The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows:

$P_0 \text{ (mmHg)}$	$250$	$300$
$t_{1/2} \text{ (minutes)}$	$135$	$112.5$

The order of reaction is -

For a reaction: $3X \to 4Y$,calculate the rate of reaction based on the following graph when the concentration of $X$ is $0.1 \ M$.

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.

For the reaction $A + B \to C + D$,if the concentration of $A$ is doubled without affecting the concentration of $B$,the rate doubles. If the concentration of $B$ is increased $9$ times without affecting the concentration of $A$,the rate becomes $3$ times. Determine the order of the reaction.

If the concentration of reactant $A$ is increased by $10$ times,the rate of reaction becomes $100$ times. What is the order of reaction if the rate law is,$\text{rate} = k[A]^{x}$?

$A_2 + 2 \, B \to 2 \, AB$

$[A_2]$	$[B]$	$-d[A_2]/dt$
$0.1$	$0.2$	$1 \times 10^{-2} \, M \, s^{-1}$
$0.2$	$0.2$	$2 \times 10^{-2} \, M \, s^{-1}$
$0.2$	$0.4$	$8 \times 10^{-2} \, M \, s^{-1}$

The order of reaction with respect to $A_2$ and $B$ are respectively: