In a `1.0 L` aqueous solution when the reaction
`2Ag^(o+)(aq)+Cu(s) hArr Cu^(2+)(aq)+2Ag(s)`
reaches equilibrium, `[Cu^(2+)]=Cu(s) hArr Cu^(2+)(aq)+2Ag(s)`
reaches equilibrium, `[Cu^(2+)]=xM` and `[Ag^(o+)]=y M`.
If the volume of solution is doubled by adding water, then at equilibrium:

Options

A. `[Cu^(2+)] = x/2 M, [Ag^(+)] = Y/2 M`
B. `[Cu^(2+)] gt x/2 M, [Ag^(+)] gt Y/2 M`
C. `[Cu^(2+)] lt x/2 M, [Ag^(+)] gt Y/2 M`
D. `[Cu^(2+)] lt x/2 M, [Ag^(+)] lt Y/2 M`

Answer

C

Explanation

Consider the equation : `2Ag^(+)(aq) + Cu(s) rarr Cu^(2+)(aq) + 2Ag(s)`
At equilibrium : `[Cu^(2+)] = xM , [Ag^(+)] = yM`
`K_(eq) = K_(c) = [Cu^(2+)]/[Ag^(+)]^(2) = x/y^(2)`