If the rate of the reaction is equal to the rate constant, the order of the reaction is

For a reaction, $A+B \rightarrow$ Product; the rate law is given by, $r=k[ A ]^{1 / 2}[ B ]^{2}$ What is the order of the reaction?

For a certain reaction, $10\%$ of the reactant dissociates in $1\, hour$, $20\%$ of the reactant dissociate in $2\, hour$, $30\%$ of the reactant dissociates in $3\, hour$. Then the units of rate constant is

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

For a reaction $2NO(g) + C{l_2}(g)$ $\rightleftharpoons$ $\,2NOCl(g)$. When concentration of $C{l_2}$ is doubled, the rate of reaction becomes two times of the original. When the concentration of $NO$  is doubled the rate becomes four times. What is the order of the reaction