The water-gas shift reaction plays an important role in the production of clean fuel from coal. Co(g) + H,O(g) = CO:(8) + H;(g) Use the following thermodynamic data to determine the equilibrium constant K, at 700K. Substance: Co(g) H,O(g) Co:(g) H;(g) AH", (kJ/mol): S'(I/mol-K): -110.5 -241.8 -393.5 197.7 188.8 213.7 130.7
The water-gas shift reaction plays an important role in the production of clean fuel from coal. Co(g) + H,O(g) = CO:(8) + H;(g) Use the following thermodynamic data to determine the equilibrium constant K, at 700K. Substance: Co(g) H,O(g) Co:(g) H;(g) AH", (kJ/mol): S'(I/mol-K): -110.5 -241.8 -393.5 197.7 188.8 213.7 130.7
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![**Topic: Water-Gas Shift Reaction**
The water-gas shift reaction is crucial in producing clean fuel from coal. The reaction can be represented as:
\[ \text{CO(g) + H}_2\text{O(g) } \rightleftharpoons \text{ CO}_2\text{(g) + H}_2\text{(g)} \]
To determine the equilibrium constant \( K_p \) at 700 K, use the following thermodynamic data:
| Substance | \( \Delta H^\circ \) (kJ/mol) | \( S^\circ \) (J/mol·K) |
|-----------|---------------------|-------------------|
| CO(g) | -110.5 | 197.7 |
| \( \text{H}_2\text{O(g)} \) | -241.8 | 188.8 |
| \( \text{CO}_2\text{(g)} \) | -393.5 | 213.7 |
| \( \text{H}_2\text{(g)} \) | 0 | 130.7 |
**Instructions:**
Utilize the provided thermodynamic values to calculate \( K_p \) using the relation between Gibbs free energy and the equilibrium constant. Apply the formula for calculating \( \Delta G^\circ \) for the reaction and then relate it to \( K_p \) using:
\[ \Delta G^\circ = \Delta H^\circ - T\Delta S^\circ \]
\[ \Delta G^\circ = -RT \ln K_p \]
where:
- \( R \) is the universal gas constant.
- \( T \) is the temperature in Kelvin.
Calculate both \( \Delta H^\circ \) and \( \Delta S^\circ \) for the reaction using the standard enthalpies and entropies provided, then proceed to find \( \Delta G^\circ \) and subsequently \( K_p \) at 700 K.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F01e5e66e-0e79-4c86-85a9-0b0202abd934%2F2b890981-61b0-41a2-a44e-a0b9faf54f36%2Fytitmqf_processed.png&w=3840&q=75)
Transcribed Image Text:**Topic: Water-Gas Shift Reaction**
The water-gas shift reaction is crucial in producing clean fuel from coal. The reaction can be represented as:
\[ \text{CO(g) + H}_2\text{O(g) } \rightleftharpoons \text{ CO}_2\text{(g) + H}_2\text{(g)} \]
To determine the equilibrium constant \( K_p \) at 700 K, use the following thermodynamic data:
| Substance | \( \Delta H^\circ \) (kJ/mol) | \( S^\circ \) (J/mol·K) |
|-----------|---------------------|-------------------|
| CO(g) | -110.5 | 197.7 |
| \( \text{H}_2\text{O(g)} \) | -241.8 | 188.8 |
| \( \text{CO}_2\text{(g)} \) | -393.5 | 213.7 |
| \( \text{H}_2\text{(g)} \) | 0 | 130.7 |
**Instructions:**
Utilize the provided thermodynamic values to calculate \( K_p \) using the relation between Gibbs free energy and the equilibrium constant. Apply the formula for calculating \( \Delta G^\circ \) for the reaction and then relate it to \( K_p \) using:
\[ \Delta G^\circ = \Delta H^\circ - T\Delta S^\circ \]
\[ \Delta G^\circ = -RT \ln K_p \]
where:
- \( R \) is the universal gas constant.
- \( T \) is the temperature in Kelvin.
Calculate both \( \Delta H^\circ \) and \( \Delta S^\circ \) for the reaction using the standard enthalpies and entropies provided, then proceed to find \( \Delta G^\circ \) and subsequently \( K_p \) at 700 K.
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