Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Boxxxed on April 20, 2011, 02:13:44 PM
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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
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:delta: G° and E° are independent of concentration.
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Ok. I was mixing up the E and Eo.
How would I find the ksp value of PbCl2?
Ink=nEocell/0.0257?
Ink=(2)(-0.272)/0.0257 = 21.167
K = 1559007402
ksp = 1/k = 6.4x10-10
This isn't right. How do I find it?
Edit: I just subbed in a wrong value.
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d. If both half-cells in the reaction initially contain 0.1 M Pb2+ (aq) and 0.1 M Cl-(aq), respectively, what potential would be measured for the cell?
ECell = 0.142 - (0.0257/2) x In(1/0.13)
Are the substituted numbers correct? Namely the Q values?
http://img859.imageshack.us/i/pbcl2.jpg
Above is a chart summarizing some concepts. I've marked my answers but I'm not sure if they are correct as I don't fully understand this yet. Please take a look