In a standard electrochemical cell, A4+ constant is 2.23x1054 (Use R = 8.314 J/mol-K; F = 96485 C/mol) is reduced to solid A, while gaseous Z2 is oxidized to 23-. Calculate the standard cell potential (in V) if its equilibrium

Chemistry: Principles and Practice
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Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
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Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.48QE: The standard potential of the cell reaction Ag+(aq)+Eu2+(aq)Ag(s)+Eu3+(aq) is E = +1.23 V. Use the...
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In a standard electrochemical cell, A4+ is reduced to solid A, while gaseous Z2 is oxidized to Z3-. Calculate the standard cell potential (in V) if its equilibrium
constant is 2.23x1054
(Use R = 8.314 J/mol-K; F = 96485 C/mol)
Express your answer with 3 decimal places and do not encode the units. If negative, include the sign in your encoded answer.
Transcribed Image Text:In a standard electrochemical cell, A4+ is reduced to solid A, while gaseous Z2 is oxidized to Z3-. Calculate the standard cell potential (in V) if its equilibrium constant is 2.23x1054 (Use R = 8.314 J/mol-K; F = 96485 C/mol) Express your answer with 3 decimal places and do not encode the units. If negative, include the sign in your encoded answer.
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