Why is molecularity applicable only for elementary reactions,while order is applicable for both elementary and complex reactions?
(N/A) An elementary reaction is a single-step process where the molecularity is defined as the number of reacting species taking part in the collision.
In contrast,a complex reaction occurs through a series of elementary steps.
Since each step in a complex reaction may have a different number of molecules involved,the molecularity of the overall complex reaction is not defined or is considered meaningless.
However,the order of a reaction is an experimentally determined quantity that depends on the rate-determining step (the slowest step) of the mechanism,making it applicable to both elementary and complex reactions.
In contrast,a complex reaction occurs through a series of elementary steps.
Since each step in a complex reaction may have a different number of molecules involved,the molecularity of the overall complex reaction is not defined or is considered meaningless.
However,the order of a reaction is an experimentally determined quantity that depends on the rate-determining step (the slowest step) of the mechanism,making it applicable to both elementary and complex reactions.
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Similar Questions
Which of the following statements is incorrect?
Easy
View SolutionIf a reaction has the experimental rate expression $\text{rate} = K [A]^2[B]$,what happens to the reaction rate if the concentration of $A$ is doubled and the concentration of $B$ is halved?
Medium
View SolutionThe results given in the below table were obtained during kinetic studies of the following reaction:
$2 A + B \longrightarrow C + D$
Experiment $[A] / mol \ L^{-1}$ $[B] / mol \ L^{-1}$ Initial rate / $mol \ L^{-1} \ min^{-1}$ $I$ $0.1$ $0.1$ $6.00 \times 10^{-3}$ $II$ $0.1$ $0.2$ $2.40 \times 10^{-2}$ $III$ $0.2$ $0.1$ $1.20 \times 10^{-2}$ $IV$ $X$ $0.2$ $7.20 \times 10^{-2}$ $V$ $0.3$ $Y$ $2.88 \times 10^{-1}$
$X$ and $Y$ in the given table are respectively :
$2 A + B \longrightarrow C + D$
| Experiment | $[A] / mol \ L^{-1}$ | $[B] / mol \ L^{-1}$ | Initial rate / $mol \ L^{-1} \ min^{-1}$ |
| $I$ | $0.1$ | $0.1$ | $6.00 \times 10^{-3}$ |
| $II$ | $0.1$ | $0.2$ | $2.40 \times 10^{-2}$ |
| $III$ | $0.2$ | $0.1$ | $1.20 \times 10^{-2}$ |
| $IV$ | $X$ | $0.2$ | $7.20 \times 10^{-2}$ |
| $V$ | $0.3$ | $Y$ | $2.88 \times 10^{-1}$ |
$X$ and $Y$ in the given table are respectively :
DifficultJEE MAIN 2020
View SolutionThe rate law for the reaction $A + 2B \rightarrow C + 2D$ is given by:
Easy
View SolutionFor the reaction,$H_{2(g)} + Br_{2(g)} \longrightarrow 2 HBr_{(g)}$,$r = k[H_2][Br_2]^{\frac{1}{2}}$. What is the molecularity and order of reaction respectively?
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