If the initial concentration of a reactant is doubled,its half-life period also doubles. Determine the order of the reaction.

Consider the data given below for the hypothetical reaction $A \to X$:

$Time \ (s)$	$Rate \ (mol \ L^{-1} s^{-1})$
$0$	$1.60 \times 10^{-2}$
$10$	$1.60 \times 10^{-2}$
$20$	$1.60 \times 10^{-2}$
$30$	$1.60 \times 10^{-2}$

From the above data,the order of the reaction is:

For the reaction $A \longrightarrow 3 B$,the rate is given by $rate = k[A]^0$. Based on the data provided in the table,what is the concentration of the product $B$ (in $mol \ L^{-1}$) after $20 \ s$?

Time $(s)$	Concentration of the reactant $(mol \ L^{-1})$
$0$	$0.1$
$15$	$0.05$
$20$	$0.1 - x$

If the rate of a reaction is equal to the rate constant,what is the order of the reaction?

The unit of the velocity constant in case of zero order reaction is

The half-life period of a zero order reaction is: