Question

If the rate of reaction:
$2S{O}_2\left(g\right)+O_2\left(g\right)\stackrel{Pt}{\to }2S{O}_3\left(g\right)$ is given by:
$Rate=\frac{K\left[S{O}_2\right]}{[S{O}_3{]}^{1/2}}$
Which statements are correct?

• A. The overall order of reaction is -1/2
• B. The overall order of reaction is +1/2
• C. The reaction slows down as the product $S{O}_3$ is build up
• D. The rate of reaction does not depend upon concentration of $S{O}_3$ formed

Answer 1

Answer: (B), (C)

The correct options are
B The overall order of reaction is +1/2
C The reaction slows down as the product $S{O}_3$ is build up

The overall order of reaction is +1/2{1-1/2 =1/2}.The reaction slows down as the product $S{O}_3$ is build up.The rate of reaction depend upon concentration of $S{O}_2$and $O_2$.
Rate of a reaction is directly proportional to the concentration of reactants.