Question

Which represents the correct equilibrium constant expression for the reaction below? Cu(s)+2Ag+(aq)<->Cu2+(aq)+2Ag(s)

Answer 1

K(eq) = concentration of products/concentration of reactant         = [Cu+2] / [Ag+]^2 
Activity of pure solid and liquid is taken as 1.
Hence last option is correct.
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Answer 2

Answer : The correct option is, $k_{eq}=\frac{[Cu^{2+}]}{[Ag^+]^2}$

Explanation :

The given balanced chemical reaction is,

$Cu(s)+2Ag^+(aq)\rightleftharpoons Cu^{2+}(aq)+2Ag(s)$

The equilibrium expression for the reaction is determined by multiplying the concentrations of products and divided by the concentrations of the reactants and each concentration is raised to the power that is equal to the coefficient in the balanced reaction.

So, the equilibrium constant expression will be,

$k_{eq}=\frac{[Cu^{2+}]}{[Ag^+]^2}$

As we know that the concentrations of pure solids are constant that is they do not change. Thus, they are not included in the equilibrium expression.

Hence, the correct expression for the equilibrium constant is, $k_{eq}=\frac{[Cu^{2+}]}{[Ag^+]^2}$