Year 12 · WACE / Chemistry
Flashcards and recall.
Make a short deck from material you need to recall without notes.
Try this with Chemistry
- Write one prompt per card. Use definitions, explanations or examples from your current topic.
- Answer aloud before turning the card. Split a card if it asks for several unrelated facts.
- Set aside missed cards and revisit them in a later session.
Recall topics
- What two conditions make a collision chemically effective?
- Why can a powdered solid react faster than the same mass in large pieces?
- How does increasing solution concentration influence reaction rate?
- What changes in the energy distribution when temperature rises?
- Why does compression often accelerate a reaction involving gases?
- What does a catalyst change on an energy profile?
- How is an initial gas-production rate obtained from a volume–time graph?
- What does a horizontal product-volume curve establish, and what does it not establish?
- Which variables should be controlled when testing the effect of solid particle size?
- Why do repeated measurements not remove a calibration error?
- What distinguishes a closed chemical system from an isolated system?
- What is dynamic equilibrium in a reversible reaction?
- Can a physical change reach dynamic equilibrium?
- Why is constant concentration compatible with continuing reaction?
- What happens initially if only reactants are placed in a closed reversible system?
- Can equilibrium be approached starting from products?
- What does equilibrium position describe?
- Why can escaping gas prevent a reversible mixture reaching its closed-system equilibrium?
- What evidence is stronger than colour alone for establishing equilibrium?
- How should a rate–time graph identify the moment equilibrium is established?
- How does Le Châtelier’s Principle describe an equilibrium disturbance?
- What is the equilibrium effect of heating an exothermic forward reaction?
- Why does adding a reactant leave K unchanged at fixed temperature?
- When does compression favour the product side of a gas equilibrium?
- Why does pressure not shift H₂(g) + I₂(g) ⇌ 2HI(g) under the ideal model?
- What is the effect of adding an inert gas at constant volume?
- Why must constant pressure be distinguished from constant volume when adding inert gas?
- What does continuous removal of a product do to a reversible synthesis?
- Why does adding more pure solid sometimes leave equilibrium unchanged?
- How does additional dissolved carbon dioxide affect carbonate availability in seawater?
- How is Kc written for N₂(g) + 3H₂(g) ⇌ 2NH₃(g)?
- Which species are omitted from the usual school equilibrium concentration expression?
- What does a large Kc imply?
- What does a small positive Kc imply?
- How does reversing a reaction equation change its equilibrium constant?
- What happens to K when every coefficient in the equation is doubled?
- Where are forward and reverse activation energies measured on an energy profile?
- How is reaction enthalpy read from an energy profile?
- Why is it incorrect to say a catalyst supplies the reaction’s activation energy?
- How can two reactions have similar equilibrium favourability but very different rates?
Resource inventory inspected 4 November 2026. The main ATARMAXXING study platform is separate from tutoring. Topic labels show what was found, not a guarantee of complete curriculum coverage or tutor availability.
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