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
$1,\,\frac{1}{2}$
Similar Questions
The half-life of decomposition of gaseous $CH_3CHO$ at initial pressure of $364\, mm$ and $182\, mm$ of $Hg$ were $440\, sec$ and $880\, sec$ respectively. The order of the reaction is
The half-life of decomposition of gaseous $CH_3CHO$ at initial pressure of $364\, mm$ and $182\, mm$ of $Hg$ were $440\, sec$ and $880\, sec$ respectively. The order of the reaction is
The mechanism for the reaction is given below $2P + Q \to S + T$ $P + Q \to R + S$(slow)$P + R \to T$ (fast)The rate law expression for the reaction is
The mechanism for the reaction is given below $2P + Q \to S + T$ $P + Q \to R + S$(slow)$P + R \to T$ (fast)The rate law expression for the reaction is
If doubling the initial concentration of reactant doubles $t_{1/2}$ of reaction, the order of reaction is
If doubling the initial concentration of reactant doubles $t_{1/2}$ of reaction, the order of reaction is
For an elementary reaction, $2A + B \to C + D$ the molecularity is
For an elementary reaction, $2A + B \to C + D$ the molecularity is
The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor
The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor