Question

What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 7.98 x 10^-4 M and the Cr3+ concentration is 1.26 M? 3Hg2+(aq) + 2Cr(s) -> 3Hg(l) + 2Cr3+(aq) Hg2+(aq) + 2e- -> Hg(l) | Eored = 0.855 V Cr3+(aq) + 3e- -> Cr(s) | Eored = -0.740 V Ecell = [ ] V The cell reaction as written above is spontaneous for the concentrations given: true false

          What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 7.98 x 10^-4 M and the Cr3+ concentration is 1.26 M?

3Hg2+(aq) + 2Cr(s) -> 3Hg(l) + 2Cr3+(aq)

Hg2+(aq) + 2e- -> Hg(l) | Eored = 0.855 V
Cr3+(aq) + 3e- -> Cr(s) | Eored = -0.740 V

Ecell = [ ] V

The cell reaction as written above is spontaneous for the concentrations given:
true
false

What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 7.98 x 10^-4 M and the Cr3+ concentration is 1.26 M?

3Hg2+(aq) + 2Cr(s) -> 3Hg(l) + 2Cr3+(aq)

Hg2+(aq) + 2e- -> Hg(l) | Eored = 0.855 V
Cr3+(aq) + 3e- -> Cr(s) | Eored = -0.740 V

Ecell = [ ] V

The cell reaction as written above is spontaneous for the concentrations given:
true
false

Added by Dee W.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Tianyu Li

12/10/2022

Step 1

Step 1: Identify the half-reactions for the given reaction: The half-reactions for the reaction are: Show more…

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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 Hg2+ concentration is 7.98 x 10^-4 M and the Cr3+ concentration is 1.26 M?