Hi guys and girls!

I am absolutely clueless on how to start this. I have my final year exams for my degree Friday and this is a certain question to come up so anyone that can help I owe you!!

A metal is corroding in an oxygen free acid of pH = 1 at 298 K according to

the overall reaction M + 2H+ → M2+ + H2. From the data given below,

calculate the corrosion rate of the metal in A cm-2.

Data: the equilibrium potential E0 M2+/M = –0.76V and the solution contains

10–2 mol dm-3 M2+. The equilibrium exchange current density, i0 for the metal

is 10–3 A cm-2 and the transfer

coefficient α is 0.5. For the hydrogen evolution reaction, i0 = 10–8 A cm-2 and

E0 H+/H2 = 0.0V and α is 0.5.

I assume you have to use the Butler volmer equation somewhere but dont know how to start.

Any help would be appreciated,

Cliff