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?

$A$ reaction $A + B \rightarrow C$ is second order in $A$ and zeroth order in $B$. How is the rate affected when the concentration of $A$ is doubled and $B$ is halved?

For the reaction $aA \to xP$,the rate is $2.4 \ mMs^{-1}$ when $[A] = 2.2 \ M$. When the concentration of $A$ is halved,the rate becomes $0.6 \ mMs^{-1}$. Determine the order of the reaction with respect to $A$.

Assertion: The order of a reaction can have a fractional value.
Reason: The order of a reaction cannot be determined from the balanced chemical equation of a reaction.

The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i)$ and $(ii).$ The respective orders of the reactions are

For the reaction $NO_2 + CO \rightarrow CO_2 + NO$,the rate law is given as $\text{Rate} = K [NO_2]^2$. What is the number of $CO$ molecules participating in the slow step?