1. Option B - Thermodynamics Year 13 SL Physics

2. Thermodynamics System – Environment of activity Surroundings – Factors impacting the system Boundary (wall) – System barriers

3. Work on a System Work done on a system or energy transferred to the system because of temperature differences result in the internal energy of that system increasing No change in state – Increase in Kinetic Energy Change in State – Increase in potential energy

4. Internal Energy Total Internal Energy of a System = – Total Potential Energy + Random Kinetic Energy of all particles

5. Ideal Gas Internal Energy is all kinetic

6. 0 th Law of Thermodynamics

7. 1 st Law of Thermodynamics Changes to Internal Energy – Doing work on the system Allowing the system to do work on the surroundings – Transferring energy to or from the system as a result of a difference in temperature

8. Q = ΔU + W

9. Types of Work Done Isobaric Changes – Constant Pressure Isothermal Changes – Constant Temperature Adiabatic Changes – Constant Energy Isovolumetric Changes – Constant Volume

10. Isobaric Changes Pressure is constant Q = ΔU + pΔV W is positive = expands W is negative = compressed

11. Isobaric Changes

12. Isothermal Changes Temperature is constant – So internal energy of the system remains constant Q = W – Where W = pΔV

13. Isothermal Change

14. Adiabatic Changes Constant Energy – No energy is transferred Usually contains a well insulated barrier between the system and surroundings

15. Isovolumetric Changes Constant volume – So no work done Q = ΔU

17. 2 nd Law of Thermodynamics It is impossible to transfer energy from a body at a lower temperature to one at higher temperature without doing work on the system It is impossible to extract energy from a hot reservoir and transfer this entirely into work. Law of Entropy

18. Entropy

19. We will do some examples and practice problems on Friday. But please learn these terms – That means you will need to study them Hubert