Question #185234
A mixture of argon and xenon gases, in a 8.85 L flask at 44 °C, contains 17.9 grams of argon and 22.6 grams of xenon. The partial pressure of xenon in the flask is____ atm and the total pressure in the flask is ____ atm.
Expert's answer
The total pressure (P) can be calculated using ideal gas equation: PV = nRT,
for the above problem n is the total number of moles, thus
n =PV/RT
V = 8.85 L, T = 44oC + 273 = 317 K, R = 0.0821 L.atm/mol.K (it is a constant).
Molar Mass of argon = 39.948
= 17.9/39.948 = 0.448M
Molar Mass of Xenon = 131.293
= 22.6/131.293 = 0.172M
0.448 +0.172 = 0.62M
PV = n×RT
8.85P = 0.62 × 0.0821 ×317
8.85p= 16.136
total Pressure = 1.82atm
Partial pressure of Xenon
= 0.172/0.62 × 1.82
= 0.5atm
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