(C) For a reaction,the rate law is given by: $\text{Rate} = k[\text{conc.}]^n$,where $n$ is the order of the reaction.Taking logarithm on both sides:$

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(C) For a reaction,the rate law is given by: $\text{Rate} = k[\text{conc.}]^n$,where $n$ is the order of the reaction.Taking logarithm on both sides:$\log(\text{rate}) = \log(k) + n \log[\text{conc.}]$This equation is of the form $y = mx + c$,where the slope $m$ is equal to the order of the reaction $n$.Comparing the slopes of the lines in the graph:The slope of line $D$ is the steepest,followed by $B$,then $A$,and finally $C$ is the least steep.Therefore,the order of the reactions follows the sequence: $d > b > a > c$.

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

Medium

Consider the following reactions:
$A$ $\rightarrow P_1; B$ $\rightarrow P_2; C$ $\rightarrow P_3; D$ $\rightarrow P_4$
The orders of the above reactions are $a, b, c,$ and $d,$ respectively. The following graph is obtained when $\log[\text{rate}]$ vs. $\log[\text{conc.}]$ are plotted:
Among the following,the correct sequence for the order of the reactions is:

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A
$a > b > c > d$
B
$c > a > b > d$
C
$d > b > a > c$
D
$d > a > b > c$

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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 a reaction,$A + B \rightarrow \text{Product}$; the rate law is given by,$r = k[A]^{1/2}[B]^2$. What is the order of the reaction?

Medium

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For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?

Difficult

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Which of the following is a unimolecular reaction?

Easy

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The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3.0 \times 10^{-4} \ s^{-1}$. If the reaction starts with $1.0 \ mol \ L^{-1}$ of $N_2O_5$,calculate the rate of formation of $NO_2$ at the moment when the concentration of $O_2$ is $0.1 \ mol \ L^{-1}$.

MediumAIIMS 2011

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For conversion of compound $A \rightarrow B$,the rate constant of the reaction was found to be $4.6 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$. The order of the reaction is $..........$

MediumJEE MAIN 2023

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For a reaction,$A + B \rightarrow \text{Product}$; the rate law is given by,$r = k[A]^{1/2}[B]^2$. What is the order of the reaction?

For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,$\frac{d[O_2]}{dt} = K_3[N_2O_5]$What is the relationship between $K_1$,$K_2$,and $K_3$?

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The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3.0 \times 10^{-4} \ s^{-1}$. If the reaction starts with $1.0 \ mol \ L^{-1}$ of $N_2O_5$,calculate the rate of formation of $NO_2$ at the moment when the concentration of $O_2$ is $0.1 \ mol \ L^{-1}$.

For conversion of compound $A \rightarrow B$,the rate constant of the reaction was found to be $4.6 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$. The order of the reaction is $..........$

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For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?