The reaction of NO with O$2$ to give oxygen is known to follow a third order rate law

$($rate $=$ k$[$NO$]2[$O$2]).$ Two possible mechanisms are shown below:

Mechanism $1$ Mechanism $2$

$2$ NO $($g$)+$ O$2($g$)->2$ NO$2($g$)($slow$)2$ NO $($g$)($NO$)2($g$)($fast$)$

$($NO$)2+$ O$2->2$ NO$2($slow$)$

Which of these two mechanisms is a more acceptable mechanism, based on the criteria given above?

Select answer from the options below $-$ Incorrect!

Mechanism $1$ because it is simplerMechanism $1$ because it is simpler

Mechanism $1$ because its rate law is the same as the known rate law

Mechanism $2$ because it only involves $2$ steps

Mechanism $2$ because only bimolecular processes are involved

Mechanism $1$ because no unstable species are formed

The option with the same rate law is incorrect, which other option suits the statement best?