Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Calculating ΔG from ΔH and ΔS
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 18.0 °C and constant total pressure. Then, she measures the reaction enthalpy ΔH and reaction entropy ΔS of the first reaction, and the reaction enthalpy ΔH and reaction free energy ΔG of the second reaction. The results of her measurements are shown in the table.
Complete the table. That is, calculate ΔG for the first reaction and ΔS 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 and the system is at equilibrium.
### Table:
1. **First Reaction:**
- Reaction: \(6 \text{C}_3 (g) + 2 \text{Te}_3 (g) \rightarrow 4 \text{C}_8 (g) + 3 \text{O}_2 (g)\)
- ΔH = 50. kJ
- ΔS = 172 J/K
- ΔG = [input field]
**Which is spontaneous?**
- ○ the forward reaction
- ○ the reverse reaction
- ○ neither
2. **Second Reaction:**
- Reaction: \(2 \text{CO}_2 (g) + 4 \text{H}_2 (g) \rightarrow 2 \text{CH}_4 (g) + 3 \text{O}_2 (g)\)
- ΔH = [input field] kJ
- ΔS = [input field] J/K
- ΔG = 1353 kJ
**Which is spontaneous?**
- ○ the forward reaction
- ○ the reverse reaction
- ○ neither
### Instructions:
- Calculate ΔG and ΔS using the provided data.
- Determine the spontaneity of each reaction under the given conditions.
### Explanation and Check:
- Use the Gibbs free energy equation: \(ΔG = ΔH - TΔS\), where T is the temperature in Kelvin.
This educational content allows students to apply thermodynamic concepts to real-world reactions, enhancing their understanding](https://content.bartleby.com/qna-images/question/9be9a090-f726-46c3-84a4-96616934014f/c685d207-489f-4b93-aeea-30209f7c6440/gf1xl5i_processed.jpeg)
Transcribed Image Text:### Calculating ΔG from ΔH and ΔS
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 18.0 °C and constant total pressure. Then, she measures the reaction enthalpy ΔH and reaction entropy ΔS of the first reaction, and the reaction enthalpy ΔH and reaction free energy ΔG of the second reaction. The results of her measurements are shown in the table.
Complete the table. That is, calculate ΔG for the first reaction and ΔS 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 and the system is at equilibrium.
### Table:
1. **First Reaction:**
- Reaction: \(6 \text{C}_3 (g) + 2 \text{Te}_3 (g) \rightarrow 4 \text{C}_8 (g) + 3 \text{O}_2 (g)\)
- ΔH = 50. kJ
- ΔS = 172 J/K
- ΔG = [input field]
**Which is spontaneous?**
- ○ the forward reaction
- ○ the reverse reaction
- ○ neither
2. **Second Reaction:**
- Reaction: \(2 \text{CO}_2 (g) + 4 \text{H}_2 (g) \rightarrow 2 \text{CH}_4 (g) + 3 \text{O}_2 (g)\)
- ΔH = [input field] kJ
- ΔS = [input field] J/K
- ΔG = 1353 kJ
**Which is spontaneous?**
- ○ the forward reaction
- ○ the reverse reaction
- ○ neither
### Instructions:
- Calculate ΔG and ΔS using the provided data.
- Determine the spontaneity of each reaction under the given conditions.
### Explanation and Check:
- Use the Gibbs free energy equation: \(ΔG = ΔH - TΔS\), where T is the temperature in Kelvin.
This educational content allows students to apply thermodynamic concepts to real-world reactions, enhancing their understanding
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