(B) The order of a reaction is an experimental quantity and can indeed have a fractional value. Thus,the Assertion is true.The order of a reaction is

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If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.

(B) The order of a reaction is an experimental quantity and can indeed have a fractional value. Thus,the Assertion is true.The order of a reaction is determined experimentally and cannot be deduced simply from the stoichiometric coefficients in a balanced chemical equation,as the reaction mechanism may involve multiple steps. Thus,the Reason is also true.However,the fact that the order is fractional (Assertion) is not explained by the fact that it cannot be determined from the balanced equation (Reason). Therefore,both are correct,but the Reason is not the correct explanation of the Assertion.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

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Assertion: The order of a reaction can have a fractional value.
Reason: The order of a reaction cannot be determined from the balanced chemical equation of a reaction.

AIIMS 2008 All AIIMS

A
If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.
B
If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.
C
If the Assertion is correct but Reason is incorrect.
D
If both the Assertion and Reason are incorrect.

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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AIIMS 2008 Paper All AIIMS years →

The initial rates of decrease of $I_2$ in acetone-iodine reaction catalysed by $H^{+}$ are given in the table.
Experiment Initial $[I_2]$ $(mol \ L^{-1})$ Initial $[H^{+}]$ $(mol \ L^{-1})$ Initial $[CH_3COCH_3]$ $(mol \ L^{-1})$ Initial rate $(mol \ L^{-1} \ s^{-1})$
$1$ $0.01$ $0.1$ $0.1$ $0.096$
$2$ $0.01$ $0.2$ $0.1$ $0.192$
$3$ $0.02$ $0.2$ $0.1$ $0.192$
$4$ $0.01$ $0.2$ $0.2$ $0.384$

The order with respect to $I_2, H^{+}$,acetone and total order of the reaction respectively are:

EasyAP EAMCET 2018

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For any reaction,the rate constant $K = 2.3 \times 10^{-5} \ mol^{-3/2} \ L^{3/2} \ S^{-1}$. The order of the reaction is . . . . . . .

EasyGUJCET 2024

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For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:
Entry $[A]$ in $M$ $[B]$ in $M$ Initial rate $(M/s)$
$1$ $0.02$ $0.02$ $2 \times 10^{-2}$
$2$ $0.02$ $0.04$ $4 \times 10^{-2}$
$3$ $0.04$ $0.04$ $8 \times 10^{-2}$

Entry	$[A]$ in $M$	$[B]$ in $M$	Initial rate $(M/s)$
$1$	$0.02$	$0.02$	$2 \times 10^{-2}$
$2$	$0.02$	$0.04$	$4 \times 10^{-2}$
$3$	$0.04$	$0.04$	$8 \times 10^{-2}$

DifficultTS EAMCET 2021

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The rate of reaction,$A + B \rightarrow \text{product}$,is $7.2 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ at $[A] = 0.4 \ mol \ dm^{-3}$ and $[B] = 0.1 \ mol \ dm^{-3}$. The reaction is first order in $A$ and second order in $B$. Calculate the rate constant.

EasyMHT CET 2024

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The mechanism of the decomposition of nitramide $(NH_2NO_2)$ in aqueous solution is given below:
$NH_2NO_2(aq) + OH^-(aq) \to NHNO_2^-(aq) + H_2O(l)$
$NHNO_2^-(aq) \to N_2O(aq) + OH^-(aq)$
Identify the catalyst for this reaction.

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Experiment	Initial $[I_2]$ $(mol \ L^{-1})$	Initial $[H^{+}]$ $(mol \ L^{-1})$	Initial $[CH_3COCH_3]$ $(mol \ L^{-1})$	Initial rate $(mol \ L^{-1} \ s^{-1})$
$1$	$0.01$	$0.1$	$0.1$	$0.096$
$2$	$0.01$	$0.2$	$0.1$	$0.192$
$3$	$0.02$	$0.2$	$0.1$	$0.192$
$4$	$0.01$	$0.2$	$0.2$	$0.384$

Assertion: The order of a reaction can have a fractional value.Reason: The order of a reaction cannot be determined from the balanced chemical equation of a reaction.

Similar Questions

For any reaction,the rate constant $K = 2.3 \times 10^{-5} \ mol^{-3/2} \ L^{3/2} \ S^{-1}$. The order of the reaction is . . . . . . .

For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:Entry$[A]$ in $M$$[B]$ in $M$Initial rate $(M/s)$$1$$0.02$$0.02$$2 \times 10^{-2}$$2$$0.02$$0.04$$4 \times 10^{-2}$$3$$0.04$$0.04$$8 \times 10^{-2}$

The rate of reaction,$A + B \rightarrow \text{product}$,is $7.2 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ at $[A] = 0.4 \ mol \ dm^{-3}$ and $[B] = 0.1 \ mol \ dm^{-3}$. The reaction is first order in $A$ and second order in $B$. Calculate the rate constant.

The mechanism of the decomposition of nitramide $(NH_2NO_2)$ in aqueous solution is given below:$NH_2NO_2(aq) + OH^-(aq) \to NHNO_2^-(aq) + H_2O(l)$$NHNO_2^-(aq) \to N_2O(aq) + OH^-(aq)$Identify the catalyst for this reaction.

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Assertion: The order of a reaction can have a fractional value.
Reason: The order of a reaction cannot be determined from the balanced chemical equation of a reaction.

For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:
Entry $[A]$ in $M$ $[B]$ in $M$ Initial rate $(M/s)$
$1$ $0.02$ $0.02$ $2 \times 10^{-2}$
$2$ $0.02$ $0.04$ $4 \times 10^{-2}$
$3$ $0.04$ $0.04$ $8 \times 10^{-2}$

The mechanism of the decomposition of nitramide $(NH_2NO_2)$ in aqueous solution is given below:
$NH_2NO_2(aq) + OH^-(aq) \to NHNO_2^-(aq) + H_2O(l)$
$NHNO_2^-(aq) \to N_2O(aq) + OH^-(aq)$
Identify the catalyst for this reaction.