(B) For a reaction of order $n$,the half-life $t_{1/2}$ is related to the initial pressure $P_0$ as $t_{1/2} \propto (P_0)^{1-n}$.Using the data from

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(B) For a reaction of order $n$,the half-life $t_{1/2}$ is related to the initial pressure $P_0$ as $t_{1/2} \propto (P_0)^{1-n}$.Using the data from the table:$\frac{(t_{1/2})_1}{(t_{1/2})_2} = \left(\frac{(P_0)_1}{(P_0)_2}\right)^{1-n}$Substituting the values for the first two entries:$\frac{4}{2} = \left(\frac{50}{100}\right)^{1-n}$$2 = \left(\frac{1}{2}\right)^{1-n}$$2 = (2)^{-(1-n)}$$2^1 = 2^{n-1}$Equating the exponents:$1 = n - 1$$n = 2$Therefore,the order of the reaction is $2$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

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$A$ student has studied the decomposition of a gas $AB_3$ at $25^{\circ} C$. He obtained the following data.

$p \ (mm \ Hg)$ $50$ $100$ $200$ $400$

Relative $t_{1/2} \ (s)$ $4$ $2$ $1$ $0.5$

The order of the reaction is

JEE MAIN 2023 All JEE MAIN

A
$0.5$
B
$2$
C
$1$
D
$0$

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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Consider the plots for the types of reaction $nA \to B + C$. These plots respectively correspond to the reaction orders:

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For the following reaction: $NO_{2(g)} + CO_{(g)} \to NO_{(g)} + CO_{2(g)}$,the rate law is: $\text{Rate} = k [NO_2]^2$. If $0.1 \ mol$ of gaseous carbon monoxide is added at constant temperature to the reaction mixture,which of the following statements is true?

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For a second-order reaction where the initial concentrations of both reactants are equal,it takes $3000 \ s$ for the reaction to be $60\%$ complete. How much time (in $s$) will it take for the reaction to be $20\%$ complete?

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For the reaction $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$,the experimental data suggests the rate law is $\text{Rate} = K[H_2][Br_2]^{1/2}$. Find the order of the reaction and its molecularity.

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The rate law for the reaction $\text{Sucrose} + \text{Water} \xrightarrow{H^+} \text{Glucose} + \text{Fructose}$ is given by:

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$p \ (mm \ Hg)$	$50$	$100$	$200$	$400$
Relative $t_{1/2} \ (s)$	$4$	$2$	$1$	$0.5$

$A$ student has studied the decomposition of a gas $AB_3$ at $25^{\circ} C$. He obtained the following data. $p \ (mm \ Hg)$ $50$ $100$ $200$ $400$ Relative $t_{1/2} \ (s)$ $4$ $2$ $1$ $0.5$ The order of the reaction is

Similar Questions

Consider the plots for the types of reaction $nA \to B + C$. These plots respectively correspond to the reaction orders:

For the following reaction: $NO_{2(g)} + CO_{(g)} \to NO_{(g)} + CO_{2(g)}$,the rate law is: $\text{Rate} = k [NO_2]^2$. If $0.1 \ mol$ of gaseous carbon monoxide is added at constant temperature to the reaction mixture,which of the following statements is true?

For a second-order reaction where the initial concentrations of both reactants are equal,it takes $3000 \ s$ for the reaction to be $60\%$ complete. How much time (in $s$) will it take for the reaction to be $20\%$ complete?

For the reaction $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$,the experimental data suggests the rate law is $\text{Rate} = K[H_2][Br_2]^{1/2}$. Find the order of the reaction and its molecularity.

The rate law for the reaction $\text{Sucrose} + \text{Water} \xrightarrow{H^+} \text{Glucose} + \text{Fructose}$ is given by:

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$A$ student has studied the decomposition of a gas $AB_3$ at $25^{\circ} C$. He obtained the following data.

$p \ (mm \ Hg)$ $50$ $100$ $200$ $400$

Relative $t_{1/2} \ (s)$ $4$ $2$ $1$ $0.5$

The order of the reaction is