For a reaction $A + B \to \text{Products}$,the rate law is: $\text{Rate} = k[A][B]^{3/2}$. Can the reaction be an elementary reaction? Explain.
(N/A) An elementary reaction is a single-step process where the order of the reaction is equal to the sum of the stoichiometric coefficients of the reactants.
For an elementary reaction,the order must be an integer (usually $1, 2, \text{or } 3$).
In the given rate law,$\text{Rate} = k[A]^1[B]^{3/2}$,the overall order of the reaction is $1 + 3/2 = 5/2 = 2.5$.
Since the order of the reaction is fractional,it cannot be an elementary reaction.
For an elementary reaction,the order must be an integer (usually $1, 2, \text{or } 3$).
In the given rate law,$\text{Rate} = k[A]^1[B]^{3/2}$,the overall order of the reaction is $1 + 3/2 = 5/2 = 2.5$.
Since the order of the reaction is fractional,it cannot be an elementary reaction.
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Similar Questions
Consider the gaseous reaction $A_2 + B_2 \rightarrow 2 AB$. The following data was obtained for the above reaction:
$[A_2]_0$ $[B_2]_0$ Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$ $0.1 \ M$ $0.1 \ M$ $2.5 \times 10^{-4}$ $0.2 \ M$ $0.1 \ M$ $5.0 \times 10^{-4}$ $0.2 \ M$ $0.2 \ M$ $1.0 \times 10^{-3}$
The value of the rate constant for the above reaction is:
| $[A_2]_0$ | $[B_2]_0$ | Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$ |
| $0.1 \ M$ | $0.1 \ M$ | $2.5 \times 10^{-4}$ |
| $0.2 \ M$ | $0.1 \ M$ | $5.0 \times 10^{-4}$ |
| $0.2 \ M$ | $0.2 \ M$ | $1.0 \times 10^{-3}$ |
The value of the rate constant for the above reaction is:
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