1. 2 NH3 (g) + H2SO4 à (NH4)2SO4 (aq)
Warm-up
Use the balanced equation below to answer the question. NOTE: NOT AT STP!!!!!
2 NH3 (g) + H2SO4 à (NH4)2SO4 (aq)
Calculate the volume of NH3 (in liters) needed at 20ºC and 25.0 atm to react with 150 kg of H2SO4.

2. Warm-up
How many liters of water can be made from 55 g of oxygen gas and an excess of hydrogen at a pressure of 12.4atm and a temperature of 85°C?

3. Warm-up
How many liters of water can be made from 55 g of oxygen gas and an excess of hydrogen at a pressure of 12.4atm and a temperature of 85°C?
O2 + 2H2  2H2O

4. Equilibrium

5. Equilibrium
Some reactions have double arrows, which means the reaction happens in both directions until equilibrium is reached.

6. Equilibrium Expressions
Every equilibrium reaction is described by an equilibrium constant (K)
Equilibrium expressions describe the ratio of product concentrations to reactant concentrations at equilibrium. They do NOT include solids or liquids.
Equilibrium Expression:

7. Le Chatelier’s Principle Henry Louis Le Chatelier
Equilibrium
Le Chatelier’s Principle
Henry Louis Le Chatelier
“When any system at equilibrium is subjected to change in concentration, temperature, volume, or pressure, then the system partially readjusts itself to counteract the effect of the applied change and a new equilibrium is established”

8. Equilibrium
Reaction will shift toward the products (to the right) if you add reactants or remove products.
Reaction will shift toward the reactants (to the left) if you add products or remove reactants.
Increasing the pressure will shift toward the side with the fewest number of balanced gas molecules. Decreasing pressure will do the opposite.
Note: Heat is a product for exothermic reactions and a reactant for endothermic reactions.

9. You DO NOT need to complete this column

11. Equilibrium Demo N2O4 (g) ↔ 2 NO2 (g) Increase Temp:
Endothermic or Exothermic?