(B) For a first order reaction,the rate law is given by $r = k[A]$. Given the rate $r = 0.6932 \times 10^{-2} \, mol \, L^{-1} \, min^{-1}$ and initia

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(B) For a first order reaction,the rate law is given by $r = k[A]$. Given the rate $r = 0.6932 \times 10^{-2} \, mol \, L^{-1} \, min^{-1}$ and initial concentration $[A] = 1 \, M$. Calculating the rate constant $k$: $k = \frac{r}{[A]} = \frac{0.6932 \times 10^{-2} \, mol \, L^{-1} \, min^{-1}}{1 \, mol \, L^{-1}} = 0.6932 \times 10^{-2} \, min^{-1}$. For a first order reaction,the half-life $T_{1/2}$ is calculated as: $T_{1/2} = \frac{0.693}{k} = \frac{0.693}{0.6932 \times 10^{-2}} \approx 100 \, min$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

The rate for a first order reaction is $0.6932 \times 10^{-2} \, mol \, L^{-1} \, min^{-1}$ and the initial concentration of the reactants is $1 \, M$. The half-life $T_{1/2}$ is equal to ........ $min$.

A
$6.932$
B
$100$
C
$0.6932 \times 10^{-3}$
D
$0.6932 \times 10^{-2}$

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Chemical Kinetics

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First Order reaction

For a first-order reaction $A \rightarrow B$,the rate of reaction is $2.0 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$ when the concentration of the reactant is $0.01 \, M$. The half-life of the reaction is ........ seconds.

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The rate constant for a first order reaction is $60 \text{ s}^{-1}$. How much time (in seconds) will it take to reduce the initial concentration of the reactant to its $1/16^{th}$ value?

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For the first-order reaction $N_2O_5 \to 2NO_2 + \frac{1}{2}O_2$,the half-life at $30 \ ^\circ C$ is $24 \ \text{hours}$. Starting with $10 \ g$ of $N_2O_5$,how many grams of $N_2O_5$ will remain after $96 \ \text{hours}$ (in $g$)?

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Half-life of a first order reaction is $20 \ s$ and initial concentration of reactant is $0.2 \ M$. The concentration of reactant left after $80 \ s$ is (in $M$)

MediumKCET 2025

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Half life of a first order reaction is $20 \ min$. The time taken to reduce the initial concentration of reactant to $(1/10)^{th}$ is $\qquad$ (in $min$)

MediumMHT CET 2025

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The rate for a first order reaction is $0.6932 \times 10^{-2} \, mol \, L^{-1} \, min^{-1}$ and the initial concentration of the reactants is $1 \, M$. The half-life $T_{1/2}$ is equal to ........ $min$.

Similar Questions

For a first-order reaction $A \rightarrow B$,the rate of reaction is $2.0 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$ when the concentration of the reactant is $0.01 \, M$. The half-life of the reaction is ........ seconds.

The rate constant for a first order reaction is $60 \text{ s}^{-1}$. How much time (in seconds) will it take to reduce the initial concentration of the reactant to its $1/16^{th}$ value?

For the first-order reaction $N_2O_5 \to 2NO_2 + \frac{1}{2}O_2$,the half-life at $30 \ ^\circ C$ is $24 \ \text{hours}$. Starting with $10 \ g$ of $N_2O_5$,how many grams of $N_2O_5$ will remain after $96 \ \text{hours}$ (in $g$)?

Half-life of a first order reaction is $20 \ s$ and initial concentration of reactant is $0.2 \ M$. The concentration of reactant left after $80 \ s$ is (in $M$)

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