Question

Rate of formation of $S{O}_3$ in the following reaction $2S{O}_2+O_2\to 2S{O}_3$ is 100 g/min. Hence rate of disappearance of $O_2$ is

• A. 50 g/min
• B. 40 g/min
• C. 200 g/min
• D. 20 g/min

Answer 1

The correct option is D 20 g/min

$\frac{-d\left[o_2\right]}{dt}=\frac{1}{2}\frac{d\left[s{o}_3\right]}{dt}\frac{d\left[S{O}_3\right]}{dt}=\frac{100}{80}mol/min\frac{-d\left[o_2\right]}{dt}=\frac{100}{2\times 80}mol/min=\frac{100}{2\times 80}\times 32gm/min=20gm/min$