A 10.0 L flask is used to collect 0.500 moles of N₂ and 0.180 moles of O₂ over water at 30°C.What is the pressure in the flask? (vapor pressure H₂O(l)= 31.8 mm Hg)

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Quizplus · Accepted Answer

The total pressure in the flask is the sum of the partial pressures of each gas plus the vapor pressure of water. The partial pressure of a gas is equal to the number of moles of that gas multiplied by the ideal gas constant and the temperature, divided by the volume of the flask. The vapor pressure of water is given as 31.8 mm Hg.P(N2) = (0.500 mol)(0.0821 Latm/(molK))(303 K) / 10.0 L = 1.28 atmP(O2) = (0.180 mol)(0.0821 Latm/(molK))(303 K) / 10.0 L = 0.458 atmP(H2O) = 31.8 mm Hg = 0.0420 atmTotal pressure = P(N2) + P(O2) + P(H2O) = 1.28 atm + 0.458 atm + 0.0420 atm = 1.78 atm

A 100 L Flask Is Used to Collect 0