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

The following are the rate constants of two different reactions. What is the overall order of each reaction?
$(a)$ $2.1 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$
$(b)$ $4.5 \times 10^{-3} \ min^{-1}$

For the reaction $AB_5 \to AB + 4B$,if $- \frac{d[AB_5]}{dt} = K_1[AB_5]$ and $\frac{d[B]}{dt} = K_2[AB_5]$,then:

Which of the following rate laws has an overall order of $0.5$ for a reaction involving substances $x$,$y$,and $z$?

For the reaction $2A + B \rightarrow C$,the rate law is given by: $\text{Rate} = k[A][B]$. Which of the following statements is correct regarding this reaction?

For a chemical reaction $Y + 2Z \to$ Product,the rate-controlling step is $Y + \frac{1}{2}Z \to Q$. If the concentration of $Z$ is doubled,the rate of reaction will: