For the reaction,

$2{N_2}{O_5}\, \to \,4N{O_2}\, + \,{O_2}$

the rate of reaction is

Reaction rate between two substance $A$ and $B$ is expressed as following $:$ rate $= k[A ]^n[B]^m$ If the concentration of $A$ is doubled and concentration of $B$ is made half of initial concentration, the ratio of the new rate to the earlier rate will be

What is the order of reaction $r\, = \,k{[A]^{\frac{3}{2}}}\,{[B]^2}$ ?

For a chemical reaction $A \rightarrow B$, it was found that concentration of $B$ is increased by $0.2\, mol\,L^{-1}$ in $30\, \mathrm{~min}$. The average rate of the reaction is $......\times 10^{-1} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~h}^{-1}$. (Nearest integer)

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 rate of reaction between two reactants $A $ and $B$ decreases by a factor of $4$ if the concentration of reactant $B$ is doubled. The order of this reaction with respect to reactant $B$ is