A study of chemical kinetics of the reaction $A + B \to$  Products, gave the following data at $25\,^oC$.

Exp. No.	[A]	[B]	Rate
$1.$	$1.0$	$0.15$	$4.2 × 10^{-6}$
$2.$	$2.0$	$0.15$	$8.4 × 10^{-6}$
$3.$	$1.0$	$0.20$	$5.6 × 10^{-6}$

Find out rate law

For the reaction:

$2 A + B \rightarrow A _{2} B $

the rate $=k[ A ][ B ]^{2}$ with $k =2.0 \times 10^{-6} \,mol ^{-2}\, L ^{2} \,s ^{-1}$. Calculate the initial rate of the reaction when $[ A ]=0.1 \,mol \,L ^{-1},[ B ]=0.2\, mol \,L ^{-1}$. Calculate the rate of reaction after $[A] $ is reduced to $0.06 \,mol\, L ^{-1}$

The order of a reaction which has the rate expression $\frac{{dc}}{{dt}} = K{[E]^{3/2}}{[D]^{3/2}}$ is

A reaction

$2NO + 2H_2 \longrightarrow N_2 + 2H_2O$

has following mechanism

Step $-I$ : $2NO \longrightarrow N_2O_2$

Step $-II$ : $N_2O_2 + H_2 \longrightarrow N_2O + H_2O$

Step $-III$ : $N_2O + H_2 \longrightarrow N_2 + H_2O$

Which of the following substance is a reaction intermediate

Order of a reaction is decided by

In the reaction $2A + B \to {A_2}B$, if the concentration of $A$ is doubled and of $B$ is halved, then the rate of the reaction will