1. Tardigrade
  2. Question
  3. Chemistry
  4. The equilibrium constant for the reaction, H 2( g )+ I 2( g ) leftharpoons 2 HI ( g ) is 32 at a given temperature. The equilibrium concentrations of I 2 and HI are 0.5 × 10-3 and 8 × 10-3 M respectively. The equilibrium concentration of H 2 is

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Q. The equilibrium constant for the reaction,
$H _{2}( g )+ I _{2}( g ) \rightleftharpoons 2 HI ( g )$
is $32$ at a given temperature. The equilibrium concentrations of $I _{2}$ and $HI$ are $0.5 \times 10^{-3}$ and $8 \times 10^{-3} M$ respectively. The equilibrium concentration of $H _{2}$ is

Equilibrium

Solution:

$H _{2}+ I _{2} \rightleftharpoons 2 HI$

$K=\frac{[ HI ]^{2}}{\left[ H _{2}\right]\left[ I _{2}\right]}$

$\left[ H _{2}\right]=\frac{[ HI ]^{2}}{\left[I_{2}\right] \times K}=\frac{\left(8 \times 10^{-3}\right)^{2}}{\left(0.5 \times 10^{-3}\right)(32)}$

$=4 \times 10^{-3}\, M$