For this I/GCSE Chemistry blog post, we will focus on what the concept of dynamic equilibrium is, as well as some examples of this reaction.
Dynamic Equilibrium
Dynamic equilibrium is when a reversible reaction is happening both ways at the same time, at the same rate.
If you move the equilibrium, you change the rate of reaction.
- If the equilibrium moves to the right, you have more products. (the reactants are reacting faster)
- If the equilibrium moves to the left, you have more reactants. (the products are reacting faster)
- If you increase the pressure: the equilibrium will move to the side with least molecules.
- If you decrease the pressure: the equilibrium will move to the side with the most molecules.
- If you increase the temperature, there will be more products that are produced by an endothermic reaction.
- (This is because the reaction is trying to use up the extra heat, and it does so by putting the energy into making bonds.)
Example of reversible reactions
Dehydration of hydrated copper(II) sulfate
If you add water to copper sulphate you can make hydrated copper sulphate.
If you remove the water from hydrated copper sulphate you can make anhydrous copper sulphate.
Heat on ammonium chloride
When heated, ammonium chloride splits into to hydrogen chloride and ammonia.
Hydrogen chloride and ammonia can be reacted to make ammonium chloride
That is all for this post!
References:
https://www.google.com/url?sa=i&url=https%3A%2F%2Fwww.jove.com%2Fscience-education%2F11385%2Fdynamic-equilibrium&psig=AOvVaw1itBkr63OXIR6pUiUjqTwz&ust=1627988524040000&source=images&cd=vfe&ved=0CAsQjRxqFwoTCMiqrISYkvICFQAAAAAdAAAAABAP
https://www.google.com/url?sa=i&url=https%3A%2F%2Fwww.tutormyself.com%2Fedexcel-igcse-2017chem-318%2F&psig=AOvVaw1qtriWnrthg9MC5L0K0M8G&ust=1627988687077000&source=images&cd=vfe&ved=0CAsQjRxqFwoTCOCCrM2YkvICFQAAAAAdAAAAABAD
Drafted by Venetia (Chemistry)