Nitric oxide $\left(\text{NO}\right)$ reacts with molecular oxygen as follows:
                                                   $\text{2NO}\left(\text{g}\right)+{\text{O}}_{\text{2}}\left(\text{g}\right)\to {\text{2NO}}_{\text{2}}\left(\text{g}\right)$
Initially $\text{NO}$  and ${\text{O}}_{\text{2}}$ are separated as shown below. When the valve is opened, the 

reaction quickly goes to completion. Assume that the temperature remains constant at 
27° C.
$[\text{R}=0.0\text{8 atm L}/\text{mol}/\text{K}]$

 

	List I		List II
I)	The number of moles of  ${\text{NO}}_{\text{2}}$ after reaction in $\text{4 L}$  flask is	P)	0
II)	The pressure (in atm) of ${\text{O}}_{\text{2}}$  in  $\text{2 L}$ container after the reaction is	Q)	1
III)	The ratio of partial pressure of ${\text{NO}}_{\text{2}}$  in $\text{4 L}$  container to   container is	R)	0.167
IV)	The number of moles of $\text{NO}$  after reaction in $\text{2 L}$  flask is	S)	0.056
		T)	0.028

The correct option is: