Ncert Exercises & Solutions

The value of K_c for the reaction $2 HI (g) ⇌ H_{2} (g) + I_{2} (g)$ is $1 \times 10^{- 4}$ . At a given time, the composition of reaction mixture is $[HI] = 2 \times 10^{- 5} mol, [H_{2}] = 1 \times 10^{- 5} mol$ and $[I_{2}] = 1 \times 10^{- 5} mol$ . In which direction will the reaction proceed?

Given that,

[HI] = 2 \times 10^{- 5} mol

[H_{2}] = 1 \times 10^{- 5} mol

[I_{2}] = 1 \times 10^{- 5} mol

At a given time, the reaction quotient Q for the reaction will be given by the expression

Q = \frac{[H_{2}] [I_{2}]}{{[HI]}^{2}}

= \frac{1 \times 10^{- 5} \times 1 \times 10^{- 5}}{{(2 \times 10^{- 5})}^{2}} = \frac{1}{4}

= 0.25 = 2.5 \times 10^{- 1}

As the value of reaction quotient is greater than the value of K_c, i.e.,

1 \times 10^{- 4}

the reaction will proceed in the reverse reaction.

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