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:

When the initial concentration of a reactant is doubled in a reaction,its half-life period is not affected. The order of the reaction is:

$A$ reaction is first order with respect to $A$ and second order with respect to $B$. How many times the rate of reaction is affected on increasing the concentration of $B$ three times?

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

$2 \ NO_{(g)} + Cl_{2(g)} \rightleftharpoons 2 \ NOCl_{(g)}$
This reaction was studied at $-10^{\circ} C$ and the following data was obtained:

$Run$	$[NO]_{0}$	$[Cl_{2}]_{0}$	$r_{0}$
$1$	$0.10$	$0.10$	$0.18$
$2$	$0.10$	$0.20$	$0.35$
$3$	$0.20$	$0.20$	$1.40$

$[NO]_{0}$ and $[Cl_{2}]_{0}$ are the initial concentrations and $r_{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).

For a reaction $A + B \rightarrow \text{Product}$,the rate of reaction doubles when the concentration of $A$ is doubled. The rate becomes four times when the concentrations of both $A$ and $B$ are doubled. What is the order of the reaction with respect to $A$ and $B$ respectively?