Solveeit Logo
Login

Question

Chemistry Question on Equilibrium

An equilibrium mixture of the reaction 2H2S(s)⇌2H2(g)+S2(g)2 H _{2} S _{( s )} \rightleftharpoons 2 H _{2( g )}+ S _{2( g )}, had 0.5 mole H2S0.5\, mole\, H _{2} S 0.100.10 mole H2H _{2} and 0.40.4 mole S2S _{2} in one litre vessel. The value of equilibrium constant (K)( K ) in mole litre −1^{-1} is

A

0.016

B

0.008

C

0.004

D

0.16

Answer

0.016

Explanation

Solution

2H2S(g)⇌2H2(g)+S2(g)2 H _{2} S (g) \rightleftharpoons 2 H _{2}(g)+ S _{2}(g) Equilibrium constant is, K=[H2]2[S2][H2S]2=[0.1]2[0.4][0.5]2K=\frac{\left[ H _{2}\right]^{2}\left[ S _{2}\right]}{\left[ H _{2} S \right]^{2}}=\frac{[0.1]^{2}[0.4]}{[0.5]^{2}} =0.016 mol L−1=0.016\, mol\, L ^{-1}