A galvanic cell operates through the reaction represented below.
3 Cu^2+ (aq) + 2 Cr (s) -> 3 Cu (s) + 2 Cr^3+ (aq)
a. What is the standard cell potential, E^o, for the reaction?
b. Find the free energy change, deltaG^o, that occurs for the reaction.
c. If the cell, initially under standard conditions, functions until [Cu^2+] becomes 0.65 M, find [Cr^3+].
d. Would the value of the cell potential, Ecell, under the conditions specified in part (c), be greater than or less than the value for E^o cell.

Calculate Eo cell = E ocathode + Eo anode
You can pick up values from the standard reduction table
delta G = -nFEoCell
n = 2 (electrons lost or gained )here
F = 96500C

Use Nernst equation
Ecell = Eo cell + (RT/nF)ln[Cr^3+]^2/[Cu2+]^3
R is 8.314 J/molK
n= 6 electrons
F = 96500C