For a second-order reaction where the initial concentrations of both reactants are equal,it takes $3000 \ s$ for the reaction to be $60\%$ complete. How much time (in $s$) will it take for the reaction to be $20\%$ complete?

For the hypothetical reaction $2X + G \to Q + 2M$,the rate expression is $\frac{d[Q]}{dt} = k[X]^2$. Which of the following is the most likely mechanism?

For the reaction $A + 2B \rightarrow \text{Product } (P)$,the rate law is given by $\frac{d[P]}{dt} = K[A]^2[B]$. If $[A]$ is taken in large excess,what will be the order of the reaction?

For the reaction $A + B \rightarrow C$, we have the following data:

Initial concentration of $A$ $(M)$	Initial concentration of $B$ $(M)$	Initial Rate $(M \cdot s^{-1})$
$1$	$10$	$100$
$1$	$1$	$1$
$10$	$1$	$10$

The order of the reaction with respect to $A$ and $B$ are:

If doubling the concentration of a reactant $A$ increases the rate $4$ times and tripling the concentration of $A$ increases the rate $9$ times,the rate is proportional to

The reaction $3ClO^{-} \rightarrow ClO_{3}^{-} + 2Cl^{-}$ occurs in the following two steps:
$(i)$ $ClO^{-} + ClO^{-} \xrightarrow{K_{1}} ClO_{2}^{-} + Cl^{-}$ (Slow step)
$(ii)$ $ClO_{2}^{-} + ClO^{-} \xrightarrow{K_{2}} ClO_{3}^{-} + Cl^{-}$ (Fast step)
Then the rate of the given reaction is equal to . . . . . . .