In an-aqueous solution of volume 500 ml , when the reaction of `2Ag^(+)+Cu hArr Cu^(2+)+2Ag` reached equilibrium , the `[Cu^(2+)]` was x M. when 500 ml of water if further a added at the equilibrium `[Cu^(2+)]` will be

In an aqueous solution of volume 500 ml when the reaction 2Ag^(+)(aq)+Cu(s) hArr Cu^(2+)(aq)+2Ag(s) reached equilibrium, the [Cu^(2+)] was 'a'M . If 500 ml water is further added, at the equilibrium [Cu^(2+)] will be :

In an aqueous solution of volume 500 ml when the reaction 2Ag^(+)(aq)+Cu(s) hArr Cu^(2+)(aq)+2Ag(s) reached equilibrium, the [Cu^(2+)] was 'a'M . If 500 ml water is further added, at the equilibrium [Cu^(2+)] will be :

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:

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:

In an aqueous solution of voume 1000 ml, the following reation reached at equilibrium 2Ag^(+) (aq) +Cu (s) hArr Cu^(2+) (aq)+2Ag (s) The concentration of Cu^(+2) is 0.4 M at equilibrium, 3000 ml of water now added then concentration of Cu^(-2) at new equilibrium is