1. Tardigrade
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  3. Chemistry
  4. An equilibrium mixture of the reaction 2H2S(g) leftharpoons 2H2(g) + S2(g) had 0.5 mole H2S, 0.10 mole H2 and 0.4 mole S2 in one litre vessel. The value of equilibrium constant (K) in mole litre-1 is

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Q. An equilibrium mixture of the reaction
$2H_{2}S(g) \rightleftharpoons 2H_{2}(g) + S_{2}(g)$ had 0.5 mole $H_{2}S, 0.10$ mole $H_{2}$ and 0.4 mole $S_{2}$ in one litre vessel. The value of equilibrium constant (K) in mole $litre^{-1}$ is

Equilibrium

Solution:

$K =\frac{[H_{2}]^{2}[S_{2}]}{[H_{2}S]^{2}} =\frac{[0.10]^{2}[0.4]}{[0.5]^{2}}=0.016$