(A) For reaction $-I$: The rate law is $-\frac{d[A]}{dt} = k_1[A]^0$. Since the order is $0$,the unit of $k_1$ is $\text{concentration} \times \text{t

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(A) For reaction $-I$: The rate law is $-\frac{d[A]}{dt} = k_1[A]^0$. Since the order is $0$,the unit of $k_1$ is $\text{concentration} \times \text{time}^{-1} = M \ sec^{-1}$.For reaction $-II$: The rate law is $-\frac{d[B]}{dt} = k_2[B]^1$. Since the order is $1$,the unit of $k_2$ is $\text{time}^{-1} = sec^{-1}$.

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

Medium

Consider the following two reactions:
$A \to \text{Product}; -\frac{d[A]}{dt} = k_1[A]^0$
$B \to \text{Product}; -\frac{d[B]}{dt} = k_2[B]$
The units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as:

A
$M \ sec^{-1}, sec^{-1}$
B
$M \ sec^{-1}, M \ sec^{-1}$
C
$sec^{-1}, M^{-1} \ sec^{-1}$
D
$M \ sec^{-1}, M \ sec^{-1}$

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Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

Rate law , Rate constant , Order of Reaction and Molecularity

What is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$

Difficult

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The half-life of a reaction is found to be inversely proportional to the cube of its initial concentration. The order of the reaction is:

Easy

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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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For a reaction $A \rightarrow \text{Product}$,the rate constant is $6.93 \times 10^{-3} \ hour^{-1}$. What is the order of the reaction?

EasyMHT CET 2025

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For the reaction $2A + B \rightarrow \text{product}$,the rate of the reaction is $15 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$ when $[A] = 0.3 \ mol \ dm^{-3}$ and $[B] = 0.05 \ mol \ dm^{-3}$. What is the value of the rate constant if the reaction is first order in both the reactants?

MediumMHT CET 2022

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

Consider the following two reactions:$A \to \text{Product}; -\frac{d[A]}{dt} = k_1[A]^0$$B \to \text{Product}; -\frac{d[B]}{dt} = k_2[B]$The units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as:

Similar Questions

What is the molecularity of the following reactions?$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$

The half-life of a reaction is found to be inversely proportional to the cube of its initial concentration. The order of the reaction is:

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

For a reaction $A \rightarrow \text{Product}$,the rate constant is $6.93 \times 10^{-3} \ hour^{-1}$. What is the order of the reaction?

For the reaction $2A + B \rightarrow \text{product}$,the rate of the reaction is $15 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$ when $[A] = 0.3 \ mol \ dm^{-3}$ and $[B] = 0.05 \ mol \ dm^{-3}$. What is the value of the rate constant if the reaction is first order in both the reactants?

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Consider the following two reactions:
$A \to \text{Product}; -\frac{d[A]}{dt} = k_1[A]^0$
$B \to \text{Product}; -\frac{d[B]}{dt} = k_2[B]$
The units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as:

What is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$

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

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

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

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

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

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