Worked out the first two steps to the problem just need help with the last where it's asking what the cell potential be with the changes to concentration Which would the cell potential be if you changed the concentrations to[Fe3*] = 0.60 [Hg²*) = 1.30 M[Hg22*] = 0.70 M[Fe2*] = 1.50 MWould the reaction become more spontaneous or less spontaneous under these newconcentrations?

The Nernst equation is shown below: Where: Ecell = cell potential E0cell = standard cell potential…

Answered: Which would the cell potential be if…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Worked out the first two steps to the problem just need help with the last where it's asking what the cell potential be with the changes to concentration

Which would the cell potential be if you changed the concentrations to
[Fe3*] = 0.60 [Hg²*) = 1.30 M
[Hg22*] = 0.70 M
[Fe2*] = 1.50 M
Would the reaction become more spontaneous or less spontaneous under these new
concentrations?

Expert Solution

Step 1

The Nernst equation is shown below:

Where:

Ecell = cell potential

E⁰cell = standard cell potential

R = gas constant

T = temperature

F = Faraday's constant

Q = reaction quotient

Step 2

Given information:

Concentration of Fe³⁺ = 0.60 M

Concentration of Hg²⁺ = 1.30 M

Concentration of Hg₂²⁺ = 0.70 M

Concentration of Fe²⁺ = 1.50 M

E⁰cell = 0.15 V

Step 3

The cell reaction is shown below:

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