Which of these does not influence the rate of reaction

Consider the following single step reaction in gas phase at constant temperature.

$2 \mathrm{~A}_{(\mathrm{g})}+\mathrm{B}_{(\mathrm{g})} \rightarrow \mathrm{C}_{(\mathrm{g})}$

The initial rate of the reaction is recorded as $r_1$ when the reaction starts with $1.5 \mathrm{~atm}$ pressure of $\mathrm{A}$ and $0.7 \mathrm{~atm}$ pressure of B. After some time, the rate $r_2$ is recorded when the pressure of $C$ becomes $0.5 \mathrm{~atm}$. The ratio $r_1: r_2$ is $\qquad$ $\times 10^{-1}$.

(Nearest integer)

If a reaction has the experimental rate expression rate $= K [A]^2[B]$, if the concentration of $A$ is doubled and the concentration of $B$ is halved, the what happens to the reaction rate

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 mechanism of the reaction $2NO_2 + F_2 \to 2NO_2F$ is

$(i)\,\,N{O_2}\,\xrightarrow{{slow}}\,NO + O$

$(ii)\,\,{F_2} + O + NO\,\xrightarrow{{fast}}\,N{O_2}F + F$

$(iii)\,\,F + N{O_2}\,\xrightarrow{{fast}}\,N{O_2}F$

Select the correct one

The reaction $2FeC{l_3} + SnC{l_2} \to 2FeC{l_2} + SnC{l_4}$ is an example of