Medium
Write about elementary and complex reactions.
(N/A) balanced chemical equation does not provide a complete picture of how a reaction proceeds.
$(a)$ Elementary reaction: Reactions that occur in a single step are known as elementary reactions. For these reactions,the order is equal to the molecularity.
$(b)$ Complex reaction: Reactions that proceed through a sequence of elementary steps (collectively called the reaction mechanism) to form products are known as complex reactions.
Complex reactions involving more than three molecules in the stoichiometric equation must occur in multiple steps.
For complex reactions,the overall order is determined by the slowest step,and the molecularity of this slowest step corresponds to the order of the overall reaction.
Examples: $(i)$ The oxidation of ethane to $CO_2$ and $H_2O$ involves a series of intermediate steps forming alcohol,aldehyde,and acid. $(ii)$ Reverse reactions and side reactions (e.g.,the nitration of phenol yields both $o$-nitrophenol and $p$-nitrophenol).
$(a)$ Elementary reaction: Reactions that occur in a single step are known as elementary reactions. For these reactions,the order is equal to the molecularity.
$(b)$ Complex reaction: Reactions that proceed through a sequence of elementary steps (collectively called the reaction mechanism) to form products are known as complex reactions.
Complex reactions involving more than three molecules in the stoichiometric equation must occur in multiple steps.
For complex reactions,the overall order is determined by the slowest step,and the molecularity of this slowest step corresponds to the order of the overall reaction.
Examples: $(i)$ The oxidation of ethane to $CO_2$ and $H_2O$ involves a series of intermediate steps forming alcohol,aldehyde,and acid. $(ii)$ Reverse reactions and side reactions (e.g.,the nitration of phenol yields both $o$-nitrophenol and $p$-nitrophenol).
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Similar Questions
For 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 $N_2O_5$?
The experimental data for the reaction $2A + B_2 \longrightarrow 2AB$ is given below:
Exp. $[A] \ (mol \ L^{-1})$ $[B_2] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ S^{-1})$ $1$ $0.50$ $0.50$ $1.6 \times 10^{-4}$ $2$ $0.50$ $1.00$ $3.2 \times 10^{-4}$ $3$ $1.00$ $1.00$ $3.2 \times 10^{-4}$
Determine the rate law for the reaction.
| Exp. | $[A] \ (mol \ L^{-1})$ | $[B_2] \ (mol \ L^{-1})$ | Rate $(mol \ L^{-1} \ S^{-1})$ |
|---|---|---|---|
| $1$ | $0.50$ | $0.50$ | $1.6 \times 10^{-4}$ |
| $2$ | $0.50$ | $1.00$ | $3.2 \times 10^{-4}$ |
| $3$ | $1.00$ | $1.00$ | $3.2 \times 10^{-4}$ |
Determine the rate law for the reaction.
Difficult
View SolutionWhat is the order of reaction for the decomposition of gaseous acetaldehyde?
The following data are obtained for a reaction,$X + Y \rightarrow$ Products.
$Expt.$ $[X]_0 / mol \ L^{-1}$ $[Y]_0 / mol \ L^{-1}$ $Rate / mol \ L^{-1} s^{-1}$ $1$ $0.25$ $0.25$ $1.0 \times 10^{-6}$ $2$ $0.50$ $0.25$ $4.0 \times 10^{-6}$ $3$ $0.25$ $0.50$ $8.0 \times 10^{-6}$
The overall order of the reaction is:
| $Expt.$ | $[X]_0 / mol \ L^{-1}$ | $[Y]_0 / mol \ L^{-1}$ | $Rate / mol \ L^{-1} s^{-1}$ |
| $1$ | $0.25$ | $0.25$ | $1.0 \times 10^{-6}$ |
| $2$ | $0.50$ | $0.25$ | $4.0 \times 10^{-6}$ |
| $3$ | $0.25$ | $0.50$ | $8.0 \times 10^{-6}$ |
The overall order of the reaction is:
MediumKVPY 2012
View SolutionThe rate constant for the reaction, $2 \,N_2O_{5(g)} \rightarrow 2 \,N_2O_{4(g)} + O_{2(g)}$ is $4.98 \times 10^{-4} \,s^{-1}$. What is the order of the reaction?
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