Which of the following is/are true :
The overall rate of a reaction is often approximately determined by the slowest step, known as the rate-determining step (RDS). For a given reaction mechanism, the prediction of the corresponding rate equation (for comparison with the experimental rate law) is often simplified by using this approximation of the rate determining step.
The molecularity of a reaction is defined as the number of molecules or ions that participate in the rate-determining step. Thus, it may be equal or greater than order but never lower.
Thus, A and B are correct.
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?
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?
What is the difference between order of a reaction and the molecularity of a reaction?