Question

The vapour pressure of water at 80°C is 355 torr. A 100 mL vessel
contained water saturated oxygen at 80°C, the total gas pressure being
760 torr. The contents of the vessel were pumped into a 50.0 mL vessel
at the same temperature. What were the partial pressures of oxygen and
water vapour, what was the total pressure in the first equilibrated state?
Neglect volume of any water which might condense.

Answer 1

Answer:

1165um

Explanation:

vapor pressure of water remain constant, it depend only on the volume of container,it remain constant in 100 mm and 50 ml container if temperature is constant

total pressure =partial pressure of of oxygen +vapor pressure of water

vapor pressure of water=355 mm

total pressure=760 mm

partial pressure of of oxygen=760?355=405 mm

when volume of container is half, pressure of O2 become double and vapor pressure is remain constant

P1V1=P2V2

405 X 100=50 X P2

P2 = 810 mm =partial pressure of of oxygen

vapor pressure of water=355mm

total pressure in 50 ml container =partial pressure of of oxygen +vapor pressure of water

=810+355

=1165mm