(C) The rate law is given as $Rate = K [CCl_3CHO]^1 [NO]^1$. The overall order of the reaction is the sum of the powers of the concentration terms,whi

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(C) The rate law is given as $Rate = K [CCl_3CHO]^1 [NO]^1$. The overall order of the reaction is the sum of the powers of the concentration terms,which is $1 + 1 = 2$. For a reaction of order $n$,the units of the rate constant $K$ are $(mol \ L^{-1})^{1-n} \ s^{-1}$. Substituting $n = 2$,we get $(mol \ L^{-1})^{1-2} \ s^{-1} = (mol \ L^{-1})^{-1} \ s^{-1} = L \ mol^{-1} \ s^{-1}$.

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

Easy

The rate of the reaction $CCl_3CHO + NO \to CHCl_3 + NO + CO$ is given by $Rate = K [CCl_3CHO] [NO]$. If concentration is expressed in $mol \ L^{-1}$,the units of $K$ are:

A
$L^2 \ mol^{-2} \ s^{-1}$
B
$mol \ L^{-1} \ s^{-1}$
C
$L \ mol^{-1} \ s^{-1}$
D
$s^{-1}$

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Class 12

Chemistry Questions

Chapter

Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

Write the general equation of a reaction and explain what the order of reaction is. What are its possible values?

Difficult

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The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3 \times 10^{-5} \, s^{-1}$. If the rate is $2.40 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$,then the concentration of $N_2O_5$ (in $mol \, L^{-1}$) is

MediumIIT 2000

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Consider the gaseous reaction $A_2 + B_2 \rightarrow 2 AB$. The following data was obtained for the above reaction:
$[A_2]_0$ $[B_2]_0$ Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$
$0.1 \ M$ $0.1 \ M$ $2.5 \times 10^{-4}$
$0.2 \ M$ $0.1 \ M$ $5.0 \times 10^{-4}$
$0.2 \ M$ $0.2 \ M$ $1.0 \times 10^{-3}$

The value of the rate constant for the above reaction is:

DifficultTS EAMCET 2024

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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

DifficultJEE MAIN 2023

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For the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate equation can be expressed in two ways $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$ and $+\frac{d[NO_2]}{dt} = k'[N_2O_5]$. $k$ and $k'$ are related as:

DifficultJEE MAIN 2014

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$[A_2]_0$	$[B_2]_0$	Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$
$0.1 \ M$	$0.1 \ M$	$2.5 \times 10^{-4}$
$0.2 \ M$	$0.1 \ M$	$5.0 \times 10^{-4}$
$0.2 \ M$	$0.2 \ M$	$1.0 \times 10^{-3}$

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

The rate of the reaction $CCl_3CHO + NO \to CHCl_3 + NO + CO$ is given by $Rate = K [CCl_3CHO] [NO]$. If concentration is expressed in $mol \ L^{-1}$,the units of $K$ are:

Similar Questions

Write the general equation of a reaction and explain what the order of reaction is. What are its possible values?

The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3 \times 10^{-5} \, s^{-1}$. If the rate is $2.40 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$,then the concentration of $N_2O_5$ (in $mol \, L^{-1}$) is

$A$ 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 the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate equation can be expressed in two ways $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$ and $+\frac{d[NO_2]}{dt} = k'[N_2O_5]$. $k$ and $k'$ are related as:

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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