A sealed flask contains a mixture of 1.0 mole of N2 and 2.0 moles of O2 at 25 °C. If the total pressure of this gas mixture is 6.0 atmospheres, what is the partial pressure of the N2?
a.
6.0 atm
b.
2.0 atm
c.
9.0 atm
d.
3.0 atm
chemistry help?
2016-05-30 4:12 pm
回答 (1)
2016-05-30 4:16 pm
Molar mass of Al(OH)₃ = (26.98 + 16.00×3 + 1.008×3) g/mol = 78.00 g/mol
No. of moles of Al(OH)₃ = (27.00 g) / (78.00 g/mol) = 0.346 mol
Mole fraction of N₂, X(N₂) = 1.0 / (1.0 + 2.0) = 1/3
Partial pressure of N₂ = P(total) × X(N₂) = (6.0 atm) × (1/3) = 2.0 atm
...... The answer is: b. 2.0 atm
No. of moles of Al(OH)₃ = (27.00 g) / (78.00 g/mol) = 0.346 mol
Mole fraction of N₂, X(N₂) = 1.0 / (1.0 + 2.0) = 1/3
Partial pressure of N₂ = P(total) × X(N₂) = (6.0 atm) × (1/3) = 2.0 atm
...... The answer is: b. 2.0 atm
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