When the Ag concentration is 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.078 V. What is the Mn²+ concentration? 2+ 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) Ag+ (aq) + e → Ag(s) = 0.799 V Mn2+ (aq) + 2e → Mn(s) [Mn²+] = M 1 Eº red EO red __ -1.180 V
When the Ag concentration is 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.078 V. What is the Mn²+ concentration? 2+ 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) Ag+ (aq) + e → Ag(s) = 0.799 V Mn2+ (aq) + 2e → Mn(s) [Mn²+] = M 1 Eº red EO red __ -1.180 V
Chemistry
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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
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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![When the Ag concentration is 1.49 M, the observed cell potential
at 298 K for an electrochemical cell with the following reaction is
2.078 V. What is the Mn2+ concentration?
2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq)
Ag+ (aq) + e → Ag(s)
= 0.799 V
Mn2+ (aq) + 2e → Mn(s)
[Mn²+] =
M
10000
Eº
red
Eº
red
-
-1.180 V
-](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5ac97eb4-3024-4277-9263-18bf0d8951d3%2F30df6ade-315c-4e6d-bebe-42ed2949c6ae%2Fzf8bg6o_processed.jpeg&w=3840&q=75)
Transcribed Image Text:When the Ag concentration is 1.49 M, the observed cell potential
at 298 K for an electrochemical cell with the following reaction is
2.078 V. What is the Mn2+ concentration?
2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq)
Ag+ (aq) + e → Ag(s)
= 0.799 V
Mn2+ (aq) + 2e → Mn(s)
[Mn²+] =
M
10000
Eº
red
Eº
red
-
-1.180 V
-
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