Hi, can anyone tell me what I'm doing wrong here?
"Calculate the equilibrium constant for the redox reaction that would take place in the following instance, and use that number to determine whether a reation would occur or not.
A piece of copper wire in a 1.0 M solution of Pb(NO3)2 (aq)"
Standard reduction potential for the half reactions is given:
Copper: 0.337 V
Lead: -0.126 V
So first I have to find the cell potential, using this formula:
E(cell)=E(red)-E(ox)
As I understand it, the half reation with the most positive reduction potential needs to be first, in this case copper:
E(cell)=0.337 V - (-0.126 V) = 0.463 V
But this is apparently wrong. The solution to the problem says I have to switch the two numbers, like this:
E(cell)=(-0.126 V) - 0.337 V = -0.463 V
Why is that?