(D) The order of a reaction is defined as the sum of the powers of the concentration terms in the rate law expression. It is an experimental quantity

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Order of reaction is always a whole number.

(D) The order of a reaction is defined as the sum of the powers of the concentration terms in the rate law expression. It is an experimental quantity and is not necessarily related to the stoichiometric coefficients of the balanced chemical equation. The order of a reaction can be zero,a whole number,or even a fraction. Therefore,the statement that the order of reaction is always a whole number is incorrect.

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

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Which one of the following statements for the order of a reaction is incorrect?

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A
Order can be determined only experimentally.
B
Order is not influenced by stoichiometric coefficient of the reactants.
C
Order of a reaction is the sum of powers to the concentration terms of reactants to express the rate of reaction.
D
Order of reaction is always a whole number.

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Rate law , Rate constant , Order of Reaction and Molecularity

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The diazonium salt decomposes as $C_6H_5N_2^+Cl^- \to C_6H_5Cl + N_2$. At $0 \ ^\circ C$,the evolution of $N_2$ becomes two times faster when the initial concentration of the salt is doubled. Therefore,it is:

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For the reaction $2NO + Cl_2 \rightarrow 2NOCl$,the following mechanism is proposed. What will be the rate law for the reaction? $NO + Cl_2 \rightleftharpoons NOCl_2$ (fast); $NOCl_2 + NO \rightarrow 2NOCl$ (slow)

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$A$ reaction $2A + B \xrightarrow{k} C + D$ is first order with respect to $A$ and second order with respect to $B$. Initial concentration $(t = 0)$ of $A$ is $C_0$ while $B$ is $2C_0$. If at $t = 30 \min$ the concentration of $C$ is $C_0/4$,then the rate expression at $t = 30 \min$ is:

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The reaction $2N_2O_5 \rightleftharpoons 2N_2O_4 + O_2$ is

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For the reaction $AB_5 \to AB + 4B$,if $- \frac{d[AB_5]}{dt} = K_1[AB_5]$ and $\frac{d[B]}{dt} = K_2[AB_5]$,then:

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Which one of the following statements for the order of a reaction is incorrect?

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The diazonium salt decomposes as $C_6H_5N_2^+Cl^- \to C_6H_5Cl + N_2$. At $0 \ ^\circ C$,the evolution of $N_2$ becomes two times faster when the initial concentration of the salt is doubled. Therefore,it is:

For the reaction $2NO + Cl_2 \rightarrow 2NOCl$,the following mechanism is proposed. What will be the rate law for the reaction? $NO + Cl_2 \rightleftharpoons NOCl_2$ (fast); $NOCl_2 + NO \rightarrow 2NOCl$ (slow)

$A$ reaction $2A + B \xrightarrow{k} C + D$ is first order with respect to $A$ and second order with respect to $B$. Initial concentration $(t = 0)$ of $A$ is $C_0$ while $B$ is $2C_0$. If at $t = 30 \min$ the concentration of $C$ is $C_0/4$,then the rate expression at $t = 30 \min$ is:

The reaction $2N_2O_5 \rightleftharpoons 2N_2O_4 + O_2$ is

For the reaction $AB_5 \to AB + 4B$,if $- \frac{d[AB_5]}{dt} = K_1[AB_5]$ and $\frac{d[B]}{dt} = K_2[AB_5]$,then:

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