Which of the following statements is incorrect?

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

$A$ reaction is first order in $A$ and second order in $B$.
$(i)$ Write the differential rate equation.
$(ii)$ How is the rate affected on increasing the concentration of $B$ three times?
$(iii)$ How is the rate affected when the concentrations of both $A$ and $B$ are doubled?

In a reaction $A \rightarrow B$,if the concentration of reactant is increased by $9$ times,then the rate of reaction increases $3$ times. What is the order of reaction?

For a gaseous reaction between $X$ and $Y$,$X + 3Y \rightarrow XY_3$,the initial rate data is given below:
$[X] = 0.1 \ M, [Y] = 0.1 \ M, \text{Rate} = 0.002 \ Ms^{-1}$
$[X] = 0.2 \ M, [Y] = 0.1 \ M, \text{Rate} = 0.002 \ Ms^{-1}$
$[X] = 0.3 \ M, [Y] = 0.2 \ M, \text{Rate} = 0.008 \ Ms^{-1}$
$[X] = 0.4 \ M, [Y] = 0.3 \ M, \text{Rate} = 0.018 \ Ms^{-1}$
What is the rate law?

The rate of the reaction $2A + 3B \rightarrow 2C + D$ is $6 \times 10^{-4} \text{ mol dm}^{-3} \text{ s}^{-1}$, when $[A] = [B] = 0.3 \text{ mol dm}^{-3}$. If the reaction is of first order with respect to $A$ and zeroth order with respect to $B$, find the rate constant $k$.