The unit of rate constant for a second-order reaction is usually expressed as:

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$H_2 O_2+3 I^{-}+2 H^{+} \rightarrow 2 H_2 O+I_3^{-} \text { Rate }=k\left[H_2 O_2\right]\left[I^{-}\right]$

The rate of a reaction is given by $r = K[x][y] / [OH^-]$. If the concentration of $[OH^-]$ is increased,the order of the reaction will be ........

The decomposition of ozone in the upper atmosphere is catalyzed by nitric oxide. The mechanism of the reaction is as follows:
$2NO \rightleftharpoons N_2O + [O]$
$O_3 + [O] \to 2O_2$ (slow)
Determine the order of the reaction.

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.

Which one of the following statements regarding the order of a reaction is not correct?