(A) The rate law for the reaction is given by $Rate = k[C_6H_5N_2^+Cl^-]^n$,where $n$ is the order of the reaction.Given that when the initial concent

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(A) The rate law for the reaction is given by $Rate = k[C_6H_5N_2^+Cl^-]^n$,where $n$ is the order of the reaction.Given that when the initial concentration is doubled,the rate of evolution of $N_2$ (which is the rate of reaction) becomes two times faster.Let the initial rate be $R_1 = k[C]^n$ and the new rate be $R_2 = k[2C]^n$.According to the problem,$R_2 = 2R_1$.Therefore,$k[2C]^n = 2 \times k[C]^n$.$2^n = 2^1$.Thus,$n = 1$.Hence,it is a first order reaction.

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

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The diazonium salt decomposes as $C_6H_5N_2^+Cl^- \to C_6H_5Cl + N_2$. At $0 \ ^\circ C$,the evolution of $N_2$ becomes two times faster when the initial concentration of the salt is doubled. Therefore,it is:

A
$A$. $A$ first order reaction
B
$B$. $A$ second order reaction
C
$C$. Independent of the initial concentration of the salt
D
$D$. $A$ zero order reaction

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

For a reaction $2 \ A + B \rightarrow P$,when the concentration of $B$ alone is doubled,the rate does not change,and when the concentrations of both $A$ and $B$ are doubled,the rate increases by a factor of $4$. The unit of the rate constant is,

DifficultWBJEE 2020

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The rate constant for a second order reaction is $8 \times 10^{-5} \ M^{-1} \ min^{-1}$. How long will it take a $1 \ M$ solution to be reduced to $0.5 \ M$?

Medium

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Rate law for the reaction,$C_2H_5I_{(g)} \rightarrow C_2H_{4_{(g)}} + HI_{(g)}$ is $r = k[C_2H_5I]$. What is the order and molecularity of this reaction?

EasyMHT CET 2025

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The rate constant of esterification is given by $k = k^{\prime} [H_2O]$. If the rate constant $k = 2.0 \times 10^{-3} \ min^{-1}$,calculate $k^{\prime}$. (Assume $[H_2O] = 55.5 \ mol \ L^{-1}$)

Medium

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The rate equation for the reaction $2 A + B \longrightarrow$ products is $\text{rate} = k[A][B]^2$. If $k$ at $T \ K$ is $5.0 \times 10^{-6} \ mol^{-2} \ L^2 \ s^{-1}$,the initial rate of the reaction,when $[A] = 0.05 \ mol \ L^{-1}$ and $[B] = 0.1 \ mol \ L^{-1}$ is:

DifficultAP EAMCET 2022

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The diazonium salt decomposes as $C_6H_5N_2^+Cl^- \to C_6H_5Cl + N_2$. At $0 \ ^\circ C$,the evolution of $N_2$ becomes two times faster when the initial concentration of the salt is doubled. Therefore,it is:

Similar Questions

For a reaction $2 \ A + B \rightarrow P$,when the concentration of $B$ alone is doubled,the rate does not change,and when the concentrations of both $A$ and $B$ are doubled,the rate increases by a factor of $4$. The unit of the rate constant is,

The rate constant for a second order reaction is $8 \times 10^{-5} \ M^{-1} \ min^{-1}$. How long will it take a $1 \ M$ solution to be reduced to $0.5 \ M$?

Rate law for the reaction,$C_2H_5I_{(g)} \rightarrow C_2H_{4_{(g)}} + HI_{(g)}$ is $r = k[C_2H_5I]$. What is the order and molecularity of this reaction?

The rate constant of esterification is given by $k = k^{\prime} [H_2O]$. If the rate constant $k = 2.0 \times 10^{-3} \ min^{-1}$,calculate $k^{\prime}$. (Assume $[H_2O] = 55.5 \ mol \ L^{-1}$)

The rate equation for the reaction $2 A + B \longrightarrow$ products is $\text{rate} = k[A][B]^2$. If $k$ at $T \ K$ is $5.0 \times 10^{-6} \ mol^{-2} \ L^2 \ s^{-1}$,the initial rate of the reaction,when $[A] = 0.05 \ mol \ L^{-1}$ and $[B] = 0.1 \ mol \ L^{-1}$ is:

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