The equilibrium constant for the reaction A-B- C-D is 2-85 at room temperature and 1-4- 10 -2 at 698K- This shows that forward reaction is-

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Standard XII

Chemistry

Le Chatelier's Principle for Del N Equals to 0

The equilibri...

Question

The equilibrium constant for the reaction $A + B ⇌ C + D$ is $2.85$ at room temperature and $1.4 \times 10^{- 2}$ at $698 K$ . This shows that forward reaction is:

Exothermic

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Endothermic

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Unpredictable

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There is no relationship between

Δ H

and

K

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Solution

The correct option is D Exothermic
With increase in temperature, the value of the equilibrium constant decreases.
As temperature increases, the amount of products decreases and the amount of reactants increases.
With increase in temperature, the equilibrium shifts to left.
This is characteristic of exothermic reaction.

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Q. The equilibrium constant K for the reaction

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The equilibrium constant for the reaction A+B⇌C+D is 2.85 at room temperature and 1.4×10−2 at 698K. This shows that forward reaction is:

The equilibrium constant for the reaction $A + B ⇌ C + D$ is $2.85$ at room temperature and $1.4 \times 10^{- 2}$ at $698 K$ . This shows that forward reaction is: