Respuesta :
Answer:
Total pressure → 2.08 atm
Partial pressure N₂ → 1.31 atm
Partial pressure O₂ → 0.76 atm
Explanation:
To determine the total pressure of the mixture we need to know the total moles of the gases:
Sum of moles from gases at the mixture = Total moles (Dalton's law)
We convert the mass from kg to g and then, we states the moles of each:
0.6 kg . 1000g/ 1kg = 600 g // 0.4g . 1000g/ 1kg = 400 g
600 g . 1 mol/28g = 21.4 moles of N₂
400 g . 1mol/32g = 12.5 moles of O₂
Total moles → 21.4 + 12.5 = 33.9 moles
Before to replace the data in the Ideal Gases Law, we notice that the volume is in m³. (1000 dm³ = 1 m³ and 1dm³ = 1L)
0.4m³ . 1000 dm3 / 1m³ = 400 dm³ → 400L
Now, we can put the data on the Ideal Gases Law:
400L . P = 33.9 mol . 0.082L.atm/mol.K . 300K
P = (33.9 mol . 0.082L.atm/mol.K . 300K) / 400L → 2.08 atm
We apply the mole fraction for the partial pressures of each gas:
Moles of N₂ / Total moles = Partial pressure N₂ / Total pressure
Moles of O₂ / Total moles = Partial pressure O₂ / Total pressure
Partial pressure = Total pressure . (Moles of the gas / Total moles)
Partial pressure N₂ = 2.08 atm . (21.4 mol / 33.9 moles) → 1.31 atm
Partial pressure O₂ = 2.08 atm . (12.5 mol / 33.9 moles) → 0.76 atm
Answer:
pN2 = 133.56 kPa
pO2 = 77.94 kPa
Total pressure = 211.5 kPa
Explanation:
Step 1: Data given
Volume of the tank = 0.4 m³
Mass of N2 = 0.6 kg
Mass of O2 = 0.4 kg
Temperature = 300 K
The gas constant for N2 is 0.2968 kPa*m3/kg*K
The gas constant for O2 is 0.2598 kPa*m3/kg*K
Step 2: Calculate the partial pressures
pN2 = MRT / V = (0.6 * 0.2968 * 300)/0.4
pN2 = 133.56 kPa
pO2 = (0.4 * 0.2598 * 300)/ 0.4
pO2 = 77.94 kPa
Step 3: Calculate total pressure
Total pressure = 133.56 kPa + 77.94 kPa
Total pressure = 211.5 kPa
