The driving force Δ G diminishes to zero on the way to equilibrium, just as in any other spontaneous process. Both Δ G and the cell potential 
are zero when the redox reaction comes to equilibrium. The Nernst equation for the redox process of the cell may be given as :
E = Eº – 
log10Q
The key to the relationship is the standard cell potential Eº, derived from the standard free energy change as :
Eº = 
At equilibrium, the Nernst equation is given as :
Eº = 
log10K
(i)On the basis of information available for the reaction 
Al + O2 ⎯→ 
Al2O3; Δ G = –827 kJ/mol of O2 the minimum emf required to carry out an electrolysis of Al2O3 is –
(Given : 1 F = 96500 C)
Cu2+(aq) + 2Ag(s) (Eºcell = 0.46V) will be – antilog 12.2 (v) Eº for the electrochemical cell, Zn(s) |Zn2+ (1 M) aq || Cu2+ (1 M) aq| Cu(s) is 1.10 volt at 25ºC. The equilibrium constant for the cell reaction: Zn(s) + Cu2+ (aq) 
Cu(s) + Zn2+(aq) will be – 1039
Text Solution
Verified by ExpertsB
(i)
Sol. 2.14 V
(ii)
Sol. E = 0
(iii)
Sol. straight line
(iv)
Sol. antilog 15.6
(v)
Sol. 1037
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