Question

A reaction mixture contains 0.15 M CS2, 0.75 M H2, 0.55 M CH4, and 0.95 M H2S.
Is this reaction at equilibrium? If it is not at equilibrium, indicate the direction in which
it much shifts to reach equilibrium. Show work to support your answer. (Hint: Do not use

Answer 1

By the given first of all we calculate the equilibrium constant

CS₂(g) + 4 H₂(g) $\rightarrow$ CH₄(g) + 2 H₂S(g)

Equilibrium constant , $K=\frac{\left [ CH_{4} \right ]\left [ H_{2}S \right ]^{2}}{\left [ CS_{2} \right ]\left [ H_{2} \right ]^{4}}$

                               $K=\frac{\left0.55\left \times 0.95^{2}}{\left 0.15\times \left 0.75^{4}}$

                                K = 10.46

But given that K = 0.280 , the reaction is not at eqilibrium.

Since the value(10.46) obtained by our calculation is more than the actual K value ( 0.280) ,the equilibrium is shifted towards left side that is towards to the reactant side.