For the reaction ${H_2}(g) + B{r_2}(g) \to 2HBr(g)$, the experimental data suggest, rate $ = K[{H_2}]{[B{r_2}]^{1/2}}$. The molecularity and order of the reaction are respectively
For the reaction ${H_2}(g) + B{r_2}(g) \to 2HBr(g)$, the experimental data suggest, rate $ = K[{H_2}]{[B{r_2}]^{1/2}}$. The molecularity and order of the reaction are respectively
- A
$2,\,\frac{3}{2}$
- B
$\frac{3}{2},\,\frac{3}{2}$
- C
$1, 1$
- D
$1,\,\frac{1}{2}$
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