Question

Which represents the correct equilibrium constant expression for the reaction below?

Answer 1

Answer:

the answer is D

Explanation:3

ON EDG

Answer 2

Answer:

       $\large\boxed{\large\boxed{K_c=\dfrac{[Cu^{2+}]}{[Ag^+]^2}}}$

Explanation:

1. Chemical equilibrium equation:

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

2. Species

In an equilibrium constant expression you do not include the solid substances; only gases and dissolved substances.

The symbol $(s)$ means solid, thus Cu(s) and Ag(s) shall not appear in your equilibrium constant expression.

The symbol $(aq)$ means in aqueous solution, thus the both $Ag^+$ and $Cu^{2+}$ must appear in the equilibrium constant expression.

3. Equilibrium constant expression.

It is the quotient of the product of the concentrations of the species on the right hand side of the equilibrium equation, each raised to its corresponding coefficient, and the product of the concentrations of the species on the left hand side, each raised to its coresponding coefficient.

        $K_c=\dfrac{[Cu^{2+}]}{[Ag^+]^2}$