Given the reaction S + O2 ---> SO2
(a) How many grams of oxygen is needed to completely react 15.0 g of sulfur
to produce sulfur dioxide?
(b) What is the mass of sulfur dioxide produced?
SnO2 is reduced by carbon according to the this reaction:
SnO2 + C ---> Sn + CO2
(a) How many grams of CO2 are formed when 1.00 kilogram of tin is produced?
(b) How much SnO2 is required to produce 5.00 moles of tin?
2 KMnO4 + H2SO4 ---> K2SO4 + Mn2O7 + H2O
(a) How many moles of Mn2O7 can be formed from 16.0 g of KMnO4?
(b) How many grams of Mn2O7 can be formed from 30.0 g of KMnO4?
4 FeCr2O7 + 8 K2CO3 + O2 ---> 2 Fe2O3 + 8 K2CrO4 + 8 CO2
(a) How many grams of FeCr2O7 are required to produce 4.0 g of CO2? 12g
(b) How many grams of O2 are required to produce 10.0 g of Fe2O3?
(c) If 30.0 g of FeCr2O7 react, how many g of O2 will be consumed?
(d) How many g of Fe2O3 will be produced from 30.0 g of FeCr2O7? 8.82g
Need help with mass to mass stoichiometry for chemistry?
2018-03-08 12:54 pm
回答 (1)
2018-03-08 9:05 pm
1.
Molar mass of S = 32.0 g/mol
Molar mass of O₂ = 16.0 × 2 = 32.0 g/mol
Molar mass of SO₂ = (32.0 + 16.0×2) g/mol = 64.0 g/mol
S + O₂ → SO₂
Molar ratio S : O₂ : SO₂ = 1 : 1 : 1
(a)
No. of moles of S = 15.0/32.0 mol
No. of moles of O₂ = 15.0/32.0 mol
Mass of O₂ = (15.0/32.0 mol) × (32.0 g/mol) = 15.0 g
(b)
No. of moles of SO₂ produced = 15.0/32.0 mol
Mass of SO₂ produced = (15.0/32.0 mol) × (64.0 g/mol) = 30.0 g
====
2.
Molar mass of SnO₂ = (118.7 + 16.0×2) g/mol = 150.7 g/mol
Molar mass of Sn = 118.7 g/mol
Molar mass of CO₂ = (12.0 + 16.0×2) g/mol = 44.0 g/mol
SnO₂ + C → Sn + CO₂
Mole ratio SnO₂ : Sn : CO₂ = 1 : 1 : 1
(a)
No. of moles of Sn produced = 1000/118.7 mol
No. of CO₂ formed = 1000/118.7 mol
Mass of CO₂ formed = (1000/118.7 mol) × (44.0 g/mol) = 371 g
(b)
No. of moles of SnO₂ required = 5.00 mol
Mass of SnO₂ required = (5.00 mol) × (150.7 g/mol) = 754 g
====
3.
Molar mass of KMnO₄ = (39.0 + 54.9 + 16.0×4) g/mol = 157.9 g/mol
Molar mass of Mn₂O₇ = (54.9×2 + 16.0×7) g/mol = 221.8 g/mol
2 KMnO₄ + H₂SO₄ → K₂SO₄ + Mn₂O₇ + H₂O
Mole ratio KMnO₄ : Mn₂O₇ = 2 : 1
(a)
No. of moles of KMnO₄ reacted = 16.0/157.9 mol
No. of moles of Mn₂O₇ formed = (16.0/157.9 mol) × (1/2) = 8/157.9 mol
(b)
No. of moles of KMnO₄ reacted = 30.0/157.9 mol
No. of moles of Mn₂O₇ formed = (30.0/157.9 mol) × (1/2) = 15.0/157.9 mol
Mass of Mn₂O₇ formed = (15.0/157.9 mol) × (221.8 g/mol) = 21.1 g
====
4.
