A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 100.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2Al(s) + 3H₂O(g) → Al₂O3(s) + 3H₂(g) 2CO₂(g) + 4H₂O(g) 2CH₂OH(g) + 30₂ (8) AH-951. kJ AS-2549. AG = KJ Which is spontaneous? O this reaction. O the reverse reaction Oneither AH 1353. kJ J =OK AS= J K AG-30. kJ Which is spontaneous? Othis reaction O the reverse reaction O neither 2
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 100.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2Al(s) + 3H₂O(g) → Al₂O3(s) + 3H₂(g) 2CO₂(g) + 4H₂O(g) 2CH₂OH(g) + 30₂ (8) AH-951. kJ AS-2549. AG = KJ Which is spontaneous? O this reaction. O the reverse reaction Oneither AH 1353. kJ J =OK AS= J K AG-30. kJ Which is spontaneous? Othis reaction O the reverse reaction O neither 2
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![A chemical engineer is studying the two reactions shown in the table below.
In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 100.0 °C and constant total pressure. Then, she measures the reaction enthalpy \( \Delta H \) and reaction entropy \( \Delta S \) of the first reaction, and the reaction enthalpy \( \Delta H \) and reaction free energy \( \Delta G \) of the second reaction. The results of her measurements are shown in the table.
Complete the table. That is, calculate \( \Delta G \) for the first reaction and \( \Delta S \) for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
### Table
#### Reaction 1:
\[ 2\text{Al}(s) + 3\text{H}_2\text{O}(g) \rightarrow \text{Al}_2\text{O}_3(s) + 3\text{H}_2(g) \]
- \( \Delta H = -951. \, \text{kJ} \)
- \( \Delta S = -2549. \, \text{J/K} \)
- \( \Delta G = \, \, \, \, \, \text{kJ} \)
**Which is spontaneous?**
- ( ) this reaction
- ( ) the reverse reaction
- ( ) neither
#### Reaction 2:
\[ 2\text{CO}_2(g) + 4\text{H}_2\text{O}(g) \rightarrow 2\text{CH}_3\text{OH}(g) + 3\text{O}_2(g) \]
- \( \Delta H = 1533. \, \text{kJ} \)
- \( \Delta S = \, \, \, \, \, \text{J/K} \)
- \( \Delta G = -30. \, \text{kJ} \)
**Which is spontaneous?**
- ( ) this reaction
- ( ) the reverse reaction
- ( ) neither](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcf266520-407e-4b51-839c-e1d92d759be6%2Fe513fe9c-5cdc-44d5-b4c7-d04904528587%2Fr20k8x8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A chemical engineer is studying the two reactions shown in the table below.
In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 100.0 °C and constant total pressure. Then, she measures the reaction enthalpy \( \Delta H \) and reaction entropy \( \Delta S \) of the first reaction, and the reaction enthalpy \( \Delta H \) and reaction free energy \( \Delta G \) of the second reaction. The results of her measurements are shown in the table.
Complete the table. That is, calculate \( \Delta G \) for the first reaction and \( \Delta S \) for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
### Table
#### Reaction 1:
\[ 2\text{Al}(s) + 3\text{H}_2\text{O}(g) \rightarrow \text{Al}_2\text{O}_3(s) + 3\text{H}_2(g) \]
- \( \Delta H = -951. \, \text{kJ} \)
- \( \Delta S = -2549. \, \text{J/K} \)
- \( \Delta G = \, \, \, \, \, \text{kJ} \)
**Which is spontaneous?**
- ( ) this reaction
- ( ) the reverse reaction
- ( ) neither
#### Reaction 2:
\[ 2\text{CO}_2(g) + 4\text{H}_2\text{O}(g) \rightarrow 2\text{CH}_3\text{OH}(g) + 3\text{O}_2(g) \]
- \( \Delta H = 1533. \, \text{kJ} \)
- \( \Delta S = \, \, \, \, \, \text{J/K} \)
- \( \Delta G = -30. \, \text{kJ} \)
**Which is spontaneous?**
- ( ) this reaction
- ( ) the reverse reaction
- ( ) neither
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