(D) The order of a reaction is an experimental quantity and can be zero,an integer,or a fraction. Since the order of a reaction can indeed be fraction

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(D) The order of a reaction is an experimental quantity and can be zero,an integer,or a fraction. Since the order of a reaction can indeed be fractional,the statement that 'Order cannot be fractional' is incorrect. Therefore,option $D$ is the correct answer.

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

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Which one of the following statements regarding the order of a reaction is not correct?

A
Order is determined experimentally.
B
Order of reaction is equal to the sum of powers of concentration terms in the experimental rate law.
C
It is not affected by the stoichiometric coefficients of the reactants.
D
Order cannot be fractional.

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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

For the reaction $2A + B \rightarrow C$,the rate law is given by $\text{Rate} = k[A][B]$. Which of the following statements is correct for this reaction?

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The rate law for the reaction $A^{+} + B^{+} + C \longrightarrow \text{Product}$ is expressed as $\text{Rate} = k[A]^{2}[B]^{1}[C]^{0}$. What is the overall order of the reaction?

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For a reaction,$I^{-} + OCl^{-} \to IO^{-} + Cl^{-}$ in an aqueous medium,the rate of reaction is given by $\frac{d[IO^{-}]}{dt} = K \frac{[I^{-}][OCl^{-}]}{[OH^{-}]}$. The overall order of reaction is

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For a chemical reaction,$2A + 2B \to C + D$,the order of reaction is $1$ with respect to $A$ and $1$ with respect to $B$. The initial rate of the reaction is $4 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. When $50\%$ of the reactants are converted into products,the rate of the reaction would become:

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For the reaction $A + B \rightarrow \text{Product}$,if the concentration of $A$ is doubled,the reaction rate doubles. When the concentration of $B$ is doubled,the reaction rate remains unchanged. What is the overall order of the reaction?

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Which one of the following statements regarding the order of a reaction is not correct?

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For the reaction $2A + B \rightarrow C$,the rate law is given by $\text{Rate} = k[A][B]$. Which of the following statements is correct for this reaction?

The rate law for the reaction $A^{+} + B^{+} + C \longrightarrow \text{Product}$ is expressed as $\text{Rate} = k[A]^{2}[B]^{1}[C]^{0}$. What is the overall order of the reaction?

For a reaction,$I^{-} + OCl^{-} \to IO^{-} + Cl^{-}$ in an aqueous medium,the rate of reaction is given by $\frac{d[IO^{-}]}{dt} = K \frac{[I^{-}][OCl^{-}]}{[OH^{-}]}$. The overall order of reaction is

For a chemical reaction,$2A + 2B \to C + D$,the order of reaction is $1$ with respect to $A$ and $1$ with respect to $B$. The initial rate of the reaction is $4 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. When $50\%$ of the reactants are converted into products,the rate of the reaction would become:

For the reaction $A + B \rightarrow \text{Product}$,if the concentration of $A$ is doubled,the reaction rate doubles. When the concentration of $B$ is doubled,the reaction rate remains unchanged. What is the overall order of the reaction?

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