: CO2 (g) + CH4 (g) → CH3CO2H (l)

A) - 835.1 B) - 55.3. C) + 835.1. D) + 55.3. A) - 835.1 B) - 55.3. C) + 835.1. D) + 55.3.

Using $\Delta_{\mathrm{f}} H_{298}^{\circ}$ and $S_{298}^{\circ}$ data given below: $\begin{array}{|l|l|l|l|l|} \hline & \mathrm{CH}_{4}(\mathrm{~g}) & \mathrm{O}_{2}(\mathrm{~g}) & \mathrm{CO}_{2}(\mathrm{~g}) & \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \\ \hline \Delta_{\mathrm{f}} H_{298}^{\circ} / \mathrm{kJ} \mathrm{mol}^{-1} & -74.8 & 0 & -393.5 & -285.8 \\ \hline S_{298}^{\circ} / \mathrm{J} \mathrm{K}^{-1} \mathrm{~mol}^{-1} & 186.3 & 205.1 & 213.7 & 69.9 \\ \hline \end{array}$ Calculate the standard Gibbs energy change, $\Delta_{r} G_{298}^{\circ}$ (kJ mol-1), for the following reaction: CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (l)

A) - 818. B) + 71.5. C) + 963. D) - 963. A) - 818. B) + 71.5. C) + 963. D) - 963.

The standard entropy change, $\triangle_{T} S_{298}^{∘}$ 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 $\triangle_{T} S^{∘}$ (in J K-1 mol-1) at 550 K.

A) - 226. B) - 171. C) + 226. D) + 171. A) - 226. B) - 171. C) + 226. D) + 171.

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) $\begin{array}{|c|c|c|c|c|} \hline & \begin{array}{c} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH} \\ (\mathrm{l}) \end{array} & \mathrm{O}_{2}(\mathrm{~g}) & \mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}(\mathrm{I}) & \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \\ \hline \Delta_{\mathrm{f}} H_{298}^{\circ} / \mathrm{kJ} \mathrm{mol}^{-1} & -277.6 & 0 & -484.5 & -285.8 \\ \hline S_{298}^{\circ} / \mathrm{JK}^{-1} \mathrm{~mol}^{-1} & 159.9 & 205.1 & 158.0 & 69.9 \\ \hline C_{p} / \mathrm{J} \mathrm{K}^{-1} \mathrm{~mol}^{-1} & 111.5 & 29.4 & 123.1 & 75.3 \\ \hline \end{array}$

A) - 450.2 B) - 451.8. C) -41.7. D) -533.8. A) - 450.2 B) - 451.8. C) -41.7. D) -533.8.

Using $\Delta_{\mathrm{f}} H_{298}^{\circ}$ and $S_{298}^{\circ}$ data given below: $\begin{array}{|l|l|l|l|} \hline & \mathrm{NH}_{3}(\mathrm{~g}) & \mathrm{N}_{2}(\mathrm{~g}) & \mathrm{H}_{2}(\mathrm{~g}) \\ \hline \Delta_{\mathrm{f}} H_{298}^{\circ} / \mathrm{kJ} \mathrm{mol}^{-1} & -46.1 & 0 & 0 \\ \hline S_{298}^{\circ} / \mathrm{J} \mathrm{K}^{-1} \mathrm{~mol}^{-1} & 192.5 & 191.6 & 130.7 \\ \hline \end{array}$ Calculate the standard Gibbs energy change, $\Delta_{r} G_{298}^{\circ}$ (kJ mol-1), for the following reaction: 2 NH3 (g) → N2 (g) + 3 H2 (g)

A) + 151. B) - 151. C) + 33. D) - 59. A) + 151. B) - 151. C) + 33. D) - 59.

Exam 14: Entropy and Gibbs Energy

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. -ΔG > 0

(Multiple Choice)

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Question 21

Calculate the entropy change ( $\triangle_{vap} S^{∘}$ , 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, $\triangle_{vap} H^{∘}$ for mercury is + 59.3 kJ mol^-1).

(Multiple Choice)

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Question 22

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. -ΔG = 0

(Multiple Choice)

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Question 23

The entropy change for the following reaction will be negative: C₁₁H₂₂O₁₁ (s) + 12 O₂ (g) → 12 CO₂ (g) + 11 H₂O (l)

(True/False)

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Question 24

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.

(Multiple Choice)

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Question 25

Using $\Delta_{f} G_{298}^{\circ}$ data given below: () () () / -394.4 -50.8 -389.9 calculate the standard Gibbs energy change, $\Delta _{T}G_{298}^{\circ}$ (kJ mol^-1), for the following reaction: CO₂ (g) + CH₄ (g) → CH₃CO₂H (l)

(Multiple Choice)

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Question 26

Using data in Appendix 7, (p. 1350), calculate the standard entropy change of reaction $\triangle_{T} S_{298}^{∘}$ ( in J K^-1 mol^-1) for the following reaction: CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O (l)

(Multiple Choice)

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Question 27

Using $\Delta_{\mathrm{f}} H_{298}^{\circ}$ and $S_{298}^{\circ}$ data given below: () () () () / -74.8 0 -393.5 -285.8 / 186.3 205.1 213.7 69.9 Calculate the standard Gibbs energy change, $\Delta_{r} G_{298}^{\circ}$ (kJ mol^-1), for the following reaction: CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O (l)

(Multiple Choice)

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Question 28

The standard entropy change, $\triangle_{T} S_{298}^{∘}$ 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.

