calculate the Ecell value at 298k based on the reaction Fe3+ and cr2+ 

Calculate the Ecell value at 298K for the cell based on the reaction

Fe³⁺(aq)+ Cr²⁺(aq) --> Fe²⁺(aq)+Cr³⁺(aq)

when [Fe³⁺] = [Cr²⁺] = 1.50x10^-3 M and [Fe²⁺]= [Cr³⁺] = 2.5x10^-4 M?

GIven that : HalfReactions Ered(V)

Cu2+(aq) + 2e- ------>Cu(s) +0.337

Pb2+(aq) + 2e- ------>Pb(s) -0.125

a) Calculate E cell for the reaction: Cu2+ (aq) + Pb (s)<----------> Cu (s) + Pb2+ (aq)

b) Calculate Delta G for the reaction (F = 9.65 x10^4 J/Vmol)

c) Determine the Keq value for the reaction

d)Using the Nernst equation, calculate the Ecell when [Pb2+] = 1.0 x10^-2 M and [Cu2+] =1.0 M