IB Chemistry HL 2.3.4 Le Châtelier's principle
IB Chemistry HL 2.3.4 Le Châtelier's principle
Practise equilibrium shifts by using colour changes, gas mole counts and added chloride at constant temperature to separate position changes from K changes.
How this is tested
- from pink blue cobalt equilibrium, deduce [CoCl4]^2- formation is endothermic because heating favors blue
- predict higher pressure shifts equilibrium to the side with fewer gas moles, using the balanced equation
- separate shift from K change: adding Cl- shifts cobalt equilibrium right, but K stays constant if T is unchanged