Question

$S{O}_2$ reacts with $O_2$ as follows $2S{O}_2+O_2\to 2S{O}_3$ the rate of disappearance of $S{O}_2$ is $2.4\times {10}^{-4}mol$ $li{t}^{-1}mi{n}^{-1}$Then:

• A. rate of reaction is $1.2\times {10}^{-4}moleli{t}^{-1}mi{n}^{-1}$
• B. rate of appearance of $S{O}_3$ is $2.4\times {10}^{-4}moleli{t}^{-1}mi{n}^{-1}$
• C. rate of disappearance of $O_2$ is $1.2\times {10}^{-4}moleli{t}^{-1}mi{n}^{-1}$
• D. rate or reaction is twice the rate of disappearance of $S{O}_3$

Answer 1

The correct option is A rate of reaction is $1.2\times {10}^{-4}moleli{t}^{-1}mi{n}^{-1}$

Rate = $-\frac{1}{2}\frac{d\left[S{O}_2\right]}{dt}=\frac{-d\left[O_2\right]}{dt}=\frac{1}{2}\frac{d\left[S{O}_2\right]}{dt}$

$\therefore$Rate = $\frac{1}{2}\times 2.4\times {10}^{-4}$ = $1.2\times {10}^{-4}mol{L}^{-1}{min}^{-1}$

Similarily, the rate of appearance of $S{O}_3$ will be $1.2\times {10}^{-4}$ and rate of disapperance of $O_2$ will be $-1.2\times {10}^{-4}$