Question

The rate of formation of $S{O}_3$ in the reaction $2S{O}_2+O_2\to 2S{O}_{3}is100gmi{n}^{-1}$. Hence rate of disappearance of $O_2$ is:

• A. 50g $mi{n}^{-1}$
• B. 100g $mi{n}^{-1}$
• C. 20g $mi{n}^{-1}$
• D. 40g $mi{n}^{-1}$

Answer 1

The correct option is C 20g $mi{n}^{-1}$

$-\frac{1}{2}\frac{d\left[S{O}_3\right]}{dt}$ = $-\frac{d\left[O_2\right]}{dt}$

$\frac{1}{2}\times \frac{100}{80}$ = $\frac{x}{32}$

$RateofDisappearanceof{O}_2=20g{min}^{-1}$