You are given the following half-reactions. AgCl(s) + e → Ag(s) + Cl - (aq) صلح = +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? 4.0 -.58 = +0.80 V (b) What is the value of AG for the reaction? 4.0 56 kJ/mol (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 1.59e-10 x
You are given the following half-reactions. AgCl(s) + e → Ag(s) + Cl - (aq) صلح = +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? 4.0 -.58 = +0.80 V (b) What is the value of AG for the reaction? 4.0 56 kJ/mol (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 1.59e-10 x
General Chemistry - Standalone book (MindTap Course List)
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.127QP
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Question
![You are given the following half-reactions.
AgCl(s) + e → Ag(s) + Cl - (aq)
&
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
= +0.22 V
= +0.80 V
(b) What is the value of AGº for the reaction?
4.0 56
kJ/mol
(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
1.59e-10
X](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F61ff295b-afd4-43c3-8ed2-2cc17b9c2249%2F46842732-a701-4ff4-81bb-f7b5121834ee%2Fbb4zlx5_processed.png&w=3840&q=75)
Transcribed Image Text:You are given the following half-reactions.
AgCl(s) + e → Ag(s) + Cl - (aq)
&
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
= +0.22 V
= +0.80 V
(b) What is the value of AGº for the reaction?
4.0 56
kJ/mol
(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
1.59e-10
X
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