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In a 1.0 L aqueous solution when the rea...

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:

A

`[Cu^(2+)]=x/2M, [Ag^(o+)]=y/2 M`

B

`[Cu^(2+)] gt x/2 M, [Ag^(o+)] gt y/2 M`

C

`[Cu^(2+)] lt x/2 M, [Ag^(o+)] gt y/2 M`

D

`[Cu^(2+)] lt x/2 M, [Ag^(o+)] lt y/2 M`

Text Solution

Verified by Experts

Consoder the equation
`2Ag^(o+)(aq)+Cu(s) hArr Cu^(2+)(aq)+2Ag(s)`
equilibrium: `[Cu^(2+)]=x M, [Ag^(o+)]=y M`
`K_(eq)=K_(c )=([Cu^(2+)])/([Ag^(o+)]^(2))=x/y^(2)`
Now volume is doubled by adding water. As a result, the concentration of ions will become half and the direction of equilibrium, let us find the value of reaction coefficients, `Q`.
`Q=Q_(c )=([Cu^(2+)])/([Ag^(o+)]^(2))=(x//2)/((y//2)^(2))=(2x)/y^(2)`
`rArr Q gt K_(eq)`
This means that the system will move in backward direction in order to re-establish the equilibrium state.
`rArr [Ag^(o+)]_("At new eq") gt y/2` and `[Cu^(2+)]_("At new eq") lt x/2`
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