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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

AI Generated Solution

To solve the problem step by step, we will analyze the equilibrium reaction and how the concentrations change when the volume of the solution is doubled. ### Step 1: Write the equilibrium expression The given reaction is: \[ 2Ag^{+}(aq) + Cu(s) \rightleftharpoons Cu^{2+}(aq) + 2Ag(s) \] For this reaction, the equilibrium constant \( K_c \) can be expressed as: \[ K_c = \frac{[Cu^{2+}]}{[Ag^{+}]^2} \] ...
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