The equilibrium constant of the reaction:
Cu(s)+2Ag+(aq)→Cu2+(aq)+2Ag(s);E∘=0.46V at 298K is :
4.0×1015
2.4×1010
2.0×1010
4.0×1010
ΔG∘=−n×F×e=−2×96500×0.46=−88780J
ΔG∘=2.303 RT log Kc
or−88780=−2.303×8.314×298 log Kc
or −88780=−5705.84logKc
⟹logKc=15.55⇒[Kc≈4×1015]
Calculate the equilibrium constant of the reaction.Cu(s)+2Ag+(aq)→Cu2+(aq)+2Ag(s), E⊖cell=0.46V