Please help For the following voltaic cell that is observed to proceed as writte
ID: 961340 • Letter: P
Question
Please help For the following voltaic cell that is observed to proceed as written under standard conditions, give the cell potential. Identify the anode and cathode, and calculate Delta G degree. Zn(s) + Fe^2+(aq) rightarrow Zn^2+(aq) + Fe(s) Zn^2+(aq) + 2e^- rightarrow Zn(s) E^degree = -0.76 V Fe^2+(aq) + 2e^- rightarrow Fe(s) E^degree = -0.44 V For the voltaic cell in which Pb is oxidized to Pb^2+ and Cu^2+ is reduced to Cu under standard conditions, the following cell potentials were observed at the given temperatures. calculate Delta G^0 for each E and T value. Graph Delta G^0(y axis) against temperature in kelvin. this gives DeltaS^0, which is the slope. using the gibbs free energy equation calculate DeltaH^0.Explanation / Answer
ANSWER
Dear candidate you have asked two different questions. As per guidelines one question one time. So here we solve the first question, please send other separately..
1. The electrode at which reduction takes place is called Cathode and the elecrode at which oxidation takes place is called Anode. Reduction takes place at Fe and oxidation takes place at Zn, hence Fe is cathode and Zn is anode.
Eocell = Eocathode - Eoanode
Eocell = (-0.44) -(-0.76) = 0.32 V
Go = -nFEocell
n = number of electrons involved in balanced equation = 2
F = faraday constant = 96500 C
Go = - 2 X 96500 X 0.32 = 61.76KJ