(True/False)

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Question 29

Match the reaction description and whether it is spontaneous and under which conditions -ΔH > 0, ΔS > 0

(Multiple Choice)

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Question 30

The standard entropy change, $\triangle_{T} S_{298}^{∘}$ 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 $\triangle_{T} S^{∘}$ (in J K^-1 mol^-1) at 550 K.

(Multiple Choice)

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Question 31

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

(Short Answer)

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Question 32

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

(True/False)

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Question 33

Match the reaction description and whether it is spontaneous and under which conditions -ΔH < 0, ΔS < 0

(Multiple Choice)

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Question 34

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.

(True/False)

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Question 35

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) () () () () / -277.6 0 -484.5 -285.8 / 159.9 205.1 158.0 69.9 / 111.5 29.4 123.1 75.3

(Multiple Choice)

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Question 36

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.

(True/False)

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Question 37

Using $\Delta_{\mathrm{f}} H_{298}^{\circ}$ and $S_{298}^{\circ}$ data given below: () () () / -46.1 0 0 / 192.5 191.6 130.7 Calculate the standard Gibbs energy change, $\Delta_{r} G_{298}^{\circ}$ (kJ mol^-1), for the following reaction: 2 NH₃ (g) → N₂ (g) + 3 H₂ (g)

(Multiple Choice)

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Question 38

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.

(Multiple Choice)

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Question 39

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

(True/False)

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Question 40

Exam 14: Entropy and Gibbs Energy

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. -ΔG > 0

Calculate the entropy change ( △vapS∘\triangle_{vap} S^{∘}△vap​S∘ , J K-1 mol-1) when 1.00 mol of mercury at its boiling point (Tb = 356.55 °C) vaporizes (in the process the temperature does not change, △vapH∘\triangle_{vap} H^{∘}△vap​H∘ for mercury is + 59.3 kJ mol-1).

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. -ΔG = 0

The entropy change for the following reaction will be negative: C11H22O11 (s) + 12 O2 (g) → 12 CO2 (g) + 11 H2O (l)

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, Cp, of methanol is 81.6 J K-1 mol-1, assume that the molar heat capacity, Cp is constant over this temperature range.

Using ΔfG298∘\Delta_{f} G_{298}^{\circ}Δf​G298∘​ data given below: () () () / -394.4 -50.8 -389.9 calculate the standard Gibbs energy change, ΔTG298∘\Delta _{T}G_{298}^{\circ}ΔT​G298∘​ (kJ mol-1), for the following reaction: CO2 (g) + CH4 (g) → CH3CO2H (l)

Using data in Appendix 7, (p. 1350), calculate the standard entropy change of reaction △TS298∘\triangle_{T} S_{298}^{∘}△T​S298∘​ ( in J K-1 mol-1) for the following reaction: CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (l)

The standard entropy change, △TS298∘\triangle_{T} S_{298}^{∘}△T​S298∘​ 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.

Match the reaction description and whether it is spontaneous and under which conditions -ΔH > 0, ΔS > 0

The standard entropy change, △TS298∘\triangle_{T} S_{298}^{∘}△T​S298∘​ 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 △TS∘\triangle_{T} S^{∘}△T​S∘ (in J K-1 mol-1) at 550 K.

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

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

Match the reaction description and whether it is spontaneous and under which conditions -ΔH < 0, ΔS < 0

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.

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) () () () () / -277.6 0 -484.5 -285.8 / 159.9 205.1 158.0 69.9 / 111.5 29.4 123.1 75.3

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.

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, Cp, of ethanol is 111.5 J K-1 mol-1 and assume that Cp is constant over this temperature range.

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

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Calculate the entropy change ( $\triangle_{vap} S^{∘}$ , 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, $\triangle_{vap} H^{∘}$ for mercury is + 59.3 kJ mol^-1).

The entropy change for the following reaction will be negative: C₁₁H₂₂O₁₁ (s) + 12 O₂ (g) → 12 CO₂ (g) + 11 H₂O (l)

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.

Using $\Delta_{f} G_{298}^{\circ}$ data given below: () () () / -394.4 -50.8 -389.9 calculate the standard Gibbs energy change, $\Delta _{T}G_{298}^{\circ}$ (kJ mol^-1), for the following reaction: CO₂ (g) + CH₄ (g) → CH₃CO₂H (l)

Using data in Appendix 7, (p. 1350), calculate the standard entropy change of reaction $\triangle_{T} S_{298}^{∘}$ ( in J K^-1 mol^-1) for the following reaction: CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O (l)

The standard entropy change, $\triangle_{T} S_{298}^{∘}$ 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.

The standard entropy change, $\triangle_{T} S_{298}^{∘}$ 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 $\triangle_{T} S^{∘}$ (in J K^-1 mol^-1) at 550 K.

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.

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) () () () () / -277.6 0 -484.5 -285.8 / 159.9 205.1 158.0 69.9 / 111.5 29.4 123.1 75.3

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.

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.