[schan1]

a chem question...

A galvanic cell is constructed with a silver-silver chloride electrode, and a nickel strip immersed in a beaker containing 1.45x 10-2 M solution of NiCl2. Determine the balanced cell reaction and calculate the potential of the cell. Enter in volts. (assume a temperature of 25oC)

I know I need to use the nernst equation
E = E0cell - 0.592/n log (Q)
But i don't understand how I can get Q. Do I need the concentration of silver in order to calculate Q?
The balanced equation is:
2Ag+ (aq) + Ni (s) ---> Ni2+ (aq) + 2 Ag (s)
so i think Q = [Ni2+]/[Ag+]^2 

[Borek]

Ag/AgCl cell potential depends on Cl^- concentration, not Ag⁺.

[schan1]

I know how to solve it now. 
I used Ksp for AgCl to solve for the concentration of Ag+, then plug in everything in the Enernst equation, and I got the right answer. So, you have another appoach to this problem?