Year 10 - Science
Moles and masses (RAM 1 d.p.)
Calculations involving masses
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This pupil-friendly study guide includes a unit summary, clear notes, common mistakes, and quick questions with answers.
Unit Summary
This unit covers writing chemical formulae, balancing equations, and using the conservation of mass. It includes calculating moles, empirical formulae, relative formula masses, and theoretical yields. Emphasis is on stoichiometry, concentration, gas volumes, and using standard form.
Lesson Summary
You will learn to calculate mass of a substance or the number of moles it contains from data.
Key Notes
- The number of particles (atoms, ions, molecules etc.) in one mole of a substance is always the same.
- The mass of one mole of a substance is equal to the relative mass of the substance measured in grams.
- Mathematical relationships are manipulated to process practical results, calculating the number of moles in a substance.
Vocabulary To Learn
- mole: 1 mole of a substance is 6.02 × 10²³ particles of it. The mass of a mole of a substance is its relative mass in grams.
- Avogadro's constant: Avogadro's constant is the number of particles in one mole of a substance (6.02 × 10²³ mol⁻¹).
- relative formula mass: The relative formula mass (RFM or Mᵣ) of a substance is the sum of the relative atomic masses of all the atoms in its formula.
Common Mistakes To Avoid
- Pupils struggle to link a mole to number of particles.
3 Quick Questions (With Answers)
1. Explain the scientific idea in this lesson using two key points.
The number of particles (atoms, ions, molecules etc.) in one mole of a substance is always the same. The mass of one mole of a substance is equal to the relative mass of the substance measured in grams.
2. Define this scientific word and use it in context. 'mole'
1 mole of a substance is 6.02 × 10²³ particles of it. The mass of a mole of a substance is its relative mass in grams. Include the word in a full scientific explanation, not as a single label.
3. Correct this common scientific misunderstanding.
Mistake: Pupils struggle to link a mole to number of particles. Correction: Use real world examples of converting volumes / masses into number of particles so pupils become more comfortable converting between moles, number of particles particles and masses.
More Lessons In This Unit
- Balancing equations Study Guide
- Conservation of mass Study Guide
- Converting between mass and volume using moles Study Guide
- Converting between mass and volume using moles (RAM 1 d.p.) Study Guide
- Deducing an empirical formula experimentally Study Guide
- Deducing an empirical formula experimentally: using moles Study Guide
- Determining an equation experimentally: magnesium oxide Study Guide
- Determining an equation experimentally: magnesium oxide (RAM 1 d.p.) Study Guide
- Determining an equation experimentally: sodium hydrogencarbonate Study Guide
- Determining an equation experimentally: sodium hydrogencarbonate (RAM 1 d.p.) Study Guide
- Determining an equation from given values Study Guide
- Determining an equation from given values (RAM 1 d.p.) Study Guide
- Empirical formula calculations Study Guide
- Empirical formula calculations: using moles Study Guide
- Gas volumes Study Guide
- Gas volumes (RAM 1 d.p.) Study Guide
- Limiting reactants Study Guide
- Limiting reactants (RAM 1 d.p.) Study Guide
- Mass in a chemical reaction Study Guide
- Mass in a chemical reaction (RAM 1 d.p.) Study Guide
- Mass in a chemical reaction: using moles Study Guide
- Mass in a chemical reaction: using moles (RAM 1 d.p.) Study Guide
- Moles and masses Study Guide
- Representations of a mole Study Guide
- Representations of a mole (RAM 1 d.p.) Study Guide
- The mole Study Guide
- The mole (RAM 1 d.p.) Study Guide
- Three types of chemical reaction Study Guide
- Uncertainties in measurements: chemistry Study Guide
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