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Statement 1 : A reaction $2 {SO}_{2} + O_{2} ⇌ 2 {SO}_{3};$ has $K_{P}$ at 298 K and 500 K as $4.0 \times 10^{24}$ and $8.5 \times 10^{10}$ respectively.
Statement 2 : The $E_{a}$ for the forward reaction is lesser than $E_{b}$ for the backward reaction.

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Both Statement 1 and Statement 2 are true.

Statement 1 is true and statement 2 is false.

Statement 1 is false and Statement 2 is true.

Both statement 1 and Statement 2 are false.

answer is A.

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Detailed Solution

$K_{P}$ decreases with temperature and thus, $∆ H = - ve .$ Also, $∆ H = E_{a} (f) - E_{a} (b)$ . The negative value of $∆ H$ is possible only when $E_{a} (b) > E_{a} (f) .$

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