For the reaction $A + 2B \rightarrow \text{Product } (P)$,the rate law is given by $\frac{d[P]}{dt} = K[A]^2[B]$. If $[A]$ is taken in large excess,what will be the order of the reaction?

Which among the following is a false statement?

Which of the following represents a second-order reaction?

Which of the following is an example of a second-order reaction?

The following reactions occur for the reaction of $NO$ with $Br_2$ to form $NOBr$:
$NO_{(g)} + Br_{2_{(g)}} \rightleftharpoons NOBr_{2_{(g)}}$
$NOBr_{2_{(g)}} + NO_{(g)} \rightarrow 2 NOBr_{(g)}$
If the second reaction is the rate-determining step,the order of the reaction with respect to $NO_{(g)}$ will be:

For the elementary reaction $M \rightarrow N$,the rate of disappearance of $M$ increases by a factor of $8$ upon doubling the concentration of $M$. The order of the reaction with respect to $M$ is :