The concentration of $R$ in the reaction $R \rightarrow P$ was measured as a function of time and the following data is obtained:

$[R]$ (molar)	$1.0$	$0.75$	$0.40$	$0.10$
$\mathrm{t}$ (min.)	$0.0$	$0.05$	$0.12$	$0.18$

The order of the reaction is

${A_2} + {B_2} \to 2AB;R.O.R = k{[{A_2}]^a}{[{B_2}]^b}$

Order of reaction with respect to $A_2$ and $B_2$ are respectively 

Why can’t molecularity of any reaction be equal to zero ?

In a chemical reaction $A$ is converted into $B$ . The rates of reaction, starting with initial concentrations of $A$ as $2 \times {10^{ - 3}}\,M$ and $1 \times {10^{ - 3}}\,M$ , are equal to $2.40 \times {10^{ - 4}}\,M{s^{ - 1}}$ and $0.60 \times {10^{ - 4}}\,M{s^{ - 1}}$ respectively. The order of reaction with respect to reactant $A$ will be

For a reaction $2NO(g) + C{l_2}(g)$ $\rightleftharpoons$ $\,2NOCl(g)$. When concentration of $C{l_2}$ is doubled, the rate of reaction becomes two times of the original. When the concentration of $NO$  is doubled the rate becomes four times. What is the order of the reaction

For $n^{th}$ order reaction where $(n < 1)$