Ammonia reacts with sulfuric acid to form the important fertilizer, ammonium sulfate. What mass of ammonium sulfate can be produced from 75.0 kL of ammonia at 10 °C and 110 kPa?
a) Write a balance chemical equation
b) Calculate the moles of ammonia.
c) Calculate the mass of ammonium sulfate.
Thank you!
Chem 20 Stoich Question- Urgent! Thank you!?
2016-06-06 9:44 pm
回答 (1)
2016-06-06 9:59 pm
(a)
2NH₃ + H₂SO₄ → (NH₄)₂SO₄
(b)
PV = nRT
n = PV/(RT)
No. of moles of NH₃, n
= PV / RT
= 110 × (75.0 × 1000) / [8.314 × (273 + 10)]
= 3506 mol
(c)
According to the equation in (a), mole ratio NH₃ : (NH₄)₂SO₄ = 2 : 1
No. of moles of NH₃ = 3506 mol
No. of moles of (NH₄)₂SO₄ = (3506 mol) × (1/2) = 1753 mol
From Wikipedia : Molar mass of (NH₄)₂SO₄ = 132.14 g/mol
Mass of (NH₄)₂SO₄ = (132.14 g/mol) × (1753 mol) = 232000 g = 232 kg
2NH₃ + H₂SO₄ → (NH₄)₂SO₄
(b)
PV = nRT
n = PV/(RT)
No. of moles of NH₃, n
= PV / RT
= 110 × (75.0 × 1000) / [8.314 × (273 + 10)]
= 3506 mol
(c)
According to the equation in (a), mole ratio NH₃ : (NH₄)₂SO₄ = 2 : 1
No. of moles of NH₃ = 3506 mol
No. of moles of (NH₄)₂SO₄ = (3506 mol) × (1/2) = 1753 mol
From Wikipedia : Molar mass of (NH₄)₂SO₄ = 132.14 g/mol
Mass of (NH₄)₂SO₄ = (132.14 g/mol) × (1753 mol) = 232000 g = 232 kg
收錄日期: 2021-04-18 14:56:50
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