Answer:
Pressure of the gas mixture: 4.30 atm
Partial pressure N₂ = 2.15 atm
Partial pressure H₂ = 0.91 atm
Partial pressure CH₄ = 1.23 atm
Explanation:
To determine partial pressure we sum the total moles in order to find out the total pressure
We can work with mole fraction
We apply the Ideal Gases Law
0.700 N₂ + 0.300 H₂ + 0.400 CH₄ = 1.4 moles
We replace data → P . V = n . R .T
T° must be at K → 27 °C + 273 = 300 K
P . 8 L = 1.4 mol . 0.082 L.atm/mol.K . 300 K
P = ( 1.4 mol . 0.082 L.atm/mol.K . 300 K) / 8 L = 4.30 atm (Total pressure)
We apply the mol the fraction for the partial pressure
Moles x gas / total moles = partial pressure x gas / total pressure
Mole fraction N₂ → 0.700 /1.4 = 0.5
Partial pressure N₂ = 0.5 . 4.30 atm =2.15 atm
Mole fraction H₂ → 0.300 / 1.4 = 0.21
Partial pressure H₂ = 0.21 . 4.30 atm = 0.91 atm
Mole fraction CH₄ → 0.400 /1.4 = 0.28
Partial pressure CH₄ = 0.28 . 4.30 atm =1.23 atm
