[FthkuMan]

Hi guys, I'll be quick

You have the following half-cells:   

Pt(s) | Fe2+ (0.1M), Fe3+ (0.2M)
Ag(s) | Ag+ (0.1M)

1. Write the voltage in each half cell.
2. Which is the cathode and which is the anode, and what is the reaction at each electrode?
3. Calculate the voltage of the cell.
4. At which concentration of Ag+ ions will the cell reach equilibrium? assume that Fe2+ and Fe3+ remain the same concentration.





Also, unrelated question-

       Eo = -0.04 volt           Fe3+(aq) + 3e- ->  Fe(s)
       Eo = -0.13 volt           Pb2+(aq) + 2e- ->  Pb(s)

In this case, we flip the Pb half cell, and it's being oxidized. But now the voltage is 0.13, so how is it the anode?

Thanks!

[Borek]

You have to show your attempts at solving the problem to receive help, this is a forum policy.

[FthkuMan]

EDIT: added it to the OP.

As for the second question, it's just a general question about something I don't really get, if you could just explain the theory behind it to me that'd be great.

Thank you.