(A) For a $1^{st}$ order reaction,the rate constant $k$ is given by $k = \frac{0.693}{t_{1/2}}$.Thus,the half-life $t_{1/2} = \frac{0.693}{k}$.Since $

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Independent of the initial concentration of the reactant

(A) For a $1^{st}$ order reaction,the rate constant $k$ is given by $k = \frac{0.693}{t_{1/2}}$.Thus,the half-life $t_{1/2} = \frac{0.693}{k}$.Since $k$ is a constant,$t_{1/2}$ is independent of the initial concentration of the reactant $[R]_0$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Easy

The half-life of a first-order reaction is

A
Independent of the initial concentration of the reactant
B
Directly proportional to the initial concentration of the reactants
C
Inversely proportional to the initial concentration of the reactant
D
Directly proportional to the square of the initial concentration of the reactant

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Class 12 Questions

Class 12

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Chemical Kinetics

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First Order reaction

In a first order reaction,$60 \%$ of the reactant converts into product in $45 \ minutes$. Calculate the rate constant of the reaction.

EasyMHT CET 2024

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$A$ reaction that is of the first order with respect to reactant $A$ has a rate constant $6 \ min^{-1}$. If we start with $[A] = 0.5 \ mol \ L^{-1}$,when would $[A]$ reach the value $0.05 \ mol \ L^{-1}$? (in $min$)

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In a first order reaction,$60 \%$ of the reactant decomposes in $4.606 \ min$. What is the half-life of the reaction (in $min$)? (Given: $k = 0.1989 \ min^{-1}$)

MediumMHT CET 2021

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For a reaction,$r = k[A]$. If $50 \%$ of $A$ is decomposed in $120 \ \text{minutes}$,the time taken for $90 \%$ decomposition of $A$ is $............ \ \text{minutes}$.

DifficultJEE MAIN 2024

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The reaction $X \rightarrow$ products is a first-order reaction. If the concentration of reactant $X$ decreases from $0.1 \, M$ to $0.025 \, M$ in $40 \, \text{minutes}$,what will be the rate of the reaction when the concentration of the reactant is $0.01 \, M$?

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The half-life of a first-order reaction is

Similar Questions

In a first order reaction,$60 \%$ of the reactant converts into product in $45 \ minutes$. Calculate the rate constant of the reaction.

$A$ reaction that is of the first order with respect to reactant $A$ has a rate constant $6 \ min^{-1}$. If we start with $[A] = 0.5 \ mol \ L^{-1}$,when would $[A]$ reach the value $0.05 \ mol \ L^{-1}$? (in $min$)

In a first order reaction,$60 \%$ of the reactant decomposes in $4.606 \ min$. What is the half-life of the reaction (in $min$)? (Given: $k = 0.1989 \ min^{-1}$)

For a reaction,$r = k[A]$. If $50 \%$ of $A$ is decomposed in $120 \ \text{minutes}$,the time taken for $90 \%$ decomposition of $A$ is $............ \ \text{minutes}$.

The reaction $X \rightarrow$ products is a first-order reaction. If the concentration of reactant $X$ decreases from $0.1 \, M$ to $0.025 \, M$ in $40 \, \text{minutes}$,what will be the rate of the reaction when the concentration of the reactant is $0.01 \, M$?

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