Answer:
Total pressure = 2.94 atm
Explanation:
Given data:
Mass of nitrogen = 37.14 g
Mass of C₂H₂ = 34.4 g
Mass of CO = 38.25 g
Volume of vessel = 33.53 L
Temperature = 27.3 °C (27.3 + 273 = 300.3 K)
Solution:
Number of moles of nitrogen:
Number of moles = 37.14 g/ 28 g/mol
Number of moles = 1.3 mol
PV = nRT
P = nRT/V
P = 1.3 mol × 0.0821 atm. L. mol⁻¹. K⁻¹ × 300.3 K / 33.53 L
P = 32.1 atm/ 33.53
P = 0.96 atm
Number of moles of C₂H₂:
Number of moles = 34.4 g/ 26.04 g/mol
Number of moles = 1.32 mol
PV = nRT
P = nRT/V
P = 1.32 mol × 0.0821 atm. L. mol⁻¹. K⁻¹ × 300.3 K / 33.53 L
P = 32.54 atm/ 33.53
P = 0.97 atm
Number of moles of CO:
Number of moles = 38.25 g/ 28 g/mol
Number of moles = 1.37 mol
PV = nRT
P = nRT/V
P = 1.37 mol × 0.0821 atm. L. mol⁻¹. K⁻¹ × 300.3 K / 33.53 L
P = 33.8 atm/ 33.53
P = 1.008 atm
Total pressure = P₁ + P₂ + P₃
Total pressure = 1.008 atm + 0.97 atm + 0.96 atm
Total pressure = 2.94 atm
