A 250 ml sample of oxygen is collected over water at 25degrees celcius and 760 torr pressure. What is the pressure of the dry gas alone? (Vapor pressure of water at 25 =23.8 torr)
Well this is the problem. What do I do to solve this exactly?
2007-01-03 13:42:27 · 2 answers · asked by epooji 3 in Science & Mathematics ➔ Chemistry
How do I solve for the dry gas?
2007-01-03 13:54:02 · update #1
subtract the vapor pressure of water from 760 torr
760 torr-23.8 torr=ur answer sorry i dnt have a calc with me right now.
you have to solve for the pressure of the gas (partial pressure), whcih adds up to 1 atm, or 760 torr.
2007-01-03 13:45:21 · answer #1 · answered by Anonymous · 0⤊ 1⤋
When collecting a gas over water the total pressure is equal to the pressure of the gas + the vapor pressure of the water. (The water evaporates and adds water vapor to the collected gas).
Using Dalton's Law of Partial Pressure you can say:
total pressure = pressure of the gas + vapor pressure
You know the total pressure and the vapor pressure; solve for the pressure of the dry gas
2007-01-03 13:45:59 · answer #2 · answered by The Old Professor 5 · 0⤊ 1⤋