Work through the list without notes. If you cannot do a statement, follow its link, then come back. Guide = study guide; Practice = practice questions.
Understanding
- I can name the two assumptions of the kinetic molecular theory that real gases break. (Guide: “Ideal gases are a model”)
- I can explain why attractions between particles make the measured pressure lower than the ideal value. (Guide: “Effect 1”; Practice Q3)
- I can explain why particle volume makes the measured volume or pressure higher than the ideal value at very high pressure. (Guide: “Effect 2”; Practice Q4)
- I can state the conditions that make a gas behave most ideally, and those that make it least ideal. (Guide; Practice Q1)
Calculation
- I can calculate an ideal pressure or volume with PV = nRT and compare it with a measured value. (Guide: Worked example 1; Practice Q5(a), Q7(a))
- I can calculate PV/nRT and say what a value below or above 1 means. (Guide: Worked example 2; Practice Q5(b), Q7(b))
- I can show with numbers why particle volume is negligible at ordinary pressure. (Guide: “Effect 2”; Practice Q7(d))
Reasoning
- I can rank gases by how much they deviate, naming the intermolecular forces involved rather than just saying “strong” or “weak”. (Guide: “Predicting which gas deviates more”; Practice Q2)
- I can explain why a gas becomes more ideal when it is heated. (Guide: Worked example 1; Practice Q5(d), Q6(a))
- I can explain the dip below 1 and the rise above 1 on a graph or table of PV/nRT against pressure. (Guide: Figure 2, Worked example 2; Practice Q6(b), Q6(c))
- I can justify which effect dominates with a particle-level argument that links to the measured pressure or volume. (Practice Q5(c), Q7(c))
- I can explain why PV/nRT = 1 at one pressure does not prove a gas is ideal. (Guide: Worked example 2)
All ticked? Move on to Topic 3.7, Solutions and Mixtures, or return to the course roadmap.