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Electrolysis problem to find the half cell potential of a reaction

Submitted by toni31439 on Wed, 02/04/2009 - 09:48

Two students set up a simple cell at room temperature and pressure with zinc as the anode and
nickel as the cathode. The relevant standard reduction potentials are:
Zn2+(aq) + 2e- ? Zn(s) ; Eo = - 0.76V
Ni2+(aq) + 2e- ? Ni(s) ; Eo = - 0.25V
If the concentration of the solution in the nickel half-cell is increased to 2.0 mol L-1 with respect to
Ni2+ ions and the concentration of the solution in the zinc half-cell is kept at
1.0 mol L-1 with respect to Zn2+ ions, then the overall cell potential will be:
A. more positive than + 0.51 V B. equal to + 0.51 V C. between + 0.51 V and - 0.51 V
D. equal to - 0.51 V E. more negative than - 0.51 V

Actually i have no idea how to solve this , could you give a hand?/, please explain :)

Try doing a search on the Nernst Equation.