5 moles gas are introduced in 1 litre container a 47° C. Select the correct option (s).

$[\mathrm{R}=0.08\text{ litre }-\mathrm{atm}/\mathrm{mol}-\mathrm{K}]$

Pressure would be 33.33 atm if it follows van der Waals' equation, $a=4\mathrm{atm}-{\mathrm{litre}}^2 /{\mathrm{mol}}^2$ and $\mathrm{b}=0.04\mathrm{L}/\mathrm{mole}$

Pressure would be 128 atm if it behaves ideally 

Pressure would be 160 atm if it follows van der Waals' equation, $a=4\mathrm{atm}-{\mathrm{litre}}^2 /{\mathrm{mol}}^2$ and $\mathrm{b}=0.04\mathrm{L}/\mathrm{mole}$

 Pressure would be 28 atm if it follows van der Waals' equation,$a=4\mathrm{atm}-{\mathrm{litre}}^2 /{\mathrm{mol}}^2$  and b=0