# Each component contributes to the pressure in the above example. What is the partial pressure... help?

PV = nRT P = nRT/V V = nRT/P n = PV/RT T = PV/nR R = PV/nT

P = Pressure in atmospheres V = Volume in Liters n = number of moles

T = absolute temperature in oK R = the ideal gas constant 0.0821 L-atm/mol-oK

Boyle’s Law: P1V1 = P2V2 Charles’ Law: V1/T1 = V2/T2 P1/T1 = P2/T2

Molar Mass, M: M =mRT/PV For component i, Mole fraction (Xi) = ni/ntotal

where m is the mass of gas Partial pressure of i: Pi = Ptotal x Xi

1 atmosphere = 760 Torr = 760 mm Hg oK = oC + 273.15

Standard Temperature and Pressure (STP) is 0 oC and 1 atm.

6.Each component contributes to the pressure in the above example. What is the partial pressure (in atmospheres) of each of the components above?

Update:

the above example was

What is the volume at STP occupied by a gas mixture having 0.5 mol methane, 0.25 mol hydrogen and 1.25 mol of oxygen?

the answer is: 2.00 mol x 22.4 L/mol=44.8 L

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• 9 years ago