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Question: An equilibrium mixture of the reaction\(2 \mathrm { H } _ { 2 } \mathrm {~S} ( \mathrm {~g} )\)⇌<img...

An equilibrium mixture of the reaction2H2 S( g)2 \mathrm { H } _ { 2 } \mathrm {~S} ( \mathrm {~g} )⇌ had 0.5mole, 0.10 mole and 0.4 mole S2S _ { 2 } in one litre vessel. The value of equilibrium constant (K)( K ) in mole litre-1 is.

A

0.004

B

0.008

C

0.016

D

0.160

Answer

0.016

Explanation

Solution

K=[H2]2[ S2][H2 S]2=[0.10]2[0.4][0.5]2=0.016\mathrm { K } = \frac { \left[ \mathrm { H } _ { 2 } \right] ^ { 2 } \left[ \mathrm {~S} _ { 2 } \right] } { \left[ \mathrm { H } _ { 2 } \mathrm {~S} \right] ^ { 2 } } = \frac { [ 0.10 ] ^ { 2 } [ 0.4 ] } { [ 0.5 ] ^ { 2 } } = 0.016