The rate of reaction between two reactants $A$ and $B$ decreases by a factor of $4$ if the concentration of reactant $B$ is doubled. The order of this reaction with respect to reactant $B$ is

For a reaction,$I^{-} + OCl^{-} \to IO^{-} + Cl^{-}$ in an aqueous medium,the rate of reaction is given by $\frac{d[IO^{-}]}{dt} = k[I^{-}][OCl^{-}]$. The overall order of reaction is

For the reaction $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$,the experimental data suggests the rate law is $\text{Rate} = K[H_2][Br_2]^{1/2}$. Find the order of the reaction and its molecularity.

By giving three examples,explain whether the exponents of the concentration terms in a rate law are the same as their stoichiometric coefficients in the balanced chemical reaction.

If the concentration of a first-order reaction is increased by $x$ times,then the rate constant $(k)$ becomes

For the reaction ${H_{2(g)} + I_{2(g)} \to 2HI_{(g)}}$,the possible mechanism is given below:
$I_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2 I$ (fast step)
${2I + H_2 \xrightarrow{K_2} 2HI}$ (slow step)
Determine the rate law for the reaction.