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.

pCH₄ = 0.540 atm

pC₂H₆ = 0.405 atm

pC₃H₈ = 0.505 atm

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,

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

here is table 2-2:

country

percent of eligible voters that voted

rank

united states

44.9%

138

canada

60.1%

107

costa rica

84.6%

14

hungary

66.9%

82

japan

57.0%

118

egypt

27.7%

159

south africa

85.5%

10

ans is no, the data set cannot be plotted as a single circle graph