Equilibrium Revision Mindmap

Equilibrium Revision Mindmap

1. Kp

   • It is the same as Kc, except Kp is for gases and involves partial pressures instead of concentrations.
   • Partial Pressure (p) = mole fraction x total pressure.

2. Kc

   • This is the equilibrium constant = [products] / [reactants]
   • Greater than 1, equilibrium lies to the right.
   • Less than 1, equilibrium lies to the left.
   • =0, equilibrium lies directly in the middle.

3. Effect of Temperature

   • Changing the temperature causes the value of Kc/Kp to change as temperature is a condition.
   • For an exothermic reaction: increasing temperature causes K to decrease. Decreasing temperature causes K to increase.
   • For an endothermic reaction: increasing temperature causes K to increase. Decreasing temperature causes K to decrease.

4. Effect of Concentration

   • Changing concentration doesn't affect the value of Kc.

5. Effect of Pressure

   • Changing pressure doesn't affect the value of Kc.

6. Effect of Catalyst

   • Adding a catalyst doesn't affect the value of Kc.

7. Equilibrium

   • Homogeneous: all species are in the same state.
   • Heterogeneous: species which make up the reactants and products are in different physical states.
   • An equilibrium is where the rate of the forwards reaction is equal to the reverse.
   • Requires: A closed system and a reversible reaction.