The effect of changing conditions on equilibrium (HT only) — AQA GCSE Chemistry
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The effect of changing conditions on equilibrium (HT only) explained
At equilibrium, the mixture contains both reactants and products, but the proportions of each are not fixed.
Read the full explanation
They depend on the conditions under which the reaction takes place, especially temperature, pressure and concentration. Changing a condition alters the position of equilibrium, so the relative amounts of reactants and products settle at new constant values. For example, in the Haber process for ammonia, nitrogen and hydrogen react reversibly to form ammonia; at a higher pressure the equilibrium mixture contains a greater proportion of ammonia, while at a higher temperature the proportion of ammonia decreases. The relative amounts are therefore a consequence of the chosen conditions, not a universal constant.
Your focus
- Describe how the relative amounts of reactants and products at equilibrium depend on reaction conditions.
- Explain how a change in temperature or pressure alters the position of equilibrium.
- Apply the concept to an industrial equilibrium such as the Haber process.
The effect of changing conditions on equilibrium (HT only) exam tips
Marking Points
- States that the amounts of reactants and products at equilibrium are not fixed but depend on the reaction conditions.
- Identifies temperature, pressure and concentration as conditions that can affect the position of equilibrium.
- Explains that changing a condition shifts the position of equilibrium and changes the relative amounts of reactants and products.
- Applies the idea to an industrial example such as the Haber process, linking pressure or temperature to the proportion of ammonia formed.
- Recognises that the equilibrium mixture still contains both reactants and products, but in different relative amounts.
- Uses the term position of equilibrium correctly to describe the balance between reactants and products.
Examiner Tips
- 💡Name the specific condition being changed, such as temperature or pressure, and state how the relative amounts of reactants and products change.
- 💡Use a familiar industrial equilibrium such as the Haber process to illustrate the effect of conditions on relative amounts.
- 💡Avoid saying that equilibrium is destroyed; instead say that the position of equilibrium shifts to a new balance.
Common Mistakes
- Thinking that the relative amounts at equilibrium are always the same for a given reaction; the correction is that they depend on the conditions used.
- Confusing the rate of reaction with the position of equilibrium; the correction is that conditions can change both, but the position of equilibrium describes the relative amounts, not the speed.
- Assuming that changing conditions changes only the forward reaction; the correction is that both forward and reverse rates are affected and the system settles at a new equilibrium position.