The equilibrium constant for a reaction,A + B | vedclass

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(A) With an increase in temperature from $273 \ K$ to $298 \ K$,the value of the equilibrium constant $(K)$ decreases from $2$ to $1 	imes 10^{-2}$.A

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exothermic

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(A) With an increase in temperature from $273 \ K$ to $298 \ K$,the value of the equilibrium constant $(K)$ decreases from $2$ to $1 	imes 10^{-2}$.According to Le Chatelier's principle,for an exothermic reaction,the equilibrium constant decreases with an increase in temperature.Since the equilibrium constant decreases as the temperature increases,the forward reaction is exothermic.Thus,the process resulting in the formation of $C$ and $D$ is an exothermic reaction.

The equilibrium constant for a reaction,$A + B \rightleftharpoons C + D$ is $1 \times 10^{-2}$ at $298 \ K$ and is $2$ at $273 \ K$. The chemical process resulting in the formation of $C$ and $D$ is

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