1. Tardigrade
  2. Question
  3. Chemistry
  4. An equilibrium mixture of the reaction 2 H 2 S ( s ) leftharpoons 2 H 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

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Q. An equilibrium mixture of the reaction $2 H _{2} S _{( s )} \rightleftharpoons 2 H _{2( g )}+ S _{2( g )}$, 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

AIIMSAIIMS 1998Equilibrium

Solution:

$2 H _{2} S (g) \rightleftharpoons 2 H _{2}(g)+ S _{2}(g)$

Equilibrium constant is,

$K=\frac{\left[ H _{2}\right]^{2}\left[ S _{2}\right]}{\left[ H _{2} S \right]^{2}}=\frac{[0.1]^{2}[0.4]}{[0.5]^{2}}$

$=0.016\, mol\, L ^{-1}$