12,779 views
34 votes
34 votes
A mixture of gases contains 0.320 mol CH4, 0.240 mol C2H6, and 0.300 mol C3H8. The total pressure is 1.45 atm. Calculate the partial pressures of the gases.

User GIJOW
by
2.8k points

1 Answer

23 votes
23 votes

Answer:

pCH₄ = 0.540 atm

pC₂H₆ = 0.405 atm

pC₃H₈ = 0.505 atm

Step-by-step explanation:

Step 1: Calculate the total number of gaseous moles

n = n(CH₄) + n(C₂H₆) + n(C₃H₈)

n = 0.320 mol + 0.240 mol + 0.300 mol = 0.860 mol

Step 2: Calculate the partial pressure of each gas

We will use the following expression.

pi = P × Χi

where,

  • pi: partial pressure of the gas "i"
  • P: total pressure
  • Χi: mole fraction of the gas "i"

pCH₄ = 1.45 atm × 0.320 mol/0.860 mol = 0.540 atm

pC₂H₆ = 1.45 atm × 0.240 mol/0.860 mol = 0.405 atm

pC₃H₈ = 1.45 atm × 0.300 mol/0.860 mol = 0.505 atm

User Klarth
by
3.0k points