Question

PLEASE PLEASE HELP!!

Which of the following is the correct expression for the rate of the following reaction? Note: not all species are gaseous. CuO(s) + H2S (g) <--> Cu(s) + H2O (g)


A. [Cu] x [H2O] / ([CuO] x [H2S])

B. [H2O] / [H2S]

C. [CuO] x [H2S] / ([Cu] x [H2O])

D. None of these are correct

Answer 1

The following is the correct expression for the rate of the following reaction; CuO(s) + H2S (g) <--> Cu(s) + H2O (g): Products over reactants

The correct Answer, Letter Choice, (B), Keq =======> [H2O] / [H2S]

Hope that helps!!!! : )

Answer 2

Answer : The correct option is, (B) $\frac{[H_2O]}{[H_2S]}$

Explanation :

The given balanced chemical reaction is,

$CuO(s)+H_2S(g)\overset{k}\rightleftharpoons Cu(s)+H_2O(g)$

This reaction is a reversible reaction.

The rate of forward reaction will be,

$Rate=k_f[H_2S]$

The rate of backward reaction will be,

$Rate=k_b[H_2O]$

And at equilibrium the rate of reaction is equal to the rate of backward reaction divided by the rate of forward reaction.

$\frac{k_b}{k_f}=\frac{[H_2O]}{[H_2S]}$

or,

$K=\frac{[H_2O]}{[H_2S]}$

Hence, the correct expression for the equilibrium constant is, $K=\frac{[H_2O]}{[H_2S]}$