What is the difference between order of a reaction and the molecularity of a reaction?
Order of a reaction Molecularity of a reaction
It is the sum of the concentration terms on
which the rate of reaction depends or sum ofthe exponents of the concentration in the
law equation.
It is the number of molecules
involved in the slowest
step.
It may be fraction as well as zero
also. It is always a whole number
It can only be determined
experimentally i.e., can not be calculated It can be calculated by simply
adding the molecules of the slowest step.
Statement - I: For the reaction given below: The molecularity of the first step is 1 and the second step is 2. $$2O_3(g) \rightarrow 3O_2(g)$$ Step 1: $$O_3(g)\rightleftharpoons \, O_2(g) + O(g)$$ Step 2: $$O_3(g) + O \xrightarrow[]{slow} 2O_2(g)$$ Statement - II: O(g) is an intermediate. The rate of reaction is $$K[O_3]^2[O_2]^{-1}$$ and the order of the reaction is 1.
The rate of the reaction $$H_{2}(g)+Br_{2}(g)\rightarrow 2HBr(g)$$ is given by: $$r=k[H_{2}][Br_{2}]^{1/2}$$ Which among the following is correct?
Which of the following is/are true :
For a reaction; $$X + Y\rightarrow Z, rate \propto [X]$$. What is (i) molecularity and (ii) order of the reaction?
For the reaction : $$ 2NH_3 (g) \rightarrow N_2(g) + 3H_2 (g) $$ Rate $$ = k $$ Write the order and molecularity of this reaction .
Why is molecularity applicable only for elementary reactions and order is applicable for elementary as well as complex reactions ?
What is the difference between the order of a reaction and its molecularity?