Calculate the order of the reaction with respect to $A$ and $B$ based on the following data:

$[A] \ (mol/L)$	$[B] \ (mol/L)$	Rate $(mol/L \cdot s)$
$0.05$	$0.05$	$1.2 \times 10^{-3}$
$0.10$	$0.05$	$2.4 \times 10^{-3}$
$0.05$	$0.10$	$1.2 \times 10^{-3}$

Consider the reaction between chlorine and nitric oxide:
$Cl_{2(g)} + 2NO_{(g)} \rightarrow 2NOCl_{(g)}$
On doubling the concentration of both reactants,the rate of the reaction increases by a factor of $8$. However,if only the concentration of $Cl_2$ is doubled,the rate increases by a factor of $2$. The order of this reaction with respect to $NO$ is :

Why can we not determine the order of a reaction by taking into consideration the balanced chemical equation?

Ozone decomposes into oxygen as follows:
$O_3 \rightleftharpoons O_2 + [O]$
$O_3 + [O] \to 2O_2$ (slow)
Determine the order of the reaction $2O_3 \to 3O_2$.

The rate of reaction between $A$ and $B$ increases by a factor of $100$ when the concentration of $A$ is increased $10$ folds. The order of reaction with respect to $A$ is

The rate law for the reaction $A^{+} + B^{+} + C \longrightarrow \text{Product}$ is expressed as $\text{Rate} = k[A]^{2}[B]^{1}[C]^{0}$. What is the overall order of the reaction?