The rate law of the chemical reaction

$2NO+O_2\to 2N{O}_2$  is given as rate = $k{\left[NO\right]}^2\left[O_2\right]$

Mark out the incorrect inference(s)

Rate law expression of the given reaction is of third order.

Rate law expression of the given reaction is of second order.

The differential form of this rate expression is given as:

$\frac{\mathrm{d}\left[\mathrm{R}\right]}{\mathrm{dt}}=\mathrm{k}{\left[\mathrm{NO}\right]}^2\left[{\mathrm{O}}_2\right]$

If the volume of reaction vessel is reduced to ${\left(\frac{1}{4}\right)}^{th}$of its original value the rate of reaction increases 64 times