Statement 1: The value of the equilibrium constant is affected by temperature.
Statement 2: An increase in temperature causes more effective collisions to occur between the particles reacting.

Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1

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Both Statement 1 and Statement 2 are correct, but Statement 2 is NOT the correct explanation of Statement 1.

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Statement 1 is correct, but Statement 2 is not correct.

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Statement 1 is not correct, but Statement 2 is correct.

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Solution

The correct option is B Both Statement 1 and Statement 2 are correct, but Statement 2 is NOT the correct explanation of Statement 1.
By Van't Hoff equation,
$\frac{d l n K_{C}}{d T} = \frac{△ U^{0}}{{R T}^{2}}$ $\to$ change in internal energy of reaction at standard states
$↙$ $↓$
universal temperature
gas constant
So, by above equation, we can say that $K_{C}$ is dependent on temperature.
Now, $l n \frac{{(K_{C})}_{1}}{{(K_{C})}_{2}} = \frac{△ H}{2.303 R} (\frac{T_{2} - T_{1}}{T_{1} T_{2}})$
Now, as temperature increases, the molecule will gain higher energy so there will be more no. of collisions among the particle reacting.

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Statement 1: The value of the equilibrium constant is affected by temperature. Statement 2: An increase in temperature causes more effective collisions to occur between the particles reacting.

Statement 1: The value of the equilibrium constant is affected by temperature.
Statement 2: An increase in temperature causes more effective collisions to occur between the particles reacting.