1. ENERGY

2. Energy Ability to do work Kinetic Energy Energy of motion Potential Energy Stored energy Temperature Measure of the Average Kinetic Energy of the particles of a sample vs. Heat Kinetic energy of the particles (always flows from hot to cold)

3. Temperature Scales in Science Celsius : – The lowest point on the scale is -273.15 °C Absolute Zero Kelvin: – The lowest point on the scale is 0K Absolute Zero

4. NEVER, EVER USE FAHRENHEIT IN SCIENCE!!!!! IT IS THE “F” WORD!!!

5. What is Absolute Zero? The point at which no more heat can be removed from a system Almost no movement of molecules Theoretical temperature

6. Temperature Conversions Table T K= °C + 273 °C = K-273 (this is not on the table)

7. Energy Changes In a chemical or physical change there may be a transfer of energy (heat) Exothermic process: there is a release of energy (heat) Endothermic process: there is absorption of energy (heat)

8. Energy changes Exothermic Reactions will feel “hot” Endothermic Reactions will feel “cold”

9. What is heat? Bill Nye The Science Guy on Heat

10. Heating and Cooling Curves Shows the heating or the cooling of a specific substance Heat is added at a constant rate When a substance is undergoing a phase change THE TEMPERATURE DOES NOT CHANGE until the phase change is complete

11. Phase changes (Vocabulary) Melting (Fusion) Vaporization (l-g) Sublimation (solid  gas) Deposition (gas  solid) Freezing (fusion) Condensation (g-l)

12. Time (minutes) T e m p er at ur e ( ◦ C ) SOLID LIQUID GAS Melting Point Boiling Point Endothermic

13. Time (minutes) T e m p e r a t u re ( ◦ C) SOLID LIQUID GAS Freezing Point Condensation Point Exothermic

14. Time (minutes) T e m p er at ur e ( ◦ C ) Δ Kinetic Energy Kinetic Energy is constant

15. Time (minutes) T e m p er at ur e ( ◦ C ) Δ Potential Energy Potential Energy is constant

16. Time (minutes) T e m p er at ur e ( ◦ C ) q = mCΔT q = mH f q = mH v

18. Law of Conservation of Energy In any chemical or physical process, energy is neither created nor destroyed, it is merely transferred.

19. How is heat measured? Calorimetry – The precise measurement of heat flow into or out of a system. – The heat released by a system is equal to the heat absorbed by its surroundings – The heat absorbed by a system is equal to the heat released by the surroundings – A calorimeter is an insulated device used to measure the absorption or release of heat

20. Constant Pressure Calorimeter Most changes in the lab occur at constant pressure The heat of a system is it’s enthalpy (H) The heat released or absorbed by a system at constant pressure is equal to the system’s change in enthalpy (ΔH ) ΔH = q q= mC ΔT mass Specific heat Heat Change in temperature (Final Temperature – Initial Temperature)

21. ΔHΔHProcessHeat Positive (Final Temperature is higher than the initial temperature) EndothermicAbsorbed Negative(Final Temperature is lower than the initial temperature) ExothermicReleased

22. Calorimetry