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You are shown a voltaic cell in which the cathode is Cu and the anode is an unknown metal, X. You measure E°(cell) to be 0.60 V. The cell reaction is X(s) + Cu2+(aq) → X²+(aq) + Cu(s) The standard reduction potential for the half-cell Cu2+(aq)/Cu(s) is +0.34 V. Salts of both metals are in their standard states of 1.00 M concentration. Calculate the standard reduction potential of the metal X.

You are shown a voltaic cell in which the cathode is Cu and the anode is an unknown metal, X. You measure E°(cell) to be 0.60 V. The cell reaction is X(s) + Cu2+(aq) → X²+(aq) + Cu(s) The standard reduction potential for the half-cell Cu2+(aq)/Cu(s) is +0.34 V. Salts of both metals are in their standard states of 1.00 M concentration. Calculate the standard reduction potential of the metal X.

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.49QE: A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt...
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You are shown a voltaic cell in which the cathode is Cu and the anode is an unknown metal, X. You measure E°(cell) to be 0.60 V. The cell reaction is X(s) + Cu2+(aq) → X²+(aq) + Cu(s) The standard reduction potential for the half-cell Cu2+(aq)/Cu(s) is +0.34 V. Salts of both metals are in their standard states of 1.00 M concentration. Calculate the standard reduction potential of the metal X.
Transcribed Image Text:You are shown a voltaic cell in which the cathode is Cu and the anode is an unknown metal, X. You measure E°(cell) to be 0.60 V. The cell reaction is X(s) + Cu2+(aq) → X²+(aq) + Cu(s) The standard reduction potential for the half-cell Cu2+(aq)/Cu(s) is +0.34 V. Salts of both metals are in their standard states of 1.00 M concentration. Calculate the standard reduction potential of the metal X.
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