(B) For a first-order reaction,the half-life is given by $t_{1/2} = \frac{0.693}{K}$.Given $t_{1/2} = 10 \text{ minutes}$,the rate constant $K = \frac

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(B) For a first-order reaction,the half-life is given by $t_{1/2} = \frac{0.693}{K}$.Given $t_{1/2} = 10 \text{ minutes}$,the rate constant $K = \frac{0.693}{10} = 0.0693 \text{ min}^{-1}$.The integrated rate law for a first-order reaction is $t = \frac{2.303}{K} \log \frac{[A]_0}{[A]}$.Here,$[A] = 10 \% [A]_0 = 0.1 [A]_0$,so $\frac{[A]_0}{[A]} = 10$.Substituting the values: $t = \frac{2.303}{0.0693} \log(10) = \frac{2.303}{0.0693} \times 1 \approx 33.2 \text{ minutes}$.

Class 12 Chemistry Chemical Kinetics First Order reaction

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For an elementary reaction,$X_{(g)} \rightarrow Y_{(g)} + Z_{(g)}$,the $t_{1/2}$ is $10 \text{ minutes}$. In what period of time would the concentration of $X$ be reduced to $10 \%$ of its original concentration?

AP EAMCET 2003 All AP EAMCET

A
$20 \text{ minutes}$
B
$33.2 \text{ minutes}$
C
$15 \text{ minutes}$
D
$25.2 \text{ minutes}$

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Chemical Kinetics

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First Order reaction

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AP EAMCET 2003 Paper All AP EAMCET years →

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MediumAP EAMCET 2023

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For an elementary reaction,$X_{(g)} \rightarrow Y_{(g)} + Z_{(g)}$,the $t_{1/2}$ is $10 \text{ minutes}$. In what period of time would the concentration of $X$ be reduced to $10 \%$ of its original concentration?

Similar Questions

The rate constant of the reaction $2 NO_2Cl_{(g)} \longrightarrow 2 NO_{2(g)} + Cl_{2(g)}$ is $4.7672 \text{ minute}^{-1}$. Calculate the half-life of the reaction.

For a first order reaction $A \to B$,the reaction rate at reactant concentration of $0.01 \ M$ is found to be $2.0 \times 10^{-5} \ M \ sec^{-1}$. The half-life period of the reaction is .......... $sec$.

$A$ first order reaction is half completed in $45 \ min$. How long does it need $99.9 \%$ of the reaction to be completed (in $Hours$)?

The half-life of a first-order reaction is $69.35 \, \text{sec}$. The value of the rate constant of the reaction is .......... $\sec^{-1}$.

For a first order reaction,the concentration of reactant was reduced from $0.03 \ mol \ L^{-1}$ to $0.02 \ mol \ L^{-1}$ in $25 \ min$. What is its rate (in $mol \ L^{-1} \ s^{-1}$)?

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