The 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, it is $1.4 imes 10^{- 2}$. This implies that

Question

The 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, it is $1.4 	imes 10^{- 2}$. This implies that

Dr. Abubacker · Accepted Answer

(d)
Decrease of $K$ with rise of temperature means that the forward reaction is exothermic. As the given reaction is exothermic, energy of HI is greater or stability is less than $H_{2}$and $I_{2}$

Q. The 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, it is $1.4 \times 10^{- 2}$. This implies that

Explanation

Reviewed by Dr. Abubacker

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