For three reactions of first,second,and third order,the rate constants are numerically equal. If the concentration of the reactant is the same and greater than $1 \ M$,which of the following is true for the rates of these three reactions?

Which of the following represents a second-order reaction?

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

The rate constants for first-order and second-order reactions have units of ..... respectively.

Which among the following is a false statement?

For a given reaction $t_{1/2} = \frac{1}{Ka}$. The order of the reaction is