(C) For the reaction $AB_5 \to AB + 4B$,the rate of reaction is given by:$Rate = -\frac{d[AB_5]}{dt} = \frac{1}{4} \frac{d[B]}{dt}$Given that $-\frac{

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(C) For the reaction $AB_5 \to AB + 4B$,the rate of reaction is given by:$Rate = -\frac{d[AB_5]}{dt} = \frac{1}{4} \frac{d[B]}{dt}$Given that $-\frac{d[AB_5]}{dt} = K[AB_5]$ and $\frac{d[B]}{dt} = K_1[AB_5]$,we substitute these into the rate expression:$K[AB_5] = \frac{1}{4} (K_1[AB_5])$Dividing both sides by $[AB_5]$,we get:$K = \frac{1}{4} K_1 \Rightarrow K_1 = 4K$

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

Medium

For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:
$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$
What is the correct relation between $K$ and $K_1$?

A
$K_1 = K$
B
$K_1 = 2K$
C
$K_1 = 4K$
D
$2K_1 = K$

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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

For the reaction,$CH_3Br_{(aq)} + OH_{(aq)}^{-} \rightarrow CH_3OH_{(aq)} + Br_{(aq)}^{-}$,the rate law is $\text{rate} = k[CH_3Br][OH^{-}]$. What is the change in the rate of reaction if the concentration of both reactants is doubled?

MediumMHT CET 2023

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The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows:
$P_0 \text{ (mmHg)}$ $250$ $300$
$t_{1/2} \text{ (minutes)}$ $135$ $112.5$

The order of reaction is -

Medium

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Units of rate constant of first and zero order reactions in terms of molarity $M$ unit are respectively

EasyAIEEE 2002

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The following results have been obtained during the kinetic studies of the reaction: $2 \ NO + 2 \ H_2 \longrightarrow N_2 + 2 \ H_2O$
Expt $\frac{-d[NO]}{dt} \ (mol \ L^{-1} \ s^{-1})$ $[NO] \ (mol \ L^{-1})$ $[H_2] \ (mol \ L^{-1})$
$1$ $4.8 \times 10^{-5}$ $1 \times 10^{-2}$ $1 \times 10^{-3}$
$2$ $43.2 \times 10^{-5}$ $3 \times 10^{-2}$ $1 \times 10^{-3}$
$3$ $86.4 \times 10^{-5}$ $3 \times 10^{-2}$ $2 \times 10^{-3}$

MediumTS EAMCET 2019

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Which one of the following statements is wrong?

Easy

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$P_0 \text{ (mmHg)}$	$250$	$300$
$t_{1/2} \text{ (minutes)}$	$135$	$112.5$

Expt	$\frac{-d[NO]}{dt} \ (mol \ L^{-1} \ s^{-1})$	$[NO] \ (mol \ L^{-1})$	$[H_2] \ (mol \ L^{-1})$
$1$	$4.8 \times 10^{-5}$	$1 \times 10^{-2}$	$1 \times 10^{-3}$
$2$	$43.2 \times 10^{-5}$	$3 \times 10^{-2}$	$1 \times 10^{-3}$
$3$	$86.4 \times 10^{-5}$	$3 \times 10^{-2}$	$2 \times 10^{-3}$

For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$What is the correct relation between $K$ and $K_1$?

Similar Questions

For the reaction,$CH_3Br_{(aq)} + OH_{(aq)}^{-} \rightarrow CH_3OH_{(aq)} + Br_{(aq)}^{-}$,the rate law is $\text{rate} = k[CH_3Br][OH^{-}]$. What is the change in the rate of reaction if the concentration of both reactants is doubled?

The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows: $P_0 \text{ (mmHg)}$$250$$300$$t_{1/2} \text{ (minutes)}$$135$$112.5$The order of reaction is -

Units of rate constant of first and zero order reactions in terms of molarity $M$ unit are respectively

Which one of the following statements is wrong?

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For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:
$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$
What is the correct relation between $K$ and $K_1$?

The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows:
$P_0 \text{ (mmHg)}$ $250$ $300$
$t_{1/2} \text{ (minutes)}$ $135$ $112.5$

The order of reaction is -