What is the order of reaction for the rate law $r = k [A]^{\frac{3}{2}} [B]^2$ ?

For the reaction $A \to B$,the rate increases by a factor of $2.25$ when the concentration of $A$ is increased by $1.5$. What is the order of the reaction?

For the reaction $2A + 2B \rightarrow 2C + D$,the rate law is expressed as $\text{rate} = k[A]^2[B]$. Calculate the rate constant if the rate of reaction is $0.24 \ mol \ dm^{-3} \ s^{-1}$ where $[A] = 0.5 \ M$ and $[B] = 0.2 \ M$.

The half-life for a second-order reaction is $30 \ min$. If the initial concentration is $0.1 \ M$,then the value of the rate constant will be $............ \ M^{-1} \ min^{-1}$.

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 . . . . . . .

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: