1. Tardigrade
  2. Question
  3. Chemistry
  4. The equilibrium constant K, for the reaction 2 textHI ( textg) leftharpoons ( textH)2 ( textg) + ( textI)2 ( textg) at room temperature is 2.85 and that at 698 K is 1.4 × 10-2. This implies that the forward reaction is

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Q. The equilibrium constant K, for the reaction
$2 \text{HI} \left(\text{g}\right) \rightleftharpoons \left(\text{H}\right)_{2} \left(\text{g}\right) + \left(\text{I}\right)_{2} \left(\text{g}\right)$ at room temperature is 2.85 and that at 698 K is 1.4 × 10-2. This implies that the forward reaction is

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Solution:

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.