[ss4vegeta1]

Please someone help me figure this out.
I calculated the E°cell of these two equations:
Which is 0.54V
2ClO3- + 12H + 10e- --->Cl2 + 6H20
(S2O8)^2 + 2e- --> 2SO4^2-

I have to find change in Gibbs    DeltaG°=-nFE°cell

Can someone please help any steps or do I have to add these two and balance? How to do this please?

[ss4vegeta1]

Also the equations are the half lives. They also gave the E°cells of the two
E°cell ClO3- =1.47V
E°cell S208^2- =2.0V

[tamim83]

I removed your other post since it is the same question.  No Cross posting if you please. 

Anyway, which equation has the most pnegative (less positive) reduction potential?  Whicheverone you choose will need to be reversed and the reduction potential will change signs (now it is an oxidation reaction.  You then need to balance elctrons by multiplying the botom equation by 5.  That way when you add them, the elctrons cancel out.  This also gives you the appropiate "n" value for calculating the delta G.