(A) For a first order reaction,the rate constant $k$ is given by the formula:$k = \frac{2.303}{t} \log \frac{[A]_0}{[A]}$Given values are:$t = 5 \ min

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(A) For a first order reaction,the rate constant $k$ is given by the formula:$k = \frac{2.303}{t} \log \frac{[A]_0}{[A]}$Given values are:$t = 5 \ min$$[A]_0 = 0.6 \ mol \ L^{-1}$$[A] = 0.2 \ mol \ L^{-1}$Substituting the values in the formula:$k = \frac{2.303}{5} \log \frac{0.6}{0.2}$$k = \frac{2.303}{5} \log 3$Using $\log 3 = 0.4771$:$k = \frac{2.303 \times 0.4771}{5}$$k = \frac{1.0988}{5} = 0.21976 \ min^{-1} \approx 0.219 \ min^{-1}$

Class 12 Chemistry Chemical Kinetics First Order reaction

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In a first order reaction,the concentration of the reactant is reduced from $0.6 \ mol \ L^{-1}$ to $0.2 \ mol \ L^{-1}$ in $5 \ min$. What is the rate constant of the reaction (in $min^{-1}$)? $(\log 3 = 0.4771)$

AP EAMCET 2012 All AP EAMCET

A
$0.219$
B
$0.325$
C
$0.421$
D
$0.522$

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Chemical Kinetics

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First Order reaction

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The rate of a first-order reaction is $1.5 \times 10^{-2} \, mol \, L^{-1} \, min^{-1}$ when the concentration of the reactant is $0.5 \, M$. Find the half-life $(t_{1/2})$ of the reaction in $min$.

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Thermal decomposition of a compound is of first order. If $50\%$ of a sample of this compound is decomposed in $120 \ min$,then how long will it take $90\%$ of the compound to decompose? ........ $min.$

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For the reaction $2A + B \to \text{Product}$,the rate law is given as $\frac{-d[A]}{dt} = K[A]$. At a time when $t = \frac{1}{K}$,the concentration of the reactant $A$ is ($Co =$ initial concentration).

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The half-life period of a first order reaction is $100 \, \text{sec}$. The rate constant of the reaction is

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In a first order reaction,the concentration of the reactant is reduced from $0.6 \ mol \ L^{-1}$ to $0.2 \ mol \ L^{-1}$ in $5 \ min$. What is the rate constant of the reaction (in $min^{-1}$)? $(\log 3 = 0.4771)$

Similar Questions

The rate of a first-order reaction is $1.5 \times 10^{-2} \, mol \, L^{-1} \, min^{-1}$ when the concentration of the reactant is $0.5 \, M$. Find the half-life $(t_{1/2})$ of the reaction in $min$.

Thermal decomposition of a compound is of first order. If $50\%$ of a sample of this compound is decomposed in $120 \ min$,then how long will it take $90\%$ of the compound to decompose? ........ $min.$

$A$ first order reaction requires $30 \ min$ for $50\%$ completion. The time required to complete the reaction by $75\%$ will be .......... $\min.$

For the reaction $2A + B \to \text{Product}$,the rate law is given as $\frac{-d[A]}{dt} = K[A]$. At a time when $t = \frac{1}{K}$,the concentration of the reactant $A$ is ($Co =$ initial concentration).

The half-life period of a first order reaction is $100 \, \text{sec}$. The rate constant of the reaction is

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