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What does water saturated oxygen mean in this question:
The vapour pressure of water at 80º C is 355 torr. A 100 ml vessel contained water saturated oxygen at 80º 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 of water vapour, what was the total pressure in the final equilibrated state ? Neglect the volume of any water which might condense
Consider the partial pressures separately. If you answer these questions you have your own solution.
Oxygen does not condense, may be deemed an ideal gas. What does halving the volume do to its partial pressure? (We assume that exactly half the volume, 50 ml vs 100 ml, is available because we neglect the liquid volume in this problem.)
Water can condense, adjusting its partial pressure back down to equilibrium. What would that restored equilibrium pressure be versus the vapor pressure given in the problem?
Finally, what does not condense is still essentially an ideal gas, add the partial pressures to get the total pressure.
Good luck!
