1. + Chemical Energy

2. + Hmmm… Can you list 5 energy sources that do not directly produce carbon dioxide?

3. + Cellular Respiration C6H12O6 + 6O2  6CO2 + 6H2O What type of reaction does this look like? Where would energy go in this reaction?

4. + Fossil Fuels Why can fossil fuels be considered as a stored solar energy source?

5. + Types of Energy Kinetic Energy = energy of motion Thermal Energy = heat = movement of particles Potential Energy = stored

6. + Heat Heat = thermal = kinetic energy (using the definitions from the previous slide, explain to your partner how this could be)

7. + q = mc Δ t (heat formula) q = heat, kinetic energy (J or kJ) m = mass c = specific heat capacity – amount of energy involved in changing the temperature of 1g of a substance by 1 o C Δ t = change in temperature

8. + Think About THIS! If you are heating water and metal at the same temperature, which one will heat up faster? Why? How do we relate that to Heat Capacity?!

9. + EXOTHERMIC CHANGE System loses energy

10. + ENDOTHERMIC CHANGE System gains energy

11. + Example: Calculate the energy released when 250mL of water cools down from 98.0C to 25.0C. (c for water = 4.19J/g/C)

12. + Example 2: Calculate the heat capacity of a pot that water is heated in when the energy required to heat the 300gram pot from 12C to 112C is 11.7kJ.

13. + Remember: Endothermic reactions energy is ABSORBED (surroundings get cooler) Exothermic reaction energy is RELEASED (surroundings get warmer)

14. + Enthalpy Enthalpy involves only changes in POTENTIAL ENERGY changes in bond energy

15. + 3 types of enthalpy changes (Ep) phase change – intermolecular bonds (forces) chemical change – intramolecular bonds (ionic / covalent) nuclear change – protons and neutrons are altered

16. + For tomorrow… How can we relate HEAT or Thermal energy to ENTHALPY????