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
A. The pressure of the gas mixture is 4.31 atm
B. The partial pressure of N₂ is 2.16 atm
C. The partial pressure of H₂ is 0.92 atm
D. The partial pressure of CH₄ is 1.23 atm
A. Determination of the pressure of the gas mixture
Mole of N₂ = 0.7 mole
Mole of H₂ = 0.3 mole
Mole of CH₄ = 0.4 mole
Total mole (n) = 0.7 + 0.3 + 0.4 = 1.4 mole
Volume (V) = 8 L
Temperature (T) = 27 °C = 27 + 273 = 300 K
Gas constant (R) = 0.0821 atm.L/Kmol
PV = nRT
P × 8 = 1.4 × 0.0821 × 300
P × 8 = 34.482
Divide both side by 8
P = 34.482 / 8
Thus, the pressure of the gas mixture is 4.31 atm
B. Determination of the partial pressure of N₂
Total mole = 1.4 mole
Total pressure = 4.31 atm
Mole of N₂ = 0.7 mole
[tex]partial \: pressure = \frac{mole}{total \: mole} \times total \: pressure \\ \\ = \frac{0.7}{1.4} \times 4.31 \\ \\ [/tex]
C. Determination of the partial pressure of H₂
Mole of H₂ = 0.3 mole
Total mole = 1.4 mole
Total pressure = 4.31 atm
[tex]partial \: pressure = \frac{mole}{total \: mole} \times total \: pressure \\ \\ = \frac{0.3}{1.4} \times 4.31 \\ \\ [/tex]
D. Determination of the partial pressure of CH₄
Partial pressure of N₂ = 2.16 atm
Partial pressure of H₂ = 0.92 atm
Total pressure = 4.31 atm
Partial pressure of CH₄ = Total pressure – (Partial of N₂ + Partial pressure of H₂
Partial pressure of CH₄ = 4.31 – (2.16 + 0.92)
Learn more: https://brainly.com/question/16943098
