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