What is the difference between the order of a reaction and its molecularity?
Order of a reaction Molecularity of a reaction
It is the number of molecules whose concentration (changes) determines the rate of the reaction.
It is the number of reactant species which collide simultaneously in a step leading to chemical reaction.
It is the sum of the powers of the concentration of reactants in the rate equation (rate law). It is an experimentally determined quantity.
It is the total number of molecules present in the reactant(s) of a balanced chemical equation.
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 order of a reaction and the molecularity of a reaction?