(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

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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?

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

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First Order reaction

If the rate law is $r = K[A]$,then the concentration of the reactant remaining after time $t = 1/k$ is: ($[A]_0$ is the concentration of the reactant at $t = 0$)

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The half-life of a first order reaction is $30 \, min$. The time required for $75 \, \%$ completion of the same reaction will be $..... \, min$

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$R \rightarrow P$ is a first order reaction. For this reaction,a graph of $\ln [R]$ (on $y$-axis) and time (on $x$-axis) gives a straight line with a negative slope. The intercept on the $y$-axis is equal to ($k =$ rate constant):

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If the concentration of a first order reaction is increased by $x$ times,then the rate constant $(k)$ becomes

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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?

Similar Questions

If the rate law is $r = K[A]$,then the concentration of the reactant remaining after time $t = 1/k$ is: ($[A]_0$ is the concentration of the reactant at $t = 0$)

The rate constant $k = 2.303 \ min^{-1}$ for a particular reaction,and the initial concentration of the reactant is $1 \ mol/L$. What is the rate of reaction after $1 \ minute$?

The half-life of a first order reaction is $30 \, min$. The time required for $75 \, \%$ completion of the same reaction will be $..... \, min$

$R \rightarrow P$ is a first order reaction. For this reaction,a graph of $\ln [R]$ (on $y$-axis) and time (on $x$-axis) gives a straight line with a negative slope. The intercept on the $y$-axis is equal to ($k =$ rate constant):

If the concentration of a first order reaction is increased by $x$ times,then the rate constant $(k)$ becomes

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