A gaseous mixture made from 37.14 g N2, 34.4 g C2H2, and 38.25 g of CO is placed in a 33.53 L vessel at 27.3 °C. What is the total pressure in the vessel?

Total pressure = 2.94 atm

Explanation:

Given dа ta:

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