(B) The order of a reaction is the sum of the powers of the concentration terms in the rate law expression. Given rate law: $\text{Rate} = K[H_2]^1[Br

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Order $1\frac{1}{2}$ and molecularity $2$ respectively

(B) The order of a reaction is the sum of the powers of the concentration terms in the rate law expression. Given rate law: $\text{Rate} = K[H_2]^1[Br_2]^{1/2}$. Order = $1 + 1/2 = 1.5$ or $1\frac{1}{2}$. Molecularity is the number of reacting species taking part in an elementary reaction. For the given balanced chemical equation $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$,the total number of reactant molecules is $1 + 1 = 2$. Thus,the molecularity is $2$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Medium

For the reaction $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$,the experimental data suggests the rate law is $\text{Rate} = K[H_2][Br_2]^{1/2}$. Find the order of the reaction and its molecularity.

A
Order $2$ and molecularity $2$ respectively
B
Order $1\frac{1}{2}$ and molecularity $2$ respectively
C
Order $2$ and molecularity $1\frac{1}{2}$ respectively
D
Order $1\frac{1}{2}$ and molecularity $1\frac{1}{2}$ respectively

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

For a second-order reaction where both reactants have the same initial concentration,it takes $500 \ s$ for the reaction to be $20\%$ complete. How many seconds will it take for the reaction to be $80\%$ complete (in $s$)?

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$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.

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For a reaction scheme $A$ $\xrightarrow{k_1} B$ $\xrightarrow{k_2} C$,if the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:

DifficultJEE MAIN 2019

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For the reaction, $A + B \rightarrow P$, the rate law is $\text{rate} = k[A][B]^2$. The rate of reaction is $0.25 \text{ Ms}^{-1}$ when $[A] = 1 \text{ M}$ and $[B] = 0.2 \text{ M}$ at $25^\circ \text{C}$. Calculate the rate constant $k$ of the reaction at the same temperature.

DifficultMHT CET 2026

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The rate of reaction between $A$ and $B$ increases by a factor of $100$ when the concentration of $A$ is increased $10$ folds. The order of reaction with respect to $A$ is

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$Exp. \ No.$	$[A]$	$[B]$	$Rate$
$1.$	$1.0$	$0.15$	$4.2 \times 10^{-6}$
$2.$	$2.0$	$0.15$	$8.4 \times 10^{-6}$
$3.$	$1.0$	$0.20$	$5.6 \times 10^{-6}$

For the reaction $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$,the experimental data suggests the rate law is $\text{Rate} = K[H_2][Br_2]^{1/2}$. Find the order of the reaction and its molecularity.

Similar Questions

For a second-order reaction where both reactants have the same initial concentration,it takes $500 \ s$ for the reaction to be $20\%$ complete. How many seconds will it take for the reaction to be $80\%$ complete (in $s$)?

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$. $Exp. \ No.$ $[A]$ $[B]$ $Rate$ $1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$ $2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$ $3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$ Find out the rate law.

For a reaction scheme $A$ $\xrightarrow{k_1} B$ $\xrightarrow{k_2} C$,if the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:

For the reaction, $A + B \rightarrow P$, the rate law is $\text{rate} = k[A][B]^2$. The rate of reaction is $0.25 \text{ Ms}^{-1}$ when $[A] = 1 \text{ M}$ and $[B] = 0.2 \text{ M}$ at $25^\circ \text{C}$. Calculate the rate constant $k$ of the reaction at the same temperature.

The rate of reaction between $A$ and $B$ increases by a factor of $100$ when the concentration of $A$ is increased $10$ folds. The order of reaction with respect to $A$ is

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$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.