(D) For a first-order reaction,the rate law is given by $r = k[A]$.Given $r = 1 \times 10^{-2} \, \text{mol L}^{-1} \text{min}^{-1}$ and $[A] = 0.2 \,

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(D) For a first-order reaction,the rate law is given by $r = k[A]$.Given $r = 1 \times 10^{-2} \, \text{mol L}^{-1} \text{min}^{-1}$ and $[A] = 0.2 \, \text{M}$.Substituting the values: $1 \times 10^{-2} = k \times 0.2$.$k = \frac{1 \times 10^{-2}}{0.2} = 5 \times 10^{-2} \, \text{min}^{-1}$.The half-life $t_{1/2}$ is calculated as $t_{1/2} = \frac{0.693}{k}$.$t_{1/2} = \frac{0.693}{5 \times 10^{-2}} = \frac{69.3}{5} = 13.86 \, \text{min} \approx 14 \, \text{min}$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

For a first-order reaction $A \rightarrow \text{Product}$,the rate of reaction is $1 \times 10^{-2} \, \text{mol L}^{-1} \text{min}^{-1}$ when $[A] = 0.2 \, \text{M}$. What is the half-life $(t_{1/2})$ of the reaction?

A
$832 \, \text{min}$
B
$440 \, \text{sec}$
C
$416 \, \text{min}$
D
$14 \, \text{min}$

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Chemical Kinetics

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First Order reaction

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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$A \rightarrow$ products is a first-order reaction. The following data is obtained for this reaction at $T \ K$. The value of $x : y$ is:
Rate $(\text{mol } L^{-1} \ \text{min}^{-1})$ $[A]$
$0.2$ $0.02 \ M$
$0.4$ $x \ M$
$1.0$ $y \ M$

Rate $(\text{mol } L^{-1} \ \text{min}^{-1})$	$[A]$
$0.2$	$0.02 \ M$
$0.4$	$x \ M$
$1.0$	$y \ M$

MediumAP EAMCET 2025

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Rate of a first order reaction is $1.5 \times 10^{-2} \ mol \ L^{-1} \ minute^{-1}$ at $0.5 \ M$ concentration of reactant,calculate half life of reaction.

DifficultMHT CET 2024

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For a $1^{st}$ order reaction $R \rightarrow P$, the concentration of reactant $R$ changes from $0.1 \text{ M}$ to $0.025 \text{ M}$ in $40 \text{ minutes}$. The rate of reaction when the concentration of $R$ is $0.01 \text{ M}$ is

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The half-life for the reaction $N_2O_5 \rightleftharpoons 2NO_2 + \frac{1}{2}O_2$ is $24 \ hr$ at $30 \ ^\circ C$. Starting with $10 \ g$ of $N_2O_5$,how many grams of $N_2O_5$ will remain after a period of $96 \ hr$?

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For a first-order reaction $A \rightarrow \text{Product}$,the rate of reaction is $1 \times 10^{-2} \, \text{mol L}^{-1} \text{min}^{-1}$ when $[A] = 0.2 \, \text{M}$. What is the half-life $(t_{1/2})$ of the reaction?

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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 $0.01 \, M$?

$A \rightarrow$ products is a first-order reaction. The following data is obtained for this reaction at $T \ K$. The value of $x : y$ is:Rate $(\text{mol } L^{-1} \ \text{min}^{-1})$$[A]$$0.2$$0.02 \ M$$0.4$$x \ M$$1.0$$y \ M$

Rate of a first order reaction is $1.5 \times 10^{-2} \ mol \ L^{-1} \ minute^{-1}$ at $0.5 \ M$ concentration of reactant,calculate half life of reaction.

For a $1^{st}$ order reaction $R \rightarrow P$, the concentration of reactant $R$ changes from $0.1 \text{ M}$ to $0.025 \text{ M}$ in $40 \text{ minutes}$. The rate of reaction when the concentration of $R$ is $0.01 \text{ M}$ is

The half-life for the reaction $N_2O_5 \rightleftharpoons 2NO_2 + \frac{1}{2}O_2$ is $24 \ hr$ at $30 \ ^\circ C$. Starting with $10 \ g$ of $N_2O_5$,how many grams of $N_2O_5$ will remain after a period of $96 \ hr$?

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$A \rightarrow$ products is a first-order reaction. The following data is obtained for this reaction at $T \ K$. The value of $x : y$ is:
Rate $(\text{mol } L^{-1} \ \text{min}^{-1})$ $[A]$
$0.2$ $0.02 \ M$
$0.4$ $x \ M$
$1.0$ $y \ M$