Answer:
Total pressure = 27.35 atm
Explanation:
Given data:
Mass of nitrogen = 12 g
Mass of H₂ = 0.40 mol
Mass of oxygen = 9.0 g
Volume of Container = 1 L
Temperature = 27 °C (27+273 = 300 K)
Total Pressure = ?
Solution:
First of all we will calculate the number of moles of individual gas.
Number of moles = mass/ molar mass
Number of moles = 12 g/ 28 g/mol
Number of moles = 0.43 mol
Pressure of N₂:
PV = nRT
P = nRT/V
P = 0.43 mol × 0.0821 atm.L/mol.K× 300 K/ 1 L
P = 10.6 atm
Number of moles of Oxygen:
Number of moles = mass/ molar mass
Number of moles = 9 g/ 32 g/mol
Number of moles = 0.28 mol
Pressure of O₂:
PV = nRT
P = nRT/V
P = 0.28 mol × 0.0821 atm.L/mol.K× 300 K/ 1 L
P = 6.9 atm
Pressure of H₂:
PV = nRT
P = nRT/V
P = 0.40 mol × 0.0821 atm.L/mol.K× 300 K/ 1 L
P = 9.85 atm
Total pressure:
Total pressure = Pressure of H₂ + Pressure of O₂ + Pressure of N₂
Total pressure = 9.85 atm + 6.9 atm + 10.6 atm
Total pressure = 27.35 atm
