For the reaction, ${{\rm{H}}_2}\left( {\rm{g}} \right) + {\rm{B}}{{\rm{r}}_2}\left( {\rm{g}} \right) \to 2{\rm{HBr}}\left( {\rm{g}} \right)$ The experimental data suggest ${\rm{rate}} = k\left[ {{{\rm{H}}_2}} \right]{\left[ {{\rm{B}}{{\rm{r}}_2}} \right]^{1/2}}$ the molecularity and order of the reaction are respectively

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

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For the reaction,

{\mathrm{H}_2}\left( \mathrm{g} \right) + \mathrm{B}{\mathrm{r}_2}\left( \mathrm{g} \right) \to 2\mathrm{HBr}\left( \mathrm{g} \right)

The experimental data suggest

\mathrm{rate} = k\left[ {{\mathrm{H}_2}} \right]{\left[ {\mathrm{B}{\mathrm{r}_2}} \right]^{1/2}}

the molecularity and order of the reaction are respectively

View answer and explanation

Correct option: D

2,\frac{3}{2}

Option D (2,

\frac{3}{2}

) is correct because molecularity is the number of reacting molecules (2), and the order is the sum of the exponents in the rate law (1 + 1/2 = 3/2).