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What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Ag+ concentration is 6.17 x 10-4 M and the Mn²+ concentration is 1.04 M? 2+ 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) V Ecell The cell reaction as written above is for the concentrations given.

What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Ag+ concentration is 6.17 x 10-4 M and the Mn²+ concentration is 1.04 M? 2+ 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) V Ecell The cell reaction as written above is for the concentrations given.

Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter20: Electrochemistry
Section20.1: Voltaic Cells
Problem 13SSC
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What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Ag+ concentration is 6.17 x 10-4 M and the Mn²+ concentration is 1.04 M ? Ecell 2+ 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) V The cell reaction as written above is Submit Answer Retry Entire Group spontaneous nonspontaneous for the concentrations given. y attempts remaining
Transcribed Image Text:What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Ag+ concentration is 6.17 x 10-4 M and the Mn²+ concentration is 1.04 M ? Ecell 2+ 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) V The cell reaction as written above is Submit Answer Retry Entire Group spontaneous nonspontaneous for the concentrations given. y attempts remaining
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