Equilibrium Revision Mindmap

Kp
1. It is the same as Kc, except Kp is for gases and involves partial pressures instead of concentrations.
2. Partial Pressure (p) = mole fraction x total pressure.
Kc
1. This is the equilibrium constant = [products] / [reactants]
2. Greater than 1, equilibrium lies to the right.
3. Less than 1, equilibrium lies to the left.
4. =0, equilibrium lies directly in the middle.
Effect of Temperature
1. Changing the temperature causes the value of Kc/Kp to change as temperature is a condition.
2. For an exothermic reaction: increasing temperature causes K to decrease. Decreasing temperature causes K to increase.
3. For an endothermic reaction: increasing temperature causes K to increase. Decreasing temperature causes K to decrease.
Effect of Concentration
1. Changing concentration doesn't affect the value of Kc.
Effect of Pressure
1. Changing pressure doesn't affect the value of Kc.
Effect of Catalyst
1. Adding a catalyst doesn't affect the value of Kc.
Equilibrium
1. Homogeneous: all species are in the same state.
2. Heterogeneous: species which make up the reactants and products are in different physical states.
3. An equilibrium is where the rate of the forwards reaction is equal to the reverse.
4. Requires: A closed system and a reversible reaction.
5. Le Chatelier's Principle: When a system at equilibrium is disturbed, equilibrium shifts to oppose this change.

Resource summary

	Created by Chloe Drewery over 6 years ago