1. What is the density (in g/L) of a sample of nitrogen gas that occupies a volu

Question

1. What is the density (in g/L) of a sample of nitrogen gas that occupies a volume of 5.26L at a pressure of 2.65 atm and a temperature of 29.4oC?

2. The solid chemicals in a specific air bag create 0.663 moles of gas. To what volume (in L) will the air bag inflate at a pressure of 1.10 atm and a temperature of 293 K.

3. A sample of gas contains 3.12 moles of oxygen, 1.36 moles of nitrogen, and 1.09 moles of carbon dioxide. If the total pressure is 2.81 atm, what is the partial pressure of the oxygen in atm?

Explanation / Answer

answer 1

density = mass / volume

by gas law pv=nRT

n = mass / molar mass

molar mass of nitrogen gas = 14

pv = m/mm * RT
p*mm / RT = m/v (and we knw that mass / volume = density so )

density =( 2.65 * 14) / 0.08206*302.55

density = 1.49 g/L

answer 2

pv=nRT

v= nRT / p

v=0663*0.08206*293 / 1.10 = .14.49 L

answer 3

Pi = Ptotal*Xi

here Xi is mole fraction

mole fraction of oxygen = 3.12 / (3.12+1.36+1.09)
mole fraction oxygen = .560

then partial pressure = 2.81 * .5601.57 atm

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.