The rate of the simple reaction, $2NO + O_2 \to  2NO_2$, when the volume of the reaction vessel is doubled

The rate constant for a second order reaction is $8 \times {10^{ - 5}}\,{M^{ - 1}}\,mi{n^{ - 1}}$. How long will it take a $ 1\,M $ solution to be reduced to $0.5\, M$

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 $0.06 \,mol\, L ^{-1}$

When a reaction is progressing

Fill up the blank :

$1.$ The rate of reaction depends on ........... step.

$2.$ In bimolecular reaction the reaction take place with ........... species and ........... .

$3.$ The order of reaction is determine by ...........

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