(C) For a first order reaction,the rate law is given by $r = k[A]$.Given: $r = 2.0 \times 10^{-5} \ M \ sec^{-1}$ and $[A] = 0.01 \ M$.Substituting th

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(C) For a first order reaction,the rate law is given by $r = k[A]$.Given: $r = 2.0 \times 10^{-5} \ M \ sec^{-1}$ and $[A] = 0.01 \ M$.Substituting the values: $2.0 \times 10^{-5} = k \times 0.01$.$k = \frac{2.0 \times 10^{-5}}{10^{-2}} = 2.0 \times 10^{-3} \ sec^{-1}$.The half-life period $t_{1/2}$ for a first order reaction is $t_{1/2} = \frac{0.693}{k}$.$t_{1/2} = \frac{0.693}{2.0 \times 10^{-3}} = 0.3465 \times 10^3 = 346.5 \ sec$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

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
$333$
B
$300$
C
$346.5$
D
$220$

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Chemical Kinetics

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First Order reaction

$A$ first order reaction has a rate constant $1.15 \times 10^{-3} \, s^{-1}$. How long will $5 \, g$ of this reactant take to reduce to $3 \, g$?

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$A$ first order reaction takes $40 \ min$ for $30 \%$ decomposition. Calculate $t_{1/2}$.

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If the rate constant for a first order reaction is $2.303 \times 10^{-3} \ s^{-1}$,find the time required to reduce $4 \ g$ of the reactant to $0.2 \ g$. (in $hours$)

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The rate constant of a first-order reaction is $6 \ min^{-1}$. If the initial concentration of the reactant is $0.5 \ mol \ L^{-1}$,after how many minutes will the concentration of the reactant become $0.05 \ mol \ L^{-1}$?

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For a first order reaction,the rate constant is given as $\log_{10} K = 12 - \frac{6 \times 10^3}{T}$. What will be the value of temperature if its half-life period is $6.93 \times 10^{-3} \, \text{min}$ (in $, K$)?

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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 .......... $sec$.

Similar Questions

$A$ first order reaction has a rate constant $1.15 \times 10^{-3} \, s^{-1}$. How long will $5 \, g$ of this reactant take to reduce to $3 \, g$?

$A$ first order reaction takes $40 \ min$ for $30 \%$ decomposition. Calculate $t_{1/2}$.

If the rate constant for a first order reaction is $2.303 \times 10^{-3} \ s^{-1}$,find the time required to reduce $4 \ g$ of the reactant to $0.2 \ g$. (in $hours$)

The rate constant of a first-order reaction is $6 \ min^{-1}$. If the initial concentration of the reactant is $0.5 \ mol \ L^{-1}$,after how many minutes will the concentration of the reactant become $0.05 \ mol \ L^{-1}$?

For a first order reaction,the rate constant is given as $\log_{10} K = 12 - \frac{6 \times 10^3}{T}$. What will be the value of temperature if its half-life period is $6.93 \times 10^{-3} \, \text{min}$ (in $, K$)?

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