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

The mechanism of reaction $2 \ NO + Cl_2 \rightarrow 2 \ NOCl$ is given as :
$(i) 2 NO \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} N_2 O _2$ (fast)
$(ii) N_2O_2 + Cl_2 \xrightarrow{K_3} 2 \ NOCl$ (slow)
The rate expression of the reaction will be :

For the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ in $mol \ L^{-1}$ will be:

For the reaction $A + 2B \longrightarrow C$, the reaction rate is doubled if the concentration of $A$ is doubled. The rate is increased by four times when concentrations of both $A$ and $B$ are increased by four times. The order of the reaction is

The reaction $2A + B_{2} \rightarrow 2AB$ is an elementary reaction. For a certain quantity of reactants,if the volume of the reaction vessel is reduced by a factor of $3,$ the rate of the reaction increases by a factor of $.....$. (Round off to the Nearest Integer).

If a reaction has the experimental rate expression $\text{rate} = K [A]^2[B]$,what happens to the reaction rate if the concentration of $A$ is doubled and the concentration of $B$ is halved?