Question

Perm calculations with Dalton's Low Question A sample of gas isolated from unrefined petroleum contains 9.00 mol CH 0.890 mol CH. and 0.110 mol CH, at a total pressure of 307.2 kPa What is the partial pressure of CH,? Select the correct answer below: 276 LP. O 27.3 kPa 3.37 kP O 307 kPa - here to search 11:40 PM AD6 44 2/2000

Answer 1

Given data,

Moles of methane = 9.00 mol

Moles of ethane = 0.890 mol

Moles of propane = 0.110 mol

Total pressure of the mixture = 307.2 kPa

Total number of moles of gaseous mixture = 9.00 + 0.890 + 0.110 = 10.00 mol

Molefractionof methane = molesof methane Totalmolesof allgasesinthemirture

Molefractionofmethane = 9.00 10.00

Mole fraction of methane = 0.900

According Dalton's law of partial pressures, " The partial pressure of a gas in the mixture of non reacting gases is directly proportional to its mole fraction in the mixture".

Mathematically,

pCH4 $\alpha$ XCH4                                          (For methane gas in the mixture)

(OR)

pCH4 = ptotal XCH4

pCH4 = 307.2 * 0.900

pCH4 = 276.48 kPa

Therefore, the partial pressure of methane in the mixture = 276 kPa.