Question

Which of the following statement is true for the reaction, $H_2+{Br}_2\to 2HBr$. The rate law is $\frac{dx}{dt}=k\left[H_2\right]{\left[{Br}_2\right]}^{1/2}$:

• A. order of reaction is $1.5$
• B. molecularity of the reaction is $2$
• C. by increasing the concentration of ${Br}_2$ four times the rate of reaction is doubled
• D. all the above are correct

Answer 1

The correct option is D all the above are correct

All the given statements are correct.
Order of reaction $=1+\frac{1}{2}=1.5$
Molecularity$=1+1=2$
$\frac{dx}{dt}\propto {\left[Br\right]}^{1/2}$
So, reaction rate will be doubled if concentration of ${Br}_2$ is increased by $4$ times.