- Dynamic equilibrium: Forward rate = backward rate in a closed system
- Le Chatelier's Principle: System shifts to oppose any change
- Temperature ↑: Shifts in endothermic direction (absorbs heat)
- Concentration ↑: Shifts away from the increased substance
- Pressure ↑: Shifts to side with fewer gas molecules
- Catalysts: Speed up both directions equally, no position change
- Concentrations constant but not necessarily equal at equilibrium
This key facts covers Key Facts: Equilibrium within Equilibrium (HT) for GCSE Chemistry. Revise Equilibrium (HT) in Rates of Reaction for GCSE Chemistry with 23 exam-style questions and 18 flashcards. This is a high-frequency topic, so it is worth revising until the explanation feels precise and repeatable. It is section 8 of 14 in this topic. Use this key facts to connect the idea to the wider topic before moving on to questions and flashcards.
Practice questions for Equilibrium (HT)
At dynamic equilibrium, which of the following is true?
Explain the effect of increasing temperature on the position of an equilibrium where the forward reaction is exothermic.
Quick recall flashcards
What conditions are needed for equilibrium?
A closed system (nothing can escape) and a reversible reaction
What does 'dynamic equilibrium' mean?
Forward and backward reactions happen at the same rate, so concentrations stay constant