What is the molecularity of a reaction? Expla | vedclass

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(N/A) The molecularity of a reaction is defined as the total number of reacting species (atoms,ions,or molecules) that must collide simultaneously in

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(N/A) The molecularity of a reaction is defined as the total number of reacting species (atoms,ions,or molecules) that must collide simultaneously in an elementary reaction to bring about a chemical change.
$(a)$ Unimolecular reaction: Involves only one reacting species.
Example: Decomposition of ammonium nitrite: $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(g)$
$(b)$ Bimolecular reaction: Involves the simultaneous collision of two reacting species.
Example: Dissociation of hydrogen iodide: $2HI(g) \rightarrow H_2(g) + I_2(g)$
$(c)$ Trimolecular (or termolecular) reaction: Involves the simultaneous collision of three reacting species.
Example: $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
Reactions with molecularity greater than three are very rare because the probability of simultaneous collision of more than three molecules is extremely low.

$Observation$	$[A] \ (mol \ L^{-1})$	$[B] \ (mol \ L^{-1})$	$Rate \ (mol \ L^{-1} \ sec^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.2$	$0.1$	$4 \times 10^{-3}$
$3$	$0.1$	$0.2$	$8 \times 10^{-3}$

What is the molecularity of a reaction? Explain its types with examples.

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$Observation$ $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ $Rate \ (mol \ L^{-1} \ sec^{-1})$

$1$ $0.1$ $0.1$ $2 \times 10^{-3}$

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