Dynamic Equilibrium: GCSE Chemistry Definition

What is a dynamic equilibrium?

In GCSE Chemistry, dynamic equilibrium occurs in reversible reactions, within a closed system.

Dynamic equilibrium occurs when reactants are converted to products at the same rate that products are converted to reactants. This means that the concentrations of reactants and products remain constant because the forward and backward reactions proceed at the same rate.

Why is dynamic equilibrium important?

Dynamic equilibrium is important because it helps us understand chemical reactions and how to manipulate conditions to favour a reaction. It has important industrial applications, particularly in processes that require the yield to be as high as possible.

For example, in the Haber process for producing ammonia:

N₂ (g) + 3H₂ (g)  2NH₃ (g)

Temperature and pressure are carefully controlled to maintain dynamic equilibrium, ensuring a continuous and efficient production.

Similarly, dynamic equilibrium principles are applied in the production of sulfuric acid in the Contact process, optimising the reaction for higher output.

Make sure you know which industrial processes your exam specification includes:

Dynamic Equilibrium Revision Resources to Ace Your Exams

To explore cracking further, you should check out the revision notes on dynamic equilibrium and practise our exam questions to ensure success. Flashcards on equilibrium are also a great way to revise the wider topic of equilibrium before an exam. 

Explore our GCSE Chemistry revision resources.