(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 an elementary reaction,$2A + B \to C + D$,the molecularity is:

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

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Consider the plots,given below,for the reaction $A \rightarrow B + C$. The plots respectively correspond to the reaction order:

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For a reaction $X + Y \to Z$,the rate is given by $\text{rate} \propto [X]$. What are $(i)$ the molecularity and $(ii)$ the order of the reaction?

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The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are:

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For an elementary reaction,$2A + B \to C + D$,the molecularity is:

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

Consider the plots,given below,for the reaction $A \rightarrow B + C$. The plots respectively correspond to the reaction order:

For a reaction $X + Y \to Z$,the rate is given by $\text{rate} \propto [X]$. What are $(i)$ the molecularity and $(ii)$ the order of the reaction?

The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$The relationship between $k$ and $k'$ and between $k$ and $k''$ are:

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The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are: