A mixture of gases contains 4.08 g of N2, 4.10 g of H2, and 5.24 g of NH3. If the total pressure of the mixture is 3.13 atm, what is the partial pressure of each component?
PN2
PH2
PNH3
Chem help?
2018-01-24 10:25 am
回答 (1)
2018-01-24 10:39 am
Molar mass of N₂ = 14.0 × 2 g/mol = 28.0 g/mol
Molar mass of H₂ = 1.0 × 2 g/mol = 2.0 g/mol
Molar mass of NH₃ = (14.0 + 1.0×3) g/mol = 17.0 g/mol
In the mixture :
No. of moles of N₂ = (4.08 g) / (28.0 g/mol) = 0.146 mol
No. of moles of H₂ = (4.01 g) / (2.0 g/mol) = 2.005 mol
No. of moles of NH₃ = (5.24 g) / (17.0 g/mol) = 0.308 mol
Total no. of moles = (0.146 + 2.005 + 0.308) mol = 2.459 mol
Partial pressure = (Total pressure) × (Mole fraction)
Partial pressure of N₂, P(N₂) = (3.13 atm) × (0.146/2.459) = 0.186 atm
Partial pressure of H₂, P(H₂) = (3.13 atm) × (2.005/2.459) = 2.552 atm
Partial pressure of NH₃, P(NH₃) = (3.13 atm) × (0.308/2.459) = 0.392 atm
Molar mass of H₂ = 1.0 × 2 g/mol = 2.0 g/mol
Molar mass of NH₃ = (14.0 + 1.0×3) g/mol = 17.0 g/mol
In the mixture :
No. of moles of N₂ = (4.08 g) / (28.0 g/mol) = 0.146 mol
No. of moles of H₂ = (4.01 g) / (2.0 g/mol) = 2.005 mol
No. of moles of NH₃ = (5.24 g) / (17.0 g/mol) = 0.308 mol
Total no. of moles = (0.146 + 2.005 + 0.308) mol = 2.459 mol
Partial pressure = (Total pressure) × (Mole fraction)
Partial pressure of N₂, P(N₂) = (3.13 atm) × (0.146/2.459) = 0.186 atm
Partial pressure of H₂, P(H₂) = (3.13 atm) × (2.005/2.459) = 2.552 atm
Partial pressure of NH₃, P(NH₃) = (3.13 atm) × (0.308/2.459) = 0.392 atm
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