A gaseous mixture contains 160 grams of neon and 64 grams of oxygen in 82.1 litre vessel at 27°C, then the partial pressure of Neon may be __atm

Partial pressure=mole fraction × total pressure

Weight of neon=160g

Molar mass of neon=20

Number of moles=160/20=8

Number of moles of oxygen=64/32=2

Total number of moles=10

Pv=nRT

$\mathrm{P}=\frac{\mathrm{nRT}}{\mathrm{V}}$

$\mathrm{P}=\frac{0.0821\times 10\times 300}{82.1}$

P = 3atm

Partial pressure=$\frac{8}{10}\times 3$

Partial pressure of neon=2.4 atm

Hence the required option is A