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Find the FALSE statement about the voltaic cell based on the two reduction half- reactions shown below. The concentrations of the ions are [AI3+] = 0.01 M, [Mn2+]%3D 0.1 M. Al3+(aq) + 3e - Al(s) E°red = -1.66 V Mn2+(aq) + 2e¯ - Mn(s) E°red = -1.18 V %3D Al(s) is a stronger reducing agent than Mn(s) O The observed cell potential is 0.49V Using base 10, logQ = -1. O For the balanced equation, n = 6 and Q = [AI3+] / [Mn2*]. %3D The shorthand diagram for this cell is Al(s) | Al3+(aq) || Mn2*(aq) | Mn(s).

Find the FALSE statement about the voltaic cell based on the two reduction half- reactions shown below. The concentrations of the ions are [AI3+] = 0.01 M, [Mn2+]%3D 0.1 M. Al3+(aq) + 3e - Al(s) E°red = -1.66 V Mn2+(aq) + 2e¯ - Mn(s) E°red = -1.18 V %3D Al(s) is a stronger reducing agent than Mn(s) O The observed cell potential is 0.49V Using base 10, logQ = -1. O For the balanced equation, n = 6 and Q = [AI3+] / [Mn2*]. %3D The shorthand diagram for this cell is Al(s) | Al3+(aq) || Mn2*(aq) | Mn(s).

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 137CWP: Consider a galvanic cell based on the following half-reactions: a. What is the standard potential...
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Find the FALSE statement about the voltaic cell based on the two reduction half- reactions shown below. The concentrations of the ions are [Al3+] = 0.01 M, [Mn2+] = 0.1 M. %3D %3D Al3+(ag) + 3e Al(s) E°red = -1.66 V Mn2+(aq) + 2e¯ - Mn(s) E°red = -1.18 V Al(s) is a stronger reducing agent than Mn(s) The observed cell potential is 0.49V O Using base 10, logQ = -1. O For the balanced equation, n = 6 and Q = [A3+] / [Mn²*]. The shorthand diagram for this cell is Al(s) | Al3*(aq) || Mn2*(aq) | Mn(s).
Transcribed Image Text:Find the FALSE statement about the voltaic cell based on the two reduction half- reactions shown below. The concentrations of the ions are [Al3+] = 0.01 M, [Mn2+] = 0.1 M. %3D %3D Al3+(ag) + 3e Al(s) E°red = -1.66 V Mn2+(aq) + 2e¯ - Mn(s) E°red = -1.18 V Al(s) is a stronger reducing agent than Mn(s) The observed cell potential is 0.49V O Using base 10, logQ = -1. O For the balanced equation, n = 6 and Q = [A3+] / [Mn²*]. The shorthand diagram for this cell is Al(s) | Al3*(aq) || Mn2*(aq) | Mn(s).
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