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A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu(aq) + e MnO4(aq) + 2 H₂O(1)+3e + Cu (aq) MnO₂(s) + 4 OH (aq) standard reduction potential = +0.153 V red Ered = +0.59 V

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu(aq) + e MnO4(aq) + 2 H₂O(1)+3e + Cu (aq) MnO₂(s) + 4 OH (aq) standard reduction potential = +0.153 V red Ered = +0.59 V

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.4: Standard Electrochemical Potentials
Problem 1RC
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A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu²+ (aq) + e MnO4(aq) + 2 H₂O(1)+3e Cu (aq) → MnO₂(s)+4 OH (aq) standard reduction potential Eº red = 'red = +0.153 V +0.59 V
Transcribed Image Text:A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu²+ (aq) + e MnO4(aq) + 2 H₂O(1)+3e Cu (aq) → MnO₂(s)+4 OH (aq) standard reduction potential Eº red = 'red = +0.153 V +0.59 V
Write a balanced equation for the half-reaction that 0 happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. 0
Transcribed Image Text:Write a balanced equation for the half-reaction that 0 happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. 0
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