Using the Nernst equation to calculate the non-standard cell potential for the cell below when the anode contains 1.0 M

[answerhappygod]

Using the Nernst equation to calculate the non-standard
cell potential for the cell below when the anode contains 1.0 M
CuSO4 (aq) and the cathode contains 0.30 M
AgNO3 (aq) at 25 oC.
Cu (s) + 2
Ag+ (aq) ⟶ Cu2+ (aq) + 2
Ag (s)
CORRECT ME IF I'M WRONG AT ALL. I just want to give it a shot
and need some guidance to see how far I can go by myself.
I'm aware there are 2 Nernst equations to use, and I think we
would use the E = Ecell - (.05914V/n) log Q. I could be wrong, but
since it's under standard conditions, that's what I think it is. I
also do think we need to write out the half equations which would
be
Cu(s) ---> Cu^2+(aq) + 2e^- (oxidized)
2Ag^+(aq) + 2e^- ---> 2Ag (reduced)
so n = 2
Now I'm not sure what to do.