1) Sulfur dioxide is a gas. You are given 0.5 mol of this gas at room temperature and pressure. What volume will it take up and what mass of gas do you have?
2) 5 moles of gold atoms have a mass of 984.8g. Calculate the mass of one gold atom.
3) One 63Cu atom has a mass of 1.045 x 10-22g. Calculate the mass of 3 moles of 63Cu atoms.
Chemistry?
2017-09-27 2:58 am
回答 (2)
2017-09-27 3:19 am
✔ 最佳答案
1) Supposing "room temperature and pressure" to be 20°C and 1 atm:V = nRT / P = (0.5 mol) x (0.08205746 L atm/K mol) x (20 + 273) K / (1 atm) = 12 L SO2
(0.5 mol) x (64.0638 g SO2/mol) = 32 g SO2
2)
(984.8 g) / (5 mol) / (6.022 x 10^23 atoms/mol) = 3 × 10^-22 g/atom
3)
(1.045 x 10^-22 g/atom) x (6.022 x 10^23 atoms/mol) x (3 mol) = 189 g
2017-09-27 3:17 am
1.
PV = nRT
Volume, V = nRT/P = (0.5 mol) × [0.08206 atm L / (mol K)] × (298 K) / (1 atm) = 12.2 L
Molar mass of SO₂ (sulfur dioxide) = (32.1 + 16.0×2) g/mol = 64.1 g/mol
Mass of SO₂ = (0.5 mol) × (64.1 g/mol) = 32.05 g
2.
Avogadro constant = 6.022 × 10²³ /mol
No. of gold atoms = (6.022 × 10²³ /mol) × 5 mol = 3.011 × 10²⁴
Mass of one gold atom = (984.8 g) / (3.011 × 10²⁴) = 3.271 × 10²⁴ g
3.
Avogadro constant = 6.022 × 10²³ /mol
Molar mass of ⁶³Cu = (1.045 × 10⁻²² g) × (6.022 × 10²³ /mol) = 62.93 g/mol
Mass of 3 moles of ⁶³Cu atoms = (62.93 g/mol) × 3 = 188.8 g
PV = nRT
Volume, V = nRT/P = (0.5 mol) × [0.08206 atm L / (mol K)] × (298 K) / (1 atm) = 12.2 L
Molar mass of SO₂ (sulfur dioxide) = (32.1 + 16.0×2) g/mol = 64.1 g/mol
Mass of SO₂ = (0.5 mol) × (64.1 g/mol) = 32.05 g
2.
Avogadro constant = 6.022 × 10²³ /mol
No. of gold atoms = (6.022 × 10²³ /mol) × 5 mol = 3.011 × 10²⁴
Mass of one gold atom = (984.8 g) / (3.011 × 10²⁴) = 3.271 × 10²⁴ g
3.
Avogadro constant = 6.022 × 10²³ /mol
Molar mass of ⁶³Cu = (1.045 × 10⁻²² g) × (6.022 × 10²³ /mol) = 62.93 g/mol
Mass of 3 moles of ⁶³Cu atoms = (62.93 g/mol) × 3 = 188.8 g
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