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

Initial $[A_2]$	Initial $[B_2]$	$R.O.R.\,(r)\,Ms^{-1}$
$0.2$	$0.2$	$0.04$
$0.1$	$0.4$	$0.04$
$0.2$	$0.4$	$0.08$

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

Which of the following reaction will have fractional order for $A_2$ or $B_2$ ?

For a reaction, $AB_5 \to AB + 4B$ The rate can be expressed in following ways

$\frac{{ - d[A{B_5}]}}{{dt}} = K[A{B_5}]$ ;    $\frac{{d[B]}}{{dt}} = {K_1}[A{B_5}]$

So the correct relation between $K$ and $K_1$ is

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

The order of the reaction is

Write differential rate expression of following reaction and give its order of reaction :

$2 N _{2} O _{5} \rightarrow 4 NO _{2}( g )+ O _{2}$

$C _{4} H _{9} Cl + OH ^{-} \rightarrow C _{4} H _{9} OH + Cl ^{-}$

In a reaction $2A + B \to {A_2}B$, the reactant $ A $ will disappear at