Question

The rate of formation of $S{O}_3$ in the following reaction $2S{O}_2+O_2\to 2S{O}_3$ is $10gse{c}^{-1}$. The rate of disappearance of $O_2$ will be:

• A. $5gse{c}^{-1}$
• B. $100gse{c}^{-1}$
• C. $20gsec$
• D. $2gse{c}^{-1}$

Answer 1

The correct option is A $5gse{c}^{-1}$

Given, Rate of Formation of $S{O}_3$ is $10g{sec}^{-1}$

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

$\frac{1}{2}\times 10g{sec}^{-1}$ = $5g{sec}^{-1}$ = $-\frac{d\left[O_2\right]}{dt}$ = Rate of Disappearance of $O_2$