Answer:
Mass = 1.84 g
Explanation:
Given data:
Total pressure = 3.44 atm
Volume of flask = 9.62 L
Temperature = 63°C = 63+273.15K = 336.15 K
Mass of CO₂ = 12.5 g
Mass of hydrogen = ?
Solution:
Number of moles of CO₂:
Number of moles = mass/molar mass
Number of moles = 12.5 g/ 44 g/mol
Number of moles = 0.28 mol
Pressure of CO₂:
PV = nRT
R = general gas constant = 0.0821 atm.L/mol.K
P = 0.28 mol × 0.0821 atm.L/mol.K × 336.15 K / 9.62 L
P = 7.73 atm.L/ 9.62 L
P = 0.8 atm
Total pressure = Partial pressure of CO₂ + Partial pressure of H₂
3.44 atm = 0.8 atm + P(H₂)
P(H₂) = 3.44 atm - 0.8 atm
P(H₂) = 2.64 atm
Number of moles of hydrogen:
PV = nRT
2.64 atm × 9.62 L = n × 0.0821 atm.L/mol.K × 336.15 K
25.39 atm.L = n × 27.59atm.L/mol
n = 25.39 atm.L / 27.59atm.L/mol
n = 0.92 mol
Mass of hydrogen:
Mass = number of moles × molar mass
Mass = 0.92 mol × 2 g/mol
Mass = 1.84 g
