Calculate AG for the reaction 2 H₂S(g) + SO2(g) 3 Srhombic(s) + 2 H₂O(g) For the following conditions at 25°C: PH₂S=0.0004 atm Pso₂=0.0143 atm PH₂0=0.0162 atm AG = AG°f H₂S(g): = -34 kJ/mol SO2(g) = -300. kJ/mol H₂O(g) = -229 kJ/mol kJ Submit Answer 6 item attempts remaining Try Another Version
Calculate AG for the reaction 2 H₂S(g) + SO2(g) 3 Srhombic(s) + 2 H₂O(g) For the following conditions at 25°C: PH₂S=0.0004 atm Pso₂=0.0143 atm PH₂0=0.0162 atm AG = AG°f H₂S(g): = -34 kJ/mol SO2(g) = -300. kJ/mol H₂O(g) = -229 kJ/mol kJ Submit Answer 6 item attempts remaining Try Another Version
Chemistry
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Chapter1: Chemical Foundations
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![**Calculating ΔG for the Reaction**
**Reaction:**
\[ 2 \text{H}_2\text{S (g)} + \text{SO}_2\text{(g)} \rightleftharpoons 3 \text{S}_{\text{rhombic}}\text{(s)} + 2 \text{H}_2\text{O (g)} \]
**Conditions at 25°C:**
- \( P_{\text{H}_2\text{S}} = 0.0004 \text{ atm} \)
- \( P_{\text{SO}_2} = 0.0143 \text{ atm} \)
- \( P_{\text{H}_2\text{O}} = 0.0162 \text{ atm} \)
**Standard Gibbs Free Energy of Formation (ΔG⁰f):**
- \( \text{H}_2\text{S (g)} = -34 \text{ kJ/mol} \)
- \( \text{SO}_2\text{(g)} = -300 \text{ kJ/mol} \)
- \( \text{H}_2\text{O (g)} = -229 \text{ kJ/mol} \)
**Calculate:**
\[ \Delta G = \text{______} \text{ kJ} \]
---
**Instructions:**
Use the given conditions and the standard Gibbs Free Energy of formation to calculate the Gibbs Free Energy change (\( \Delta G \)) for the reaction.
**User Interface:**
- **Submit Answer**: Click to submit your calculated value.
- **Try Another Version**: Click to attempt a different version of the question.
You have 6 attempts remaining to calculate the correct value of \( \Delta G \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5ae2fa02-8eae-484a-b9a8-9a97ab671177%2Fa27f2cea-2bbb-4f19-aa35-b2e5a99f6095%2Ftox14yj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Calculating ΔG for the Reaction**
**Reaction:**
\[ 2 \text{H}_2\text{S (g)} + \text{SO}_2\text{(g)} \rightleftharpoons 3 \text{S}_{\text{rhombic}}\text{(s)} + 2 \text{H}_2\text{O (g)} \]
**Conditions at 25°C:**
- \( P_{\text{H}_2\text{S}} = 0.0004 \text{ atm} \)
- \( P_{\text{SO}_2} = 0.0143 \text{ atm} \)
- \( P_{\text{H}_2\text{O}} = 0.0162 \text{ atm} \)
**Standard Gibbs Free Energy of Formation (ΔG⁰f):**
- \( \text{H}_2\text{S (g)} = -34 \text{ kJ/mol} \)
- \( \text{SO}_2\text{(g)} = -300 \text{ kJ/mol} \)
- \( \text{H}_2\text{O (g)} = -229 \text{ kJ/mol} \)
**Calculate:**
\[ \Delta G = \text{______} \text{ kJ} \]
---
**Instructions:**
Use the given conditions and the standard Gibbs Free Energy of formation to calculate the Gibbs Free Energy change (\( \Delta G \)) for the reaction.
**User Interface:**
- **Submit Answer**: Click to submit your calculated value.
- **Try Another Version**: Click to attempt a different version of the question.
You have 6 attempts remaining to calculate the correct value of \( \Delta G \).
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