(B) 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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The order of a reaction can only be determined experimentally.

(B) 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 cannot be determined simply by looking at the stoichiometric coefficients in a balanced chemical equation. Therefore,the correct statement is that the order of a reaction can only be determined experimentally.

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

Medium

Which of the following statements is true regarding the order of a reaction?

A
The order of a reaction increases with an increase in temperature.
B
The order of a reaction can only be determined experimentally.
C
The order of a reaction can be determined from the balanced chemical equation.
D
None of the above.

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Class 12 Questions

Class 12

Chemistry Questions

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

Differential form of the rate equation is $\frac{dx}{dt} = k[P][Q]^{0.5}[R]^{0.5}$. Which statement about the above equation is wrong?

Medium

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$A$ reaction is first order with respect to $A$ and second order with respect to $B$. What is the effect on the reaction rate if the concentration of $B$ is increased $3$ times?

MediumMHT CET 2021

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The order of the reaction occurring by the following mechanism should be:
$(i)$ $A_2 \to A + A$ (fast)
$(ii)$ $A + B_2 \to AB + B$ (slow)
$(iii)$ $A + B \to AB$ (fast)

Easy

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For the reaction $aA + bB \to$ product,the rate of reaction is given by $Rate = k[A]^3 [B]^0$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the rate of reaction will be: (in $\times$)

Easy

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If doubling the concentration of a reactant $A$ increases the rate $4$ times and tripling the concentration of $A$ increases the rate $9$ times,the rate is proportional to

MediumAIIMS 1991

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Which of the following statements is true regarding the order of a reaction?

Similar Questions

Differential form of the rate equation is $\frac{dx}{dt} = k[P][Q]^{0.5}[R]^{0.5}$. Which statement about the above equation is wrong?

$A$ reaction is first order with respect to $A$ and second order with respect to $B$. What is the effect on the reaction rate if the concentration of $B$ is increased $3$ times?

The order of the reaction occurring by the following mechanism should be:$(i)$ $A_2 \to A + A$ (fast)$(ii)$ $A + B_2 \to AB + B$ (slow)$(iii)$ $A + B \to AB$ (fast)

For the reaction $aA + bB \to$ product,the rate of reaction is given by $Rate = k[A]^3 [B]^0$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the rate of reaction will be: (in $\times$)

If doubling the concentration of a reactant $A$ increases the rate $4$ times and tripling the concentration of $A$ increases the rate $9$ times,the rate is proportional to

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The order of the reaction occurring by the following mechanism should be:
$(i)$ $A_2 \to A + A$ (fast)
$(ii)$ $A + B_2 \to AB + B$ (slow)
$(iii)$ $A + B \to AB$ (fast)