Which will be the unit of rate constant for the reaction having Rate $= K[A]^{\frac{1}{2}} \cdot [B]^{\frac{3}{2}}$ ?

In a one-component second-order reaction,if the concentration of the reactant is reduced to half,the rate

For a chemical reaction $A + B \rightarrow \text{Product}$,the order is $1$ with respect to $A$ and $B$.

Rate $(mol \ L^{-1} \ s^{-1})$	$[A]$ $(mol \ L^{-1})$	$[B]$ $(mol \ L^{-1})$
$0.10$	$20$	$0.5$
$0.40$	$x$	$0.5$
$0.80$	$40$	$y$

What is the value of $x$ and $y$?

For a reaction $2 \ A + B \rightarrow P$, when the concentration of $B$ alone is doubled, the rate does not change, and when the concentrations of both $A$ and $B$ are doubled, the rate increases by a factor of $4$. The unit of the rate constant is,

Assuming the reaction $2NO_{(g)} + Cl_{2(g)} \longrightarrow 2NOCl_{(g)}$ occurs in a single elementary step,we can say that

The mechanism of the reaction,$2NO_{(g)} + 2H_{2(g)} \to N_{2(g)} + 2H_2O_{(g)}$ is:
Step $1$: $2NO_{(g)} + H_{2(g)} \xrightarrow{\text{slow}} N_2 + H_2O_2$
Step $2$: $H_2O_2 + H_2 \xrightarrow{\text{fast}} 2H_2O$
Then the correct statement is: