Question

For the reaction $2S{O}_2+O_2⟶2S{O}_3$ if rate of disappearance of $O_2$ is 8 g/s, then rate of appearance of $S{O}_3$ will be:

• A. 16 g/s
• B. 4 g/s
• C. 40 g/s
• D. 10 g/s

Answer 1

The correct option is C 40 g/s

Rate of the reaction $⟹$
$\frac{-1}{2}\frac{d\left[S{O}_2\right]}{dt}=\frac{-d\left[O_2\right]}{dt}=\frac{1}{2}\frac{d\left[S{O}_3\right]}{dt}$
Rate of disapperance of $O_2=\frac{-d\left[O_2\right]}{dt}=\frac{8}{32}mol/s$
Rate of apperance of $S{O}_3=2\times \frac{-d\left[O_2\right]}{dt}=0.5mol/s=40g/s$