The rate of a certain reaction is given by, $Rate = k[H^{+}]^n$. The rate increases $100$ times when the $pH$ changes from $3$ to $1$. The order $(n)$ of the reaction is:

The value of $\frac{t_{0.875}}{t_{0.50}}$ for $n^{th}$ order reaction 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

Find the rate law for the reaction,$CHCl_{3(g)} + Cl_{2(g)} \rightarrow CCl_{4(g)} + HCl_{(g)}$ if the order of reaction with respect to $CHCl_{3(g)}$ is $1$ and with respect to $Cl_{2(g)}$ is $1/2$.

Which of the following represents a second-order reaction?

The three experimental data for determining the differential rate of reaction $2 NO_{(g)} + Cl_{2(g)} \rightarrow 2 NOCl_{(g)}$ at a definite temperature are given below.
$(a)$ Calculate the order of reaction.
$(b)$ Calculate the value of the rate constant.