The equilibrium constant for a reaction $A + B ⇋ C + D$ 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:

exothermic

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endothermic

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unpredictable

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there is no relationship between

△ H

and K

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Solution

The correct option is A exothermic
With increase in temperature, the value of the equilibrium constant decreases. Which means as the temperature increases, the amount of products decreases and the amount of reactants increases.So, with increase in temperature, the equilibrium shifts to left. This is characteristic of exothermic reaction.
Hence the reaction is exothermic.

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The equilibrium constant for a reaction A+B⇋C+D is 1×10−2 at 298 K and is 2 at 273 K. The chemical process resulting in the formation of C and D is:

The equilibrium constant for a reaction $A + B ⇋ C + D$ 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: