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

Question

The equilibrium constant K, for the reaction 2 HI g ⇌ H 2 g + I 2 g at room temperature is 2.85 and that at 698 K is 1.4 × 10 -2 . This implies that the forward reaction is

TestHub · Accepted Answer

On increasing temperature, equilibrium constant is decreasing. It means that backward reaction is favoured. According to Le-Chatelier's principle, increase in temperature favours endothermic reaction. Thus backward reaction is endothermic, consequently forward reaction should be exothermic.

Chemistry - Ionic Equilibrium Question with Solution | TestHub

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