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

For the reaction $RCl + NaOH_{(aq)} \rightarrow ROH + NaCl$,the rate is given by $Rate = K_1[RCl]$. What will happen to the reaction rate?

The kinetic study of a reaction like $vA \rightarrow P$ at $300 \ K$ provides the following curve, where concentration is taken in $mol \ dm^{-3}$ and time in $min$. Identify the correct order $(n)$ and rate constant $(k)$.

For the reaction $A + B \to C$,it is found that doubling the concentration of $A$ increases the rate by $4$ times,and doubling the concentration of $B$ doubles the reaction rate. What is the overall order of the reaction?

How can you determine the rate law of the following reaction?
$2 \, NO \, (g) + O_2 \, (g) \to 2 \, NO_2 \, (g)$

In a reaction,if the concentration of reactant $A$ is tripled,the rate of reaction becomes twenty-seven times. What is the order of the reaction?