For a certain reaction,the expression for half-life is $t_{1/2} \propto \frac{1}{a^{n-1}}$. What is the order of the reaction?

The data for the reaction $A + B \to C$ is given below:

$Exp$	$[A]_0$	$[B]_0$	Initial Rate
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.035$	$0.80$
$3$	$0.012$	$0.070$	$0.10$
$4$	$0.024$	$0.070$	$0.80$

Determine the rate law for the reaction.

If the rate constant $k = 4.5 \times 10^{-7} \text{ L}^2 \text{ mol}^{-2} \text{ s}^{-1}$, then what is the order of the reaction?

The following graph shows how $T_{1/2}$ (half-life) of a reactant $R$ changes with the initial reactant concentration $a_0$. The order of the reaction will be:

Write the differential rate expression for the following reactions and determine their order of reaction:
$1) \ 2 N_2O_5(g) \rightarrow 4 NO_2(g) + O_2(g)$
$2) \ C_4H_9Cl(aq) + OH^-(aq) \rightarrow C_4H_9OH(aq) + Cl^-(aq)$

The half-life of decomposition of gaseous $CH_3CHO$ at initial pressure of $364 \ mm$ and $182 \ mm$ of $Hg$ were $440 \ sec$ and $880 \ sec$ respectively. The order of the reaction is