For a reaction of order $(n - 1)$,what is the relationship between the half-life period $(t_{1/2})$ and the initial concentration of the reactant $([R]_0)$?

If the order of a reaction is $x$,then the unit of its rate constant is:

For the reaction $A + B \rightarrow \text{product}$,the rate of reaction is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[A] = 0.2 \ mol \ dm^{-3}$ and $[B] = 0.1 \ mol \ dm^{-3}$,calculate the rate constant of the reaction if the reaction is first order in $A$ and second order in $B$.

The bromination of acetone that occurs in acid solution is represented by this equation.
$CH_3COCH_{3(aq)} + Br_{2(aq)} \rightarrow CH_3COCH_2Br_{(aq)} + H^+_{(aq)} + Br^-_{(aq)}$
These kinetic data were obtained for given reaction concentrations.
Initial concentrations,$M$

$[CH_3COCH_3]$	$[Br_2]$	$[H^+]$
$0.30$	$0.05$	$0.05$
$0.30$	$0.10$	$0.05$
$0.30$	$0.10$	$0.10$
$0.40$	$0.05$	$0.20$

Initial rate,disappearance of $Br_2, M s^{-1}$
$5.7 \times 10^{-5}, 5.7 \times 10^{-5}, 1.14 \times 10^{-4}, 3.04 \times 10^{-4}$
Based on these data,the rate equation is

What is the order and molecularity of the following reaction?
$NO_{2(g)} + NO_{2(g)} \longrightarrow 2NO_{(g)} + O_{2(g)}$

When the concentration of a reactant,$A$,in a reaction $A \to \text{Products}$ is doubled,the rate of reaction increases seven times. The order of the reaction is between: