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

Rates of Reaction for Reversible Reactions

FACTORS AFFECTING EQUILIBRIUM CONCENTRATION TEMPERATURE PRESSURE

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

Effect of Increased Concentration on Equilibrium

Effect of Decreased Concentration on Equilibrium

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. 

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

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. 

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

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. 