How does the pH of a solution affect the Ecell of a ox/redux reaction?

Question

I have a question on a problem, it starts out as "Can H(+)(aq) oxidize Sn(s)" I said yes and wrote the following equation

2H(+)(aq) + Sn(s) <---> Sn(2+) + H2

the next part says find the Ecell. Which i found to be .1364V because E(reduction H+) = 0v and E(oxidation Sn) = .1364V.

The next part asks to find the Ecell if the Ph is 5.39 and both the H2 and Sn(2+) concentrations are 1.5M. Would I use the Nernst equation to find this out?

Thanks

Answer 1

The concept of 1.5M hydrogen gas is rather odd, but, yes, you use the Nernst Equation. Don't forget to convert the pH to a molarity of H+ ions.