Consider the reaction Ag*(aq) + Cl (aq) --> AgCI(s) Given the following table of thermodynamic data: Substance AH°; (kJ/mol) S° (J/mol K) Ag (aq) Cr(aq) AgCI(s) 105.90 73.93 -167.2 56.5 |-127.0 96.11 Determine the temperature (in °C) above which the reaction is nonspontaneous under standard conditions 1641 133.0 432.8 This reaction is spontaneous at all temperatures 150.5
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![**Consider the reaction**
\[ \text{Ag}^+(aq) + \text{Cl}^-(aq) \rightarrow \text{AgCl}(s) \]
**Given the following table of thermodynamic data:**
| Substance | \( \Delta H^\circ_f \) (kJ/mol) | \( S^\circ \) (J/mol K) |
|-----------|---------------------------------|-------------------------|
| \( \text{Ag}^+(aq) \) | 105.90 | 73.93 |
| \( \text{Cl}^-(aq) \) | -167.2 | 56.5 |
| \( \text{AgCl}(s) \) | -127.0 | 96.11 |
**Determine the temperature (in °C) above which the reaction is nonspontaneous under standard conditions:**
Options:
- 1641
- **133.0**
- 432.8
- This reaction is spontaneous at all temperatures
- 150.5
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The text describes a thermodynamic problem involving a chemical reaction between silver ions (\( \text{Ag}^+ \)) and chloride ions (\( \text{Cl}^- \)) to form silver chloride (\( \text{AgCl} \)). It provides a table of standard enthalpies of formation (\( \Delta H^\circ_f \)) and standard entropies (\( S^\circ \)) for each of the substances involved. The goal is to determine the temperature above which this reaction becomes nonspontaneous under standard conditions.
The correct answer from the given options is highlighted as 133.0°C.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F83e4d0e0-41e1-45c9-8283-0ae60fe430d6%2F85f28954-b1a5-4e05-937f-76e03de59a0a%2Fr3w78dh_processed.jpeg&w=3840&q=75)
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