Question

Two vessels of capacities 1.5 litres and 2.0 litres containing hydrogen at 750 mm pressure and
oxygen at 100 mm pressure respectively are connected to each other through a valve. What will
be the final pressure of the gaseous mixture assuming that temperature remains constant?​

Answer 1

Answer:

Explanation:

Final volume =1.5L+2.0L=3.5L

for partial pressure of H2

P1V1=P2V2

750×1.5=P2×3.5  ltbr. Or pH2=(750×1.5)/3.5=321.43mm

for partial pressure of O2

P1'V1'=P2'V2'

100×2=P2'×3.5

or pO2=(100×2)/3.5=57.14mm

∴Pmixture=321.43+57.14=378.57mm

Answer 2

Explanation:

Volume of 1.5 litre gas at 750 mm Pressure= 1.5 x750/760= 1.4802 Litre at STP.

Volume of 2.0 Litre gas at 100 mm Pressure= 2 x 100/760= 0.2632 Litre at STP .

Total volume of the gas at STP =1.4802+ 0.2632= 1.7434 Litre.

At constant temperature P°V°= P1V1

So 760 x 1.7434= P1 x 5.

Therefore P1=760 x 1.7434/5

= 265.04 mm of Hg