Question 5. A voltaic cell is constructed using the following half-reactions:
Cathode: Pb2+ (aq) + 2 e- ---> Pb(s)
Anode: Pb(s) + 2 Cl-(aq) ----> PbCl2(s) + 2 e-
Global reaction: Pb2+ + 2 Cl- ---> PbCl2(s)
a. If a potential of 0.142 V is measured for this cell under standard conditions, what is the standard oxidation potential (Eoox) for the anode reaction?
I can't find the oxidation potential values in the text but I am assuming this is just E cell=Cathode-Anode?
Also, anywhere online I can find these values so I can actually do the questions?
Edit:
Pb2+ (aq) + 2 e- Pb(s) = -0.13
Anode = -(ECell-Cathode) = -0.272 v
b) Calculate dGo for the cell reaction.
For this question I am not sure if I am supposed to use E cell given in the question or calculate non-standard Ecell? Concentrations aren't given until c) but Go requires use of Eo