A vessel has nitrogen gas and water vapour in equilibrium with liquid water at a total pressure of $1$ atm. The partial pressure of water vapours is $0.3$ atm. The volume of this vessel is reduced to one-third of the original volume, at the same temperature, then find total pressure in atm of the system. (Neglect volume occupied by liquid water)

Q. A vessel has $N_2$ gas and water vapours at a total pressure of 1 atm. The partial pressure of water vapours is 0.3 atm. The contents of this vessel are transferred to another vessel having one-third of the capacity of original volume, completely at the same temperature the total pressure of this system in the new vessel is

Q. A vessel has nitrogen gas and water vapours at a total pressure of 1 atm. The partial pressure of water vapour is 0.4 atm. The content of this vessel are transferred completely to another vessel having one-third of the capacity of the original volume at the same temperature, then the total pressure of this system in the new vessel is:

Q. A vessel has $N_2$ gas and water vapour at a total pressure of 1 atm. The partial pressure of water vapour is 0.3 atm. The contents of this vessel are transferred to another vessel having one third of the capacity of original vessel at the same temperature. The total pressure of this system in the new vessel is:

Q. A container contains the mixture of water vapour and oxygen gas with total pressure 1.1 atm at a certain temperature. If the volume is made one third then the total pressure will be:

Q. The vapour pressure of water at ${80}^{\circ }C$ is 355 torr. A 100 ml vessel contained water - saturated oxygen at ${80}^{\circ }C$, the total gas pressure being 730 torr. The contents of the vessel were pumped into 50.0 ml, vessel at the same temperature. What were partial pressures of oxygen and of vapour and the total pressure in the final equilibrium state ? Neglect the volume of any water might condense.