The mechanism of the reaction $A + 2B \to  D$ is

$2B\xrightarrow{k}{B_2}\,\left[ {Slow} \right]$

${B_2} + A \to D\,\left[ {Fast} \right]$

The rate law expression, order with respect to $A$, order with respect to $'B'$ and overall order of reaction are respectively

For reaction $2A + B \to $ products, the active mass of $ B $ is kept constant and that of $A$ is doubled. The rate of reaction will then

State a condition under which a bimolecular reaction is kinetically first order reaction.

For the reaction $A + B \rightarrow$ products, it is observed that

$(i)\,\,$on doubling the initial concentration of $A$ only, the rate of reaction is also doubled and

$(ii)$  on doubling the initial concentration of both $A$ and $B,$ there is a change by a factor of $8$ in the rate of the reaction.

The rate of this reaction is given by

Inversion of canesugar in dilute acid (conversion into glucose and fructose) is a

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