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Lead(II) nitrate decomposes when heated: 2Pb(NO₃)₂ → 2PbO + 4NO₂ + O₂ 33.1 g of lead(II) nitrate produces 20.0 g of lead(II) oxide. Calculate the percentage yield of lead(II) oxide.
89.7%
Method 1: C₂H₄ + H₂O → C₂H₅OH Method 2: C₆H₁₂O₆ → 2C₂H₅OH + 2CO₂ Which is better for the environment.
Method 1 (less waste produced)
CaCO₃ + 2HCl → CaCl₂ + CO₂ + H₂O 10.0 g of calcium carbonate reacts with 150 cm³ of hydrochloric acid of concentration 4.0 g/dm³. Calculate the volume of carbon dioxide produced at RTP.
0.197 dm³ (197 cm³)
2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O 25.0 cm³ of sodium hydroxide solution of concentration 8.0 g/dm³ reacts with excess sulfuric acid. Calculate the mass of sodium sulfate produced.
0.355 g
2Al + 6HCl → 2AlCl₃ + 3H₂ 5.4 g of aluminium reacts with excess hydrochloric acid. Calculate the volume of hydrogen produced at RTP.
7.2 dm³
Fe + S → FeS 14.0 g of iron reacts with 10.0 g of sulfur and produces 18.0 g of iron(II) sulfide. Calculate the percentage yield of iron(II) sulfide.
81.8%
Copper is produced from copper(II) oxide using carbon: 2CuO + C → 2Cu + CO₂ 20.0 g of copper(II) oxide reacts and produces 12.0 g of copper. Calculate the percentage yield of copper.
75%
Reaction 1: N₂ + 3H₂ → 2NH₃ Reaction 2: 2NH₄Cl + Ca(OH)₂ → 2NH₃ + CaCl₂ + 2H₂O Which is more sustainable.
Reaction 1
Zn + 2HCl → ZnCl₂ + H₂ 6.5 g of zinc reacts with 100 cm³ of hydrochloric acid of concentration 2.0 g/dm³. Calculate the volume of hydrogen produced at RTP.
0.066 dm³ (66 cm³)
Calcium carbonate decomposes according to the equation: CaCO₃ → CaO + CO₂ 12.5 g of calcium carbonate produces 5.0 g of calcium oxide. Calculate the percentage yield of calcium oxide.
71.4%
Mg + 2HCl → MgCl₂ + H₂ 5.0 g of magnesium reacts with 20.0 g of hydrochloric acid. Calculate the maximum mass of magnesium chloride that can be produced.
19.8 g
Calculate the concentration if 10 g of solute is dissolved in 1 dm³ of solution.
10 g/dm³
Which reactant determines the amount of product formed?
The limiting reactant
What is meant by “excess reactant”?
A reactant left over after the reaction/too much added
What does a low atom economy indicate?
A lot of waste is produced
Calculate the mass of sodium in 1 mole of NaCl (Na = 23).
23 g
What is meant by “conservation of mass”?
No atoms are lost or made. Mass of reactants = mass of products
Calculate the volume of 0.25 moles of gas at RTP.
6 dm³
What is the unit of mass used in quantitative chemistry?
grams (g)
Calculate the number of moles in 48 g of oxygen (Mr = 32).
1.5 mol
What does “theoretical yield” mean?
The maximum possible product
In the equation: 2H₂ + O₂ → 2H₂O, how many moles of water form from 2 moles of hydrogen?
2 moles
Calculate the mass of 0.5 moles of magnesium (Mr = 24).
12 g
What is the mass of 1 mole of hydrogen?
2 g
Convert 250 cm³ into dm³.
0.25 dm³
How many cm³ are in 1 dm³?
1000 cm³
Why is a high atom economy desirable?
Less waste
A reaction has an atom economy of 100%. What does this mean?
All products are desired
What is the formula for atom economy?
RFM of desired product ÷ total RFM of reactants) × 100
Why is percentage yield often less than 100%?
SPECIFIC product is lost during the reaction
Calculate the percentage yield if the theoretical yield is 20 g and the actual yield is 15 g.
75%
What is the formula for percentage yield?
(actual yield ÷ theoretical yield) × 100
What is meant by a limiting reactant?
The reactant that runs out first
What is the formula for calculating gas volume at RTP?
volume = moles × 24
Calculate the volume of 2 moles of gas at RTP.
48 dm³
What volume does one mole of gas occupy at room temperature and pressure (RTP)?
24 dm³
Calculate the concentration if 5 g of solute is dissolved in 2 dm³ of solution.
2.5 g/dm³
What is the formula to calculate concentration?
concentration = mass ÷ volume OR concentration = moles ÷ volume
What is the unit of concentration?
g/dm³ or mol/dm³
What is this number called? (6.02 × 10²³)
Avogadro constant
How many particles are in one mole of a substance?
6.02 × 10²³
Calculate the number of moles in 10 g of calcium carbonate.
0.1 mol
What is the RFM of oxygen?
32
What is the unit for amount of substance?
mol.
What is the formula to calculate the number of moles?
moles = mass ÷ RFM
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