You are given the following half-reactions. AgCl(s) + e → Ag(s) + Cl(aq) = +0.22 V Ag+ (aq) + e → Ag(s) Construct a cell with the following cell reaction. AgCl(s) → Ag+ (aq) + Cl - (aq) (a) What is the standard cell potential? -.58 4.0 V (b) What is the value of AG° for the reaction? 4.0 56 kJ/mol = +0.80 V (c) What is the equilibrium constant as determined from the cell potential? (Please recall that often a significant figures appears to be lost when raising 10 to a power.) 4.0 1.6e-10 X (d) What is this equilibrium constant called? Kea Kb 0 Ksp O Ka X
You are given the following half-reactions. AgCl(s) + e → Ag(s) + Cl(aq) = +0.22 V Ag+ (aq) + e → Ag(s) Construct a cell with the following cell reaction. AgCl(s) → Ag+ (aq) + Cl - (aq) (a) What is the standard cell potential? -.58 4.0 V (b) What is the value of AG° for the reaction? 4.0 56 kJ/mol = +0.80 V (c) What is the equilibrium constant as determined from the cell potential? (Please recall that often a significant figures appears to be lost when raising 10 to a power.) 4.0 1.6e-10 X (d) What is this equilibrium constant called? Kea Kb 0 Ksp O Ka X
Chemistry
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Part C and D.
![You are given the following half-reactions:
\[ \text{AgCl(s) + e}^- \rightarrow \text{Ag(s) + Cl}^- \, (\text{aq}) \quad E^\circ = +0.22 \, \text{V} \]
\[ \text{Ag}^+ \, (\text{aq}) + e^- \rightarrow \text{Ag(s)} \quad E^\circ = +0.80 \, \text{V} \]
Construct a cell with the following cell reaction:
\[ \text{AgCl(s) } \rightarrow \text{Ag}^+ \, (\text{aq}) + \text{Cl}^- \, (\text{aq}) \]
(a) What is the standard cell potential?
- Answer: \(-0.58 \, \text{V}\) ✔️
(b) What is the value of \(\Delta G^\circ\) for the reaction?
- Answer: \(56 \, \text{kJ/mol}\) ✔️
(c) What is the equilibrium constant as determined from the cell potential?
(Note: Significant figures are often lost when raising 10 to a power.)
- Answer: \(1.6 \times 10^{-10}\) ❌
(d) What is this equilibrium constant called?
Choices:
- \(K_{\text{eq}}\)
- \(K_b\) (selected)
- \(K_{\text{sp}}\)
- \(K_a\) ❌](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F61ff295b-afd4-43c3-8ed2-2cc17b9c2249%2Fa20bc15a-dfa0-40fd-aee0-a719ababe895%2Feh39mc_processed.png&w=3840&q=75)
Transcribed Image Text:You are given the following half-reactions:
\[ \text{AgCl(s) + e}^- \rightarrow \text{Ag(s) + Cl}^- \, (\text{aq}) \quad E^\circ = +0.22 \, \text{V} \]
\[ \text{Ag}^+ \, (\text{aq}) + e^- \rightarrow \text{Ag(s)} \quad E^\circ = +0.80 \, \text{V} \]
Construct a cell with the following cell reaction:
\[ \text{AgCl(s) } \rightarrow \text{Ag}^+ \, (\text{aq}) + \text{Cl}^- \, (\text{aq}) \]
(a) What is the standard cell potential?
- Answer: \(-0.58 \, \text{V}\) ✔️
(b) What is the value of \(\Delta G^\circ\) for the reaction?
- Answer: \(56 \, \text{kJ/mol}\) ✔️
(c) What is the equilibrium constant as determined from the cell potential?
(Note: Significant figures are often lost when raising 10 to a power.)
- Answer: \(1.6 \times 10^{-10}\) ❌
(d) What is this equilibrium constant called?
Choices:
- \(K_{\text{eq}}\)
- \(K_b\) (selected)
- \(K_{\text{sp}}\)
- \(K_a\) ❌
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