Equilibrium constant K, for the reaction, $2HI(g) ightleftharpoons H_{2}(g) + I_{2}(g)$ at room temperature is 2.85 and that at 698 K is $1.4 imes 10^{- 2}$. This implies that the forward reaction is

Question

Equilibrium constant K, for the reaction, $2HI(g) ightleftharpoons H_{2}(g) + I_{2}(g)$ at room temperature is 2.85 and that at 698 K is $1.4 	imes 10^{- 2}$. This implies that the forward reaction is

Dr. Abubacker · Accepted Answer

(a)
$2HI(g) ightleftharpoons H_{2}(g) + I_{2}(g)$
$K = \frac{\left\lbrack H_{2} ightbrack\lbrack I_{2}brack}{\lbrack HIbrack^{2}}$
When temperature increases, $K_{c}$ decreases.
$	herefore$ Concentration of product decreases.
It means forward reaction is not favoured at higher temperature. This is true for exothermic reactions. So, the forward reaction is exothermic.

Q. Equilibrium constant K, for the reaction, $2HI(g) \rightleftharpoons H_{2}(g) + I_{2}(g)$ at room temperature is 2.85 and that at 698 K is $1.4 \times 10^{- 2}$. This implies that the forward reaction is

Explanation

Reviewed by Dr. Abubacker

Want more practice?