Answer:
Total pressure: 2.89 atm
Mole fraction CO: 0.88
Partial pressure CO: 2.56 atm
Mole fraction ClF₅: 0.12
Partial pressure ClF₅: 0.33 atm
Explanation:
We should apply the Ideal Gases Law to solve this:
P . V = n . R . T
We need n, which is the total moles for the mixture
Total moles = Moles of CO + Moles of ClF₅
Moles of CO = mass of CO / molar mass CO → 18 g/28 g/mol = 0.643 mol
Moles of ClF₅ = mass of ClF₅ / molar mass ClF₅ → 10.6g/ 130.45 g/m = 0.0812 mol
0.643 mol + 0.0812 mol → 0.724 moles in the mixture
So we have the total moles so with the formula we would know the total pressure.
P . 6L = 0.724 mol . 0.082L.atm/mol.K . 292.2K
P = ( 0.724 mol . 0.082L.atm/mol.K . 292.2K) / 6L
P = 2.89 atm
Mole fraction is defined as the quotient between the moles of gas over total moles, and it is equal to partial pressure of that gas over total pressure
Moles of gas X /Total moles = Partial pressure of gas X/Total pressure
(Moles of gas X / Total moles) . Total pressure = Partial pressure of gas X
Mole fraction CO = 0.643 / 0.724 = 0.88
Partial pressure CO = 0.88 . 2.89 atm → 2.56 atm
Mole fraction ClF₅ = 0.0812 / 0.724 = 0.12
Partial pressure ClF₅ = 0.12 . 2.89 atm → 0.33 atm
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