Question

An equilibrium mixture for the reaction $2H_{2}S\left(g\right)\rightleftharpoons 2H_2\left(g\right)+S_2\left(g\right)$ has $1mole$ of $H_{2}S,0.2mole$ of $H_2$ and $0.8mole$ of $S_2$ in a $2$ litre flask. The value of $K_c$ in mol $L^{-1}$ is

• A. $0.004$
• B. $0.08$
• C. $0.016$
• D. $0.160$

Answer 1

Answer: (C)

$0.016$

${2H}_{2}S\left(g\right)\rightleftharpoons {2H}_2\left(g\right)+S_2\left(g\right)$

At $1mol$ $0.2$ $0.8$

eqb

conc $1/2$ $0.2/2$ $0.8/2$

$=0.1$ $=0.4$

$K_C=\frac{{\left(0.1\right)}^2\times \left(0.4\right)}{{\left(0.5\right)}^2}\Rightarrow 4\times 0.4\times {10}^{-2}\Rightarrow 0.016$