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

Rate law for a reaction is $r=k[A]^2[B]$. If rate constant is $6.25 \ mol^{-2} \ dm^6 \ s^{-1}$,what is the rate of reaction when $[A]=1 \ mol \ dm^{-3}$ and $[B]=0.2 \ mol \ dm^{-3}$?

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?

The velocity constant of a reaction is $K$. Which of the following statements is not true regarding $K$?

The mechanism of the reaction $2NO_{(g)} + Br_{2(g)} \rightarrow 2NOBr_{(g)}$ is given by:
$1) NO_{(g)} + Br_{2(g)} \rightleftharpoons NOBr_{2(g)}$ (fast)
$2) NOBr_{2(g)} + NO_{(g)} \rightarrow 2NOBr_{(g)}$ (slow)
If the second step is the rate-determining step,what is the order of the reaction with respect to $NO_{(g)}$?

The initial reaction $2AB + B \to A_2B_3$ is carried out in vessels of volume $1 \ dm^3$ and $2 \ dm^3$ respectively,using equal moles of reactants. The ratio of the reaction rates $(r_1/r_2)$ is: