(D) The rate law for the reaction is given by: $Rate = k[AB]^n$. Using the data from the table: $2.75 \times 10^{-8} = k(0.20)^n$ --- $(i)$ $11.0 \ti

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(D) The rate law for the reaction is given by: $Rate = k[AB]^n$. Using the data from the table: $2.75 \times 10^{-8} = k(0.20)^n$ --- $(i)$ $11.0 \times 10^{-8} = k(0.40)^n$ --- $(ii)$ Dividing equation $(ii)$ by equation $(i)$: $\frac{11.0 \times 10^{-8}}{2.75 \times 10^{-8}} = (\frac{0.40}{0.20})^n$ $4 = 2^n$ Since $4 = 2^2$,we have $2^2 = 2^n$. Therefore,$n = 2$. The reaction is of second order.

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

Difficult

For the decomposition of a compound $AB$ at $600 \ K$,the following data were obtained:
$[AB] \ (mol \ dm^{-3})$ Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$
$0.20$ $2.75 \times 10^{-8}$
$0.40$ $11.0 \times 10^{-8}$
$0.60$ $24.75 \times 10^{-8}$

The order for the decomposition of $AB$ is:

KCET 2009 All KCET

A
$1.5$
B
$0$
C
$1$
D
$2$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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$[AB] \ (mol \ dm^{-3})$	Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$
$0.20$	$2.75 \times 10^{-8}$
$0.40$	$11.0 \times 10^{-8}$
$0.60$	$24.75 \times 10^{-8}$

For the decomposition of a compound $AB$ at $600 \ K$,the following data were obtained: $[AB] \ (mol \ dm^{-3})$Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$$0.20$$2.75 \times 10^{-8}$$0.40$$11.0 \times 10^{-8}$$0.60$$24.75 \times 10^{-8}$ The order for the decomposition of $AB$ is:

Similar Questions

The rate law for the reaction $RCl + NaOH_{(aq)} \to ROH + NaCl$ is given by $\text{Rate} = K_1[RCl]$. The rate of the reaction will be

Assertion : In rate law,unlike in the expression for equilibrium constants,the exponents for concentrations do not necessarily match the stoichiometric coefficients.Reason : It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.

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Assertion : In rate law,unlike in the expression for equilibrium constants,the exponents for concentrations do not necessarily match the stoichiometric coefficients.
Reason : It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.

$A$ complex reaction takes place in the following steps:
$NO_2Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{(g)}$ (slow)
$NO_2Cl_{(g)} + Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{2(g)}$ (fast)
Identify the rate law equation for this reaction.