What is the value of the equilibrium constant (Keq) when the following redox reaction takes place at 727°C? Mn (s) + Sn¹+ (aq) →Mn²+ (aq) + Sn²+ (aq) 2.55 x 10¹3 2.76 x 10¹8 7.62 x 1036 5.23 x 10-15 3.62 x 10-19 (A) (D) (C) (D) (三)
What is the value of the equilibrium constant (Keq) when the following redox reaction takes place at 727°C? Mn (s) + Sn¹+ (aq) →Mn²+ (aq) + Sn²+ (aq) 2.55 x 10¹3 2.76 x 10¹8 7.62 x 1036 5.23 x 10-15 3.62 x 10-19 (A) (D) (C) (D) (三)
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Chemistry Problem: Equilibrium Constant Calculation
---
#### Problem Statement:
**What is the value of the equilibrium constant \( K \) when the following redox reaction takes place at 727°C?**
\[
\text{Mn (s) + Sn}^{2+} \text{(aq) } \rightarrow \text{Mn}^{2+} \text{(aq) + Sn (s)}
\]
#### Choices:
- (A) \( 2.55 \times 10^{13} \)
- (B) \( 2.76 \times 10^{6} \)
- (C) \( 7.62 \times 10^{3} \)
- (D) \( 5.23 \times 10^{15} \)
- (E) \( 3.62 \times 10^{-19} \)
---
#### Helpful Hint:
The boxed section on the page provides a useful formula for this type of calculation:
**Equation Suggested:**
\[
E_{\text{cell}} = \frac{RT}{nF} \ln K
\]
This formula may be more convenient than what you might have on your note sheet.
Where:
- \( E_{\text{cell}} \) is the cell potential.
- \( R \) is the gas constant.
- \( T \) is the temperature in Kelvin.
- \( n \) is the number of moles of electrons transferred.
- \( F \) is the Faraday constant.
- \( K \) is the equilibrium constant.
---
### Explanation:
To use the suggested equation effectively, you will need to know the values for \( E_{\text{cell}} \), \( R \), \( T \), \( n \), and \( F \). Detailed steps are often provided in your classroom materials or textbooks, which will aid in solving for \( K \).
#### Notes:
- \( R \) (Universal Gas Constant) = 8.314 J/(mol·K)
- \( F \) (Faraday Constant) = 96485 C/mol
- \( T \) = Temperature in Kelvin
- To convert Celsius to Kelvin, add 273.15 to the Celsius temperature.
Given the temperature at 727°C, the conversion to Kelvin is:
\[
727 + 273.15 = 1000.15 \text{ K}
\]
---
For more detailed guidance on solving such problems,](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc94d9e95-0e25-4757-a170-f111f0abbe77%2F9db207b3-4c51-47e5-92a5-ba9ee19f6e8a%2Foopnn15_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemistry Problem: Equilibrium Constant Calculation
---
#### Problem Statement:
**What is the value of the equilibrium constant \( K \) when the following redox reaction takes place at 727°C?**
\[
\text{Mn (s) + Sn}^{2+} \text{(aq) } \rightarrow \text{Mn}^{2+} \text{(aq) + Sn (s)}
\]
#### Choices:
- (A) \( 2.55 \times 10^{13} \)
- (B) \( 2.76 \times 10^{6} \)
- (C) \( 7.62 \times 10^{3} \)
- (D) \( 5.23 \times 10^{15} \)
- (E) \( 3.62 \times 10^{-19} \)
---
#### Helpful Hint:
The boxed section on the page provides a useful formula for this type of calculation:
**Equation Suggested:**
\[
E_{\text{cell}} = \frac{RT}{nF} \ln K
\]
This formula may be more convenient than what you might have on your note sheet.
Where:
- \( E_{\text{cell}} \) is the cell potential.
- \( R \) is the gas constant.
- \( T \) is the temperature in Kelvin.
- \( n \) is the number of moles of electrons transferred.
- \( F \) is the Faraday constant.
- \( K \) is the equilibrium constant.
---
### Explanation:
To use the suggested equation effectively, you will need to know the values for \( E_{\text{cell}} \), \( R \), \( T \), \( n \), and \( F \). Detailed steps are often provided in your classroom materials or textbooks, which will aid in solving for \( K \).
#### Notes:
- \( R \) (Universal Gas Constant) = 8.314 J/(mol·K)
- \( F \) (Faraday Constant) = 96485 C/mol
- \( T \) = Temperature in Kelvin
- To convert Celsius to Kelvin, add 273.15 to the Celsius temperature.
Given the temperature at 727°C, the conversion to Kelvin is:
\[
727 + 273.15 = 1000.15 \text{ K}
\]
---
For more detailed guidance on solving such problems,
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