Constants Constant Value Ecu 0.337V Eco -0.277V R 8.314J x mol^-1 x K^-1 F 96,48
ID: 783319 • Letter: C
Question
Constants
Constant Value
Ecu 0.337V
Eco -0.277V
R 8.314J x mol^-1 x K^-1
F 96,485 C/mol
T 298 K
Use the formula Ecell = RT/nF ln Keq for the following redox reaction that occurs in an electrochemical cell having to electrodes: a cathode and an anode. The two half-reactions that occur in the cell are:
Cu^2+(aq) +2e- ---> Cu(s) and Co(s) ---> Co^2+(aq) + 2e-
the net reaction is
Cu^2+(aq) + Co(s) ---> Cu(s) + Co^2+(aq)
Use the given standard reduction potentials in your calculation as appropriate
Keq= _______
Explanation / Answer
Ecell = Ered - Eox
in the above reaction Cu is reduced and Co is oxidised.
Ecell = 0.337 - (-0.277)
= 0.614 V
Ecell = RT/nF ln Keq
ln Keq = [nF(Ecell)] / RT
Keq = e^(Eo nF / RT) = e^(0.614 x 2 x 96,500 / 8.314*298K)
Keq = e^47.83 = 5.92*10^20