(A) For a first-order reaction,the rate constant is given by $k_1 = \frac{0.693}{t_{1/2}}$. Given $t_{1/2} = 40 \ s$,so $k_1 = \frac{0.693}{40} \ s^{-

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(A) For a first-order reaction,the rate constant is given by $k_1 = \frac{0.693}{t_{1/2}}$. Given $t_{1/2} = 40 \ s$,so $k_1 = \frac{0.693}{40} \ s^{-1}$.For a zero-order reaction,the rate constant is given by $k_0 = \frac{[A]_0}{2t_{1/2}}$. Given $[A]_0 = 1.386 \ mol \ m^{-3}$ and $t_{1/2} = 20 \ s$,so $k_0 = \frac{1.386}{2 \times 20} = \frac{1.386}{40} \ mol \ m^{-3} \ s^{-1}$.The ratio $\frac{k_1}{k_0} = \frac{0.693 / 40}{1.386 / 40} = \frac{0.693}{1.386} = 0.5 \ m^3 \ mol^{-1}$.

Class 12 Chemistry Chemical Kinetics Mix Examples-Chemical Kinetics

Medium

Under identical reaction conditions,the concentration of a substance is $1.386 \ mol \ m^{-3}$. It is halved in $40 \ s$ and $20 \ s$ by first-order and zero-order kinetics,respectively. The ratio of the rate constants for the first-order $(k_1)$ and zero-order $(k_0)$ reactions,$\left( \frac{k_1}{k_0} \right)$,is ............ $m^3 \ mol^{-1}$.

A
$0.5$
B
$1.0$
C
$1.5$
D
$2.0$

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Class 12

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Chemical Kinetics

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Mix Examples-Chemical Kinetics

The consecutive reaction $X$ $\longrightarrow Y$ $\longrightarrow Z$ takes place in a closed container. Initially,the container has $A_{0}$ moles of $X$ (and no $Y$ and $Z$). The plot of total moles of the constituents in the container as a function of time will be:

DifficultKVPY 2017

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$t_{100\%}$ is the time required for the $100\%$ completion of the reaction, while $t_{1/2}$ is the time required for $50\%$ of the reaction to be completed. Which of the following options correctly represents the relation between $t_{100\%}$ and $t_{1/2}$ for zero and first-order reactions, respectively?

MediumJEE MAIN 2026

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For a chemical reaction,the temperature is increased from $25\,^{\circ}C$ to $55\,^{\circ}C$. The rate of reaction will change by a factor of (Assume $\mu = 3$).

Medium

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The decomposition of $N_2O_5$ follows first-order kinetics: $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$. Its half-life is $2.4 \ hours$. If $10.8 \ g$ of $N_2O_5$ is taken initially,how many liters of $O_2$ will be obtained at $STP$ after $9.6 \ hours$?

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

DifficultIIT 1998

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The consecutive reaction $X$ $\longrightarrow Y$ $\longrightarrow Z$ takes place in a closed container. Initially,the container has $A_{0}$ moles of $X$ (and no $Y$ and $Z$). The plot of total moles of the constituents in the container as a function of time will be:

For a chemical reaction,the temperature is increased from $25\,^{\circ}C$ to $55\,^{\circ}C$. The rate of reaction will change by a factor of (Assume $\mu = 3$).

The decomposition of $N_2O_5$ follows first-order kinetics: $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$. Its half-life is $2.4 \ hours$. If $10.8 \ g$ of $N_2O_5$ is taken initially,how many liters of $O_2$ will be obtained at $STP$ after $9.6 \ hours$?

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

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