Determine the order of reaction on the basis of following data for the reaction $A + B \to C$.

Exp.	$[A]$	$[B]$	Rate of reaction $(mol \ L^{-1} \ s^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.4$	$0.1$	$0.8 \times 10^{-2}$
$3$	$0.1$	$0.2$	$1.6 \times 10^{-2}$

(in $.5$)

For the reaction $A \to \text{Products}$,the rate of reaction becomes one-fourth when the concentration of $A$ is halved. What is the order of the reaction?

In the hydrolysis of an organic chloride in the presence of a large excess of water; $RCl + H_2O \rightarrow ROH + HCl$. What are the molecularity and order of the reaction?

$A$ substance undergoes first-order decomposition. The decomposition follows two parallel first-order reactions as:
$A \xrightarrow{k_1} B$ $k_1 = 1.26 \times 10^{-4} \ s^{-1}$
$A \xrightarrow{k_2} C$ $k_2 = 3.8 \times 10^{-5} \ s^{-1}$
The percentage distribution of $B$ and $C$ are:

For the reaction $2HI \rightleftharpoons H_2 + I_2$,the rate of the reaction is proportional to $[HI]^2$. This means that the reaction is

For the reaction $2N_2O_5 \to 4NO_2 + O_2$,the rate of reaction and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ at that time will be: