(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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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

For a hypothetical reaction,$A \rightarrow C$. The mechanism is: $A \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} B$ (Fast),$A + B \xrightarrow{k_3} C$ (Slow). The rate law for this reaction is:

MediumTS EAMCET 2021

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For three reactions of first,second,and third order,the rate constants are numerically equal. If the concentration of the reactant is the same and greater than $1 \ M$,which of the following is true for the rates of these three reactions?

Medium

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The rate constant of which of the following reactions is independent of the concentration of the reactants?

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For the reaction $H_{2(g)} + Br_{2(g)} \to 2HBr_{(g)}$,the experimental data suggest,$\text{rate} = K[H_2][Br_2]^{1/2}$. The molecularity and order of the reaction are respectively:

Easy

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Write the differential rate expression for the following reactions and determine their order of reaction:
$1) \ 2 \ HI \rightarrow H_2 + I_2$
$2) \ 2 \ NO_{(g)} + O_{2(g)} \rightarrow 2 \ NO_{2(g)}$

Medium

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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

For a hypothetical reaction,$A \rightarrow C$. The mechanism is: $A \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} B$ (Fast),$A + B \xrightarrow{k_3} C$ (Slow). The rate law for this reaction is:

For three reactions of first,second,and third order,the rate constants are numerically equal. If the concentration of the reactant is the same and greater than $1 \ M$,which of the following is true for the rates of these three reactions?

The rate constant of which of the following reactions is independent of the concentration of the reactants?

For the reaction $H_{2(g)} + Br_{2(g)} \to 2HBr_{(g)}$,the experimental data suggest,$\text{rate} = K[H_2][Br_2]^{1/2}$. The molecularity and order of the reaction are respectively:

Write the differential rate expression for the following reactions and determine their order of reaction:$1) \ 2 \ HI \rightarrow H_2 + I_2$$2) \ 2 \ NO_{(g)} + O_{2(g)} \rightarrow 2 \ NO_{2(g)}$

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Write the differential rate expression for the following reactions and determine their order of reaction:
$1) \ 2 \ HI \rightarrow H_2 + I_2$
$2) \ 2 \ NO_{(g)} + O_{2(g)} \rightarrow 2 \ NO_{2(g)}$