A gaseous mixture of O2 and N2 contains 39.8 % nitrogen by mass. What is the par

Q: A gaseous mixture of O2 and N2 contains 39.8 % nitrogen by mass. What is the par

1. we need by mol so total mass = 100 g 39.8 g are N2 100-39.8 g are O2 mol of N2 = mass/MW = 39.8/28 = 1.4214 mol of O2= mass/MW = (100-39.8)/32 = 1.8812 total mol = 1.8812 + 1.4214 = 3.3026 mol frac of O2 = mol O2 / total = 1.8812/3.3026 = 0.56961 mol frac O2 PO2 = xo2*PT =0.56961*705 = 401.575 mm Hg

ID: 977337 • Letter: A

Question

A gaseous mixture of O2 and N2 contains 39.8 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 705 mmHg ?

Dalton's law states that the total pressure, Ptotal, of a mixture of gases in a container equals the sum of the pressures of each individual gas:

Ptotal=P1+P2+P3+…

The partial pressure of the first component, P1, is equal to the mole fraction of this component, X1, times the total pressure of the mixture:

P1=X1×Ptotal

The mole fraction, X, represents the concentration of the component in the gas mixture, so

X1=moles of component 1total moles in mixture

Explanation / Answer

we need by mol so

total mass = 100 g

39.8 g are N2

100-39.8 g are O2

mol of N2 = mass/MW = 39.8/28 = 1.4214

mol of O2= mass/MW = (100-39.8)/32 = 1.8812

total mol = 1.8812 + 1.4214 = 3.3026

mol frac of O2 = mol O2 / total = 1.8812/3.3026 = 0.56961 mol frac O2

PO2 = xo2*PT =0.56961*705 = 401.575 mm Hg

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A gaseous mixture of O2 and N2 contains 39.8 % nitrogen by mass. What is the par

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