(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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The half-life of decomposition of gaseous $CH_3CHO$ at initial pressure of $364 \ mm$ and $182 \ mm$ of $Hg$ were $440 \ sec$ and $880 \ sec$ respectively. The order of the reaction is

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For a certain reaction $A_{(g)} \to B_{(g)}$,the half-life for different initial pressures of $A$ is given below:
$P_{A_0} \text{ (atm)}$ $0.1$ $0.025$
$t_{1/2} \text{ (sec)}$ $100$ $50$

The correct statement about the order of reaction is:

Medium

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The rate law for a reaction between the substances $A$ and $B$ is given by,$rate = k[A]^n[B]^m$. On doubling the concentration of $A$ and halving the concentration of $B$,the ratio of the new rate to the earlier rate of the reaction will be as

MediumAIEEE 2003

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The rate constant for the reaction $A \longrightarrow B$ is $2 \times 10^{-4} \ L \ mol^{-1} \ min^{-1}$. The concentration of $A$ at which the rate of the reaction is $(1 / 12) \times 10^{-5} \ M \ sec^{-1}$ is :-

Medium

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The rate of reaction,$A + B + C \longrightarrow P$ is given by
$r = K[A]^{1/2} [B]^{1/2} [C]^{1/4}$
The order of reaction is

Medium

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

$P_{A_0} \text{ (atm)}$	$0.1$	$0.025$
$t_{1/2} \text{ (sec)}$	$100$	$50$

$A$ 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

The half-life of decomposition of gaseous $CH_3CHO$ at initial pressure of $364 \ mm$ and $182 \ mm$ of $Hg$ were $440 \ sec$ and $880 \ sec$ respectively. The order of the reaction is

For a certain reaction $A_{(g)} \to B_{(g)}$,the half-life for different initial pressures of $A$ is given below:$P_{A_0} \text{ (atm)}$$0.1$$0.025$$t_{1/2} \text{ (sec)}$$100$$50$The correct statement about the order of reaction is:

The rate law for a reaction between the substances $A$ and $B$ is given by,$rate = k[A]^n[B]^m$. On doubling the concentration of $A$ and halving the concentration of $B$,the ratio of the new rate to the earlier rate of the reaction will be as

The rate constant for the reaction $A \longrightarrow B$ is $2 \times 10^{-4} \ L \ mol^{-1} \ min^{-1}$. The concentration of $A$ at which the rate of the reaction is $(1 / 12) \times 10^{-5} \ M \ sec^{-1}$ is :-

The rate of reaction,$A + B + C \longrightarrow P$ is given by$r = K[A]^{1/2} [B]^{1/2} [C]^{1/4}$The order of reaction is

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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

For a certain reaction $A_{(g)} \to B_{(g)}$,the half-life for different initial pressures of $A$ is given below:
$P_{A_0} \text{ (atm)}$ $0.1$ $0.025$
$t_{1/2} \text{ (sec)}$ $100$ $50$

The correct statement about the order of reaction is:

The rate of reaction,$A + B + C \longrightarrow P$ is given by
$r = K[A]^{1/2} [B]^{1/2} [C]^{1/4}$
The order of reaction is