Use of amount of substance in relation to volumes of gases — AQA GCSE Chemistry
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Use of amount of substance in relation to volumes of gases explained
This statement is the molar volume principle.
Read the full explanation
Under identical temperature and pressure, one mole of any gas fills the same volume, because gas volume depends on the number of particles and their spacing, not on particle mass or identity. At room temperature and pressure (about 20 °C and 1 atmosphere), that volume is approximately 24 dm³, so 24 dm³ equals 24 000 cm³. Consequently, equal moles give equal volumes: 0.5 mol of any gas occupies about 12 dm³, and 2 mol occupies about 48 dm³. The relationship is volume = moles × 24 dm³ when volume is in dm³ at r.t.p. This lets you compare reacting gas volumes directly from a balanced equation, because coefficients give mole ratios and therefore volume ratios for gases measured under the same conditions.
Your focus
- State that equal amounts in moles of gases occupy the same volume under the same conditions of temperature and pressure.
- Recall and use the molar gas volume of approximately 24 dm³ at room temperature and pressure.
- Calculate the volume of a gas from its amount in moles using volume = moles × 24 dm³ at r.t.p.
Use of amount of substance in relation to volumes of gases exam tips
Marking Points
- States that equal numbers of moles of any gas occupy equal volumes when temperature and pressure are the same.
- Recalls the molar gas volume at room temperature and pressure as approximately 24 dm³ per mole.
- Uses volume = moles × 24 dm³ to convert between amount in moles and gas volume at r.t.p.
- Explains that gas volume depends on number of particles and their spacing, not on the mass or identity of the gas particles.
- Applies the principle to compare volumes of different gases: equal moles give equal volumes under the same conditions.
Examiner Tips
- 💡Write the condition 'at room temperature and pressure' whenever you use the value 24 dm³, because the molar volume changes with temperature and pressure.
- 💡Convert mass to moles first using moles = mass ÷ relative formula mass, then multiply by 24 dm³ to find the gas volume at r.t.p.
- 💡For comparison questions, compare the number of moles of each gas rather than their masses, then state that equal moles occupy equal volumes under the same conditions.
Common Mistakes
- Thinking that equal masses of different gases occupy equal volumes; correct this by comparing moles, not grams, because equal moles occupy equal volumes.
- Using 24 dm³ without checking that the gas is measured at room temperature and pressure; correct this by stating the condition and converting if a different temperature or pressure is given.
- Mixing up dm³ and cm³; correct this by remembering 1 dm³ = 1000 cm³, so 24 dm³ = 24 000 cm³.