Calculate the equilibrium constant for the reaction `Cu(s)+2Ag^(+)(aq)rarrCu^(2+)(aq)+2Ag(s), E_(cell)^(@)=0.46 V`.

Let us apply Nernst equation at equilibrium
`E_(cell)^(@)=(0.0591)/(n)log" "K_(C)`
`0.47=(0.0591)/(2)logK_(c)`
`K_(c)="antilog"[(0.47xx2)/(0.0591)]`
`=8.5xx10^(15)`.

Calculate the equilibrium constant for the reaction `Cu(s)+2Ag^(+)(aq)rarrCu^(2+)(aq)+2Ag(s), E_(cell)^(@)=0.46 V`.

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