A) Cu(s) + Fe2+(aq) ----> Cu2+(aq) + Fe(s)
Ecell = E0cell-0.0591/nlog[Cu2+/Fe2+]
E0cell = E0cathode - E0anode
= -0.440 - 0.339
= -0.779 v
Ecell = (-0.779)-(0.0591/2)log(0.1/0.0053)
= -0.817 v
DG = - nFEcell
= -2*96500*-0.817
= 157.68 kj
as DG = +ve, the process is non-spontaneous.
B) Sn2+ + 2 Fe3+ -----> Sn4+ + 2 Fe2+
Ecell = E0cell-0.0591/nlog
([Fe2+]^2[Sn4+]/[Fe3+]^2[Sn2+])
E0cell = 0.771 - 0.154
= 0.617 v
Ecell = 0.617-(0.0591/2)log((0.0012^2*0.15)/(0.12^2*0.0021))
= 0.68 v
DG = - nFEcell
= -2*96500*0.68
= -131.24 kj
as DG = -ve, the process is spontaneous.
For the spontaneous as written at 25°C. A) Cu(s) I Cu (0.10 M)IFe (0.0053 M) I...
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Answers and detailed explanations For the following electrochemical cell, calculate the potential and determine if the cell reaction is spontaneous as written at 25 °C. Cu(s)|Cu2+(0.15 M)||Fe2+(0.0020 M)|Fe(s) Ecuaticu = 0.339 V Efez-ffe = -0.440 V Ecell = Determine if the cell reaction is spontaneous as written. O spontaneous O not spontaneous
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