1. Le Chatelier's Principle
If a system at equilibrium is altered in a way that disrupts the equilibrium, the system will adjust in such a way as to counter the change.
N2(g) + 3 H2(g) ⇆ 2 NH3(g) + energy

2. Rates of Reaction for Reversible Reactions

3. FACTORS AFFECTING EQUILIBRIUM
CONCENTRATION
TEMPERATURE
PRESSURE

4. 1. CONCENTRATION CONCENTRATION CHANGES FAVORING FORWARD REACTION:
Addition of more reactants;
Removal of some products

5. Effect of Increased Concentration on Equilibrium

6. Effect of Decreased Concentration on Equilibrium

7. N2(g) + 3 H2(g) ⇆ 2 NH3(g) + energy
Addition of N2 or H2 or removal of NH3 would result to an increase in NH3. 
Removal of N2 or H2 or addition of NH3 would result to an increase in N2 and H2. 

8. TEMPERATURE
Increasing temperature favors the forward reaction of endothermic reactions
Increasing temperature favors the backward reaction of an exothermic reactions

9. N2(g) + 3 H2(g) ⇆ 2 NH3(g) + energy
exothermic
Lowering of temperature would result to an increase in NH3. 
Increasing temperature would result to an decrease in NH3. 

10. PRESSURE
- Increasing pressure favors the direction of reaction which will produce lesser number of particles.

11. N2(g) + 3 H2(g) ⇆ 2 NH3(g) + energy
There are 4 moles of the reactant and 2 moles of the product.
Increasing pressure favors the formation of lesser number of moles therefore producing more NH3 and using up N2 and H2. 