A sample of O2 of volume 4.56 L was collected over water at 25c and a total pressure of 1.00 atm. The partial pressure of water is 34.5 Torr. How many moles of O2molescules were collected?

0.178 moles of oxygen gas molecules were collected.

Explanation:

Pressure at which oxygen gas collected = p= 1.00 atm

Vapor pressure of the water

Pressure of the oxygen gas = P

p = p' + P

P = 1.00 atm -  0.0454 atm = 0.9546 atm

Volume of the oxygen gas = V = 4.56 L

Moles of oxygen gas = n

Temperature at which gas collected = T =

(ideal gas)

0.178 moles of oxygen gas molecules were collected.

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