What is the molecularity and order of the following reaction if the rate law is $\text{rate} = k[O_3][O]$ respectively?
$O_{3(g)} + O_{(g)} \longrightarrow 2O_{2(g)}$

The rate of reaction $A + 2B \to 3C$ becomes $72$ times when the concentration of $A$ is tripled and the concentration of $B$ is doubled. The order of reaction with respect to $A$ and $B$ respectively is:

The reaction $A_{(g)} + 2B_{(g)} \longrightarrow C_{(g)} + D_{(g)}$ is an elementary process. In an experiment,the initial partial pressure of $A$ and $B$ are $0.6 \ atm$ and $0.8 \ atm$,respectively. When partial pressure of $C$ is $0.2 \ atm$,the rate of reaction relative to the initial rate is

In a multistep reaction,the overall rate of reaction is equal to the

Consider the given graph showing the variation of reactant concentration with time. Three different reactions were started with identical initial concentration of reactants. Which of the following statements is correct?

For the reaction $A + B \to \text{Product}$,the rate of reaction becomes four times when the concentration of $A$ is doubled. If the rate of reaction does not change when the concentration of $B$ is doubled,the rate law for the reaction will be.....