(A) The rate law is determined experimentally by measuring the rate of reaction at different concentrations of reactants. Therefore,the statement that

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The rate law for any reaction cannot be determined experimentally.

(A) The rate law is determined experimentally by measuring the rate of reaction at different concentrations of reactants. Therefore,the statement that the rate law cannot be determined experimentally is incorrect. Complex reactions often exhibit fractional orders,bimolecular reactions involve the collision of two species,and molecularity is a concept defined specifically for elementary reactions.

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

Easy

Which of the following statements is incorrect?

KCET 2017 All KCET

A
The rate law for any reaction cannot be determined experimentally.
B
Complex reactions have fractional order.
C
Bimolecular reactions involve simultaneous collision between two species.
D
Molecularity is only applicable for elementary reactions.

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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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For the reaction $2A + B \rightarrow \text{Product}$,the half-life remains unchanged when the concentration of $A$ is doubled. When the concentration of $B$ is doubled,the rate of reaction increases by a factor of $2$. What is the unit of the rate constant for this reaction?

Easy

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The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

DifficultJEE MAIN 2016

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The half-life of decomposition of gaseous $CH_3CHO$ at initial pressure of $364 \ mm$ and $182 \ mm$ of $Hg$ were $440 \ sec$ and $880 \ sec$ respectively. The order of the reaction is

Medium

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Select the rate law for the reaction $A + B \longrightarrow C$ based on the following data:

$Exp$ $[A]$ $[B]$ $Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

Difficult

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$A$ reaction is first order with respect to $A$ and second order with respect to $B$. How many times the rate of reaction is affected on increasing the concentration of $B$ three times?

EasyGSEB 2024

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$Exp$	$[A]$	$[B]$	$Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

Which of the following statements is incorrect?

Similar Questions

For the reaction $2A + B \rightarrow \text{Product}$,the half-life remains unchanged when the concentration of $A$ is doubled. When the concentration of $B$ is doubled,the rate of reaction increases by a factor of $2$. What is the unit of the rate constant for this reaction?

The rate law for the reaction below is given by the expression $Rate = k[A][B]$.$A + B \to \text{Product}$If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

The half-life of decomposition of gaseous $CH_3CHO$ at initial pressure of $364 \ mm$ and $182 \ mm$ of $Hg$ were $440 \ sec$ and $880 \ sec$ respectively. The order of the reaction is

Select the rate law for the reaction $A + B \longrightarrow C$ based on the following data: $Exp$ $[A]$ $[B]$ $Rate$ $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.070$ $0.80$ $3$ $0.024$ $0.035$ $0.10$ $4$ $0.012$ $0.070$ $0.80$

$A$ reaction is first order with respect to $A$ and second order with respect to $B$. How many times the rate of reaction is affected on increasing the concentration of $B$ three times?

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The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

Select the rate law for the reaction $A + B \longrightarrow C$ based on the following data:

$Exp$ $[A]$ $[B]$ $Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$