During Kinetic study of reaction $2 A+B \rightarrow C+D$, the following results were obtained :

	$A[M]$	$B[M]$	initial rate of formation of $D$
$i$	$0.1$	$0.1$	$6.0 \times 10^{-3}$
$ii$	$0.3$	$0.2$	$7.2 \times 10^{-2}$
$ii$	$0.3$	$0.4$	$2.88 \times 10^{-1}$
$iv$	$0.4$	$0.1$	$2.40 \times 10^{-2}$

Based on above data, overall order of the reaction is $\qquad$

The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor

Consider the following reaction,

$2 H _2( g )+2 NO ( g ) \rightarrow N _2( g )+2 H _2 O ( g )$

which following the mechanism given below:

$2 NO ( g ) \underset{ k _{-1}}{\stackrel{ k _1}{\rightleftharpoons}} N _2 O _2( g )$

$N _2 O _2( g )+ H _2( g ) \stackrel{ k _2}{\rightleftharpoons} N _2 O ( g )+ H _2 O ( g )$

$N _2 O ( g )+ H _2( g ) \stackrel{ k _3}{\rightleftharpoons} N _2( g )+ H _2 O ( g )$

(fast equilibrium)

(slow reaction)

(fast reaction)

The order of the reaction is

The reaction $2 A + B _{2} \rightarrow 2 AB$ is an elementary reaction.

For a certain quantity of reactants, if the volume of the reaction vessel is reduced by a factor of $3,$ the rate of the reaction increases by a factor of $.....$. (Round off to the Nearest Integer).

For a reaction $X + Y \to Z$, rate $ \propto \, [X]$. What is $(i)$ molecularity and $(ii)$ order of reaction ?

The rate of reaction, $A + B + C \longrightarrow P$ is given by

$r = \frac{{ - d\left[ A \right]}}{{dt}} = K\,{\left[ A \right]^{\frac{1}{2}}}\,{\left[ B \right]^{\frac{1}{2}}}\,{\left[ C \right]^{\frac{1}{4}}}$

The order of reaction is