$A$ reaction involving two different reactants:

Identify the reaction order for which the rate constant $K = 2.3 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$.

Assuming the reaction $2NO_{(g)} + Cl_{2(g)} \longrightarrow 2NOCl_{(g)}$ occurs in a single elementary step,we can say that

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:

The rate of reaction is determined by the slow step of the reaction. This step is called:

For the reaction $aA + bB \to$ product,the rate of reaction is given by $Rate = k[A]^3 [B]^0$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the rate of reaction will be: (in $\times$)