Molar mass of FeCr₂O₇ = (55.8 + 52.0×2 + 16.0×7) g/mol = 271.8 g/mol
Molar mass of O₂ = 16.0 × 2 g/mol = 32.0 g/mol
Molar mass of Fe₂O₃ = (55.8×2 + 16.0×3) g/mol = 159.6 g/mol
Molar mass of CO₂ = (12.0 + 16.0×2) g/mol = 44.0 g/mol
4 FeCr₂O₇ + 8 K₂CO₃ + O₂ → 2 Fe₂O₃ + 8 K₂CrO₄ + 8 CO₂
Mole ratio FeCr₂O₇ : O₂ : Fe₂O₃ : CO₂ = 4 : 1 : 2 : 8
(a)
No. of moles of CO₂ produced = 4.0/44.0 mol
No. of moles of FeCr₂O₇ required = (4.0/44.0 mol) × (4/8) = 2.0/44.0 mol
Mass of FeCr₂O₇ required = (2.0/44.0 mol) × (271.8 g/mol) = 12.4 g
(b)
No. of moles of Fe₂O₃ produced = 10.0/159.6 mol
No. of moles of O₂ required = (10.0/159.6 mol) × (1/2) = 5.00/159.6 mol
Mass of O₂ required = (5.00/159.6 mol) × (32.0 g/mol) = 1.00 g
(c)
No. of moles of FeCr₂O₇ reacted = 30.0/271.8 mol
No. of O₂ consumed = (30.0/271.8 mol) × (1/4) = 7.50/271.8 mol
Mass of O₂ consumed = (7.50/271.8 mol) × (32.0 g/mol) = 0.883 g
(d)
No. of moles of FeCr₂O₇ reacted = 30.0/271.8 mol
No. of Fe₂O₃ produced = (30.0/271.8 mol) × (1/2) = 15.0/271.8 mol
Mass of Fe₂O₃ produced = (15.0/271.8 mol) × (159.6 g/mol) = 8.81 g
Molar mass of S = 32.0 g/mol
Molar mass of O₂ = 16.0 × 2 = 32.0 g/mol
Molar mass of SO₂ = (32.0 + 16.0×2) g/mol = 64.0 g/mol
S + O₂ → SO₂
Molar ratio S : O₂ : SO₂ = 1 : 1 : 1
(a)
No. of moles of S = 15.0/32.0 mol
No. of moles of O₂ = 15.0/32.0 mol
Mass of O₂ = (15.0/32.0 mol) × (32.0 g/mol) = 15.0 g
(b)
No. of moles of SO₂ produced = 15.0/32.0 mol
Mass of SO₂ produced = (15.0/32.0 mol) × (64.0 g/mol) = 30.0 g
====
2.
Molar mass of SnO₂ = (118.7 + 16.0×2) g/mol = 150.7 g/mol
Molar mass of Sn = 118.7 g/mol
Molar mass of CO₂ = (12.0 + 16.0×2) g/mol = 44.0 g/mol
SnO₂ + C → Sn + CO₂
Mole ratio SnO₂ : Sn : CO₂ = 1 : 1 : 1
(a)
No. of moles of Sn produced = 1000/118.7 mol
No. of CO₂ formed = 1000/118.7 mol
Mass of CO₂ formed = (1000/118.7 mol) × (44.0 g/mol) = 371 g
(b)
No. of moles of SnO₂ required = 5.00 mol
Mass of SnO₂ required = (5.00 mol) × (150.7 g/mol) = 754 g
====
3.
Molar mass of KMnO₄ = (39.0 + 54.9 + 16.0×4) g/mol = 157.9 g/mol
Molar mass of Mn₂O₇ = (54.9×2 + 16.0×7) g/mol = 221.8 g/mol
2 KMnO₄ + H₂SO₄ → K₂SO₄ + Mn₂O₇ + H₂O
Mole ratio KMnO₄ : Mn₂O₇ = 2 : 1
(a)
No. of moles of KMnO₄ reacted = 16.0/157.9 mol
No. of moles of Mn₂O₇ formed = (16.0/157.9 mol) × (1/2) = 8/157.9 mol
(b)
No. of moles of KMnO₄ reacted = 30.0/157.9 mol
No. of moles of Mn₂O₇ formed = (30.0/157.9 mol) × (1/2) = 15.0/157.9 mol
Mass of Mn₂O₇ formed = (15.0/157.9 mol) × (221.8 g/mol) = 21.1 g
====
4.
Molar mass of FeCr₂O₇ = (55.8 + 52.0×2 + 16.0×7) g/mol = 271.8 g/mol
Molar mass of O₂ = 16.0 × 2 g/mol = 32.0 g/mol
Molar mass of Fe₂O₃ = (55.8×2 + 16.0×3) g/mol = 159.6 g/mol
Molar mass of CO₂ = (12.0 + 16.0×2) g/mol = 44.0 g/mol
4 FeCr₂O₇ + 8 K₂CO₃ + O₂ → 2 Fe₂O₃ + 8 K₂CrO₄ + 8 CO₂
Mole ratio FeCr₂O₇ : O₂ : Fe₂O₃ : CO₂ = 4 : 1 : 2 : 8
(a)
No. of moles of CO₂ produced = 4.0/44.0 mol
No. of moles of FeCr₂O₇ required = (4.0/44.0 mol) × (4/8) = 2.0/44.0 mol
Mass of FeCr₂O₇ required = (2.0/44.0 mol) × (271.8 g/mol) = 12.4 g
(b)
No. of moles of Fe₂O₃ produced = 10.0/159.6 mol
No. of moles of O₂ required = (10.0/159.6 mol) × (1/2) = 5.00/159.6 mol
Mass of O₂ required = (5.00/159.6 mol) × (32.0 g/mol) = 1.00 g
(c)
No. of moles of FeCr₂O₇ reacted = 30.0/271.8 mol
No. of O₂ consumed = (30.0/271.8 mol) × (1/4) = 7.50/271.8 mol
Mass of O₂ consumed = (7.50/271.8 mol) × (32.0 g/mol) = 0.883 g
(d)
No. of moles of FeCr₂O₇ reacted = 30.0/271.8 mol
No. of Fe₂O₃ produced = (30.0/271.8 mol) × (1/2) = 15.0/271.8 mol
Mass of Fe₂O₃ produced = (15.0/271.8 mol) × (159.6 g/mol) = 8.81 g
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