The vapor pressure of water at `80^(@)C` is `355` torr. A `100 ml` vessel contained water-saturated oxygen `80^(@)C`, the total gas pressure being `760` torr. The contents of the vessel were pumped into a `50.0m` vessel at the same temperature. What were the partial pressure of oxygen and of water vapor, with was the total pressure in the final equilibrated state? Neglect the volume of any water which condense.

The vapor pressure of water at `80^(@)C` is `355` torr. A `100 ml` ves

1.	The vapor pressure of water at `80^(@)C` is `355` torr. A `100 ml` vessel contained water-saturated oxygen `80^(@)C`, the total gas pressure being `760` torr. The contents of the vessel were pumped into a `50.0m` vessel at the same temperature. What were the partial pressure of oxygen and of water vapor, with was the total pressure in the final equilibrated state? Neglect the volume of any water which condense.
Answer» Correct Answer - `P_(O_(2))=810mmHg, P_(H_(2))O=355mm Hg, P_("total")=1165mm Hg` In `100ml` vessel which contained water-saturated oxygen, the pressure of `O_(2)` gas`=760-355=405` torr when the contents of this vessel were pumped into `50ml` at the same temperature, pressure of oxygen gets doubled i.e. `P_(O_(2)=810` torr. But pressure of water vapour will remain constant, as some vapour in this `50ml` vessel, gets condense. So `P

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