The equilibrium constant at `278K` for `Cu(s)+2Ag^(o+)(aq) hArr Cu^(2+)(aq)+2Ag(s)` is `2.0xx10^(15)`. In a solution in which copper has displaced, some silver ions from the solution, the concentration of `Cu^(2+)` ions from the solution, the concentration of `Cu^(2+)` ions is `1.8xx10^(-2) mol L^(-1)` and the concentration of `Ag^(o+)` ions is `3.0xx10^(-9) mol L^(-1)`. Is the system at equilibrium?

Explanation

For the reaction , `Cu (s) +2Ag^(+)(aq) hArr Cu^(2) (aq) + 2Ag (s)`
The concentration quotient `Q_(c)` is :
`Q_(c) +([Cu^(2+) (aq)][Ag(s)]^(2))/([Cu(s)][Ag^(+) (aq)]^(2))= ([Cu^(2+) (aq)])/([Ag^(+) (aq)]^(2))`
`:. [Ag (s)] = [Cu(s)]=1mol L^(-1)]`
According to the available data,
`[Cu^(2+) (aq)]=1.8 xx 10^(-2) mol L^(-1) and [Ag^(+) (aq)] = 3.0 xx 10^(-9) mol L^(-1).`
`Q_(c) =((1.8xx 10^(-2)))/(3.0 xx 10^(-9))^(2)=2xx10^(15)`
Since the value of the concentration quotient is the same as that of hte equilibrium constant , the reaction is in a state of equilibrium.