(C) For a first-order reaction,the rate constant $K$ is given by $K = \frac{0.693}{t_{1/2}}$.Given $t_{1/2} = 0.3010 \ min$,so $K = \frac{0.693}{0.301

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(C) For a first-order reaction,the rate constant $K$ is given by $K = \frac{0.693}{t_{1/2}}$.Given $t_{1/2} = 0.3010 \ min$,so $K = \frac{0.693}{0.3010} \approx 2.303 \ min^{-1}$.The integrated rate equation is $\ln \frac{[A]_0}{[A]_t} = Kt$,which can be written as $\log \frac{[A]_0}{[A]_t} = \frac{Kt}{2.303}$.Substituting the values: $\log \frac{[A]_0}{[A]_t} = \frac{2.303 \times 2.0}{2.303} = 2.0$.Therefore,$\frac{[A]_0}{[A]_t} = 10^2 = 100$.

Class 12 Chemistry Chemical Kinetics First Order reaction

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For the given first order reaction $A \rightarrow B$,the half-life of the reaction is $0.3010 \ min$. The ratio of the initial concentration of reactant to the concentration of reactant at time $2.0 \ min$ will be equal to $........$ (Nearest integer).

JEE MAIN 2022 All JEE MAIN

A
$110$
B
$112$
C
$100$
D
$113$

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Chemical Kinetics

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First Order reaction

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For the given first order reaction $A \rightarrow B$,the half-life of the reaction is $0.3010 \ min$. The ratio of the initial concentration of reactant to the concentration of reactant at time $2.0 \ min$ will be equal to $........$ (Nearest integer).

Similar Questions

In a first-order reaction of the type: $A_{(g)} \to 2B_{(g)}$,the initial pressure is $P_i$ and the total pressure at time $t$ is $P_t$. The rate constant $k$ can be expressed as:

After how many seconds will the concentration of the reactants in a first order reaction be halved,if the decay constant is $1.155 \times 10^{-3} \, \sec^{-1}$?

For a first-order reaction,which of the following statements is correct?

What is the half-life of a first-order reaction if the time required to decrease the concentration of the reactant from $0.8 \ mol \ dm^{-3}$ to $0.2 \ mol \ dm^{-3}$ is $12 \ hour$ (in $hour$)?

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