Medium
What is the molecularity of a reaction? Explain its types with examples.
(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.
$(a)$ 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.
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Similar Questions
Identify the reaction order from each of the following rate constants.
$(i)$ $k = 2.3 \times 10^{-5} \, L \, mol^{-1} \, s^{-1}$
$(ii)$ $k = 3 \times 10^{-4} \, s^{-1}$
$(i)$ $k = 2.3 \times 10^{-5} \, L \, mol^{-1} \, s^{-1}$
$(ii)$ $k = 3 \times 10^{-4} \, s^{-1}$
Medium
View SolutionFor the reaction between $A$ and $B$,the initial rate of reaction $(r_0)$ was measured for different initial concentrations of $A$ and $B$ as given below. Determine the order of the reaction with respect to $A$ and $B$ respectively.
$[A] / mol \ L^{-1}$ $0.2, 0.2, 0.4$ $[B] / mol \ L^{-1}$ $0.3, 0.1, 0.05$ $r_0 / mol \ L^{-1} s^{-1}$ $5.0 \times 10^{-5}, 5.0 \times 10^{-5}, 1.4 \times 10^{-4}$
| $[A] / mol \ L^{-1}$ | $0.2, 0.2, 0.4$ |
| $[B] / mol \ L^{-1}$ | $0.3, 0.1, 0.05$ |
| $r_0 / mol \ L^{-1} s^{-1}$ | $5.0 \times 10^{-5}, 5.0 \times 10^{-5}, 1.4 \times 10^{-4}$ |
Difficult
View SolutionIf the surface area of the reactants increases,then the order of the reaction:
Easy
View SolutionFor the reaction $2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. What is the concentration of $N_2O_5$?
Considering the reaction $aG + bH \rightarrow \text{Products}$,when the concentrations of both reactants $G$ and $H$ are doubled,the rate increases by $8$ times. However,when the concentration of $G$ is doubled while the concentration of $H$ remains constant,the rate doubles. What is the overall order of the reaction?
Medium
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