The First Law of Thermodynamics

1. Chapter 19 The First Law of Thermodynamics

2. Thermodynamics “A theory is the more impressive the greater the simplicity of its premises, the more different kinds of things it relates, and the more extended its area of applicability. Therefore the deep impression that classical thermodynamics made upon me. It is the only physical theory of universal content which I am convinced will never be overthrown, within the framework of applicability of its basic concepts.” A. Einstein

3. (Internal) Energy of a gas

4. P(atm) P(atm) A B 4 4 A B 2 2 Case 1 Case 2 3 9 3 9 V(m3) V(m3) Change in internal energy ΔU An monatomic ideal gas moves from state A to state B along the straight line shown.In which case is the change in internal energy of the system the biggest? 1. Case 1 2. Case 2 3. Same

5. P(atm) P(atm) A B 4 4 A B 2 2 Case 1 Case 2 3 9 3 9 V(m3) V(m3) Solution

6. Heat (reminder) Heat is the amount energy transfer due to a temperature difference. All other forms of energy transfer are classified as work. In the picture below, heat is flowing from the hot object to the cold object.

7. Energy transfer (Heat and work) Q: Heat going into the system W: Work done by the system

8. Work Done ON or BY the systemHeat into or out of the system (Work done by the system) = (−1) × (Work done on the system) (Heat going into the system) = (−1) × (Heat going out of the system)

9. The first Law of Thermodynamics ΔU = Q- W Work done by system Increase in internal energy Heat going intosystem U, Q, W are all in J. When work done by the system is positive, the system loses energy. When work done by the system is negative, the system gains energy.

10. Examples: Energy Transfer

11. Work by a gas

12. Work done and area under the curve

13. The sign of W If all the signs seems confusing, simply remember this: Expansion W >0 Compression W <0

14. W is path-dependent The work in each case is different, so you must be careful when calculating W.

15. Path dependence of W and Q

16. P(atm) P(atm) A B 4 4 A B 2 2 Case 1 Case 2 3 9 3 9 V(m3) V(m3) Example: Work A system moves from state A to state B along the straight line shown. In which case is the work done by the system the biggest? 1. Case 1 2. Case 2 3. Same

17. P P W = 0 W = PΔV 1 1 2 2 4 4 3 3 V ΔV = 0 V P PV = const W V Special Cases Isobaric: constant pressure Isochoric: constant volume Isothermal: constant temperature Adiabatic: no heat exchange Q =0

18. Summary

19. Work for special cases

20. Work for Isothermal case We used:

21. Imagine that an ideal monatomic gas is taken from its initial state A to state B by an isothermal process, from B to C by an isobaric process, and from C back to its initial state A by an isochoric process. Fill in the signs of Q, W, and ΔU for each step. P (atm) + + 0 A 2 -- -- -- + 0 + B 1 C 1 2 V (m3)

22. P 1 P 2 V V1 V2 Example: Isobaric Case Nmolecules of ideal gas is taken from state 1 to state 2 at constant pressureP, from V1to V2. Find T1, T2, ΔU, W, Q in terms of N, P, V1, V2.

23. Finding W and Q

24. A cyclic process A process is cyclic if after one cycle the system returns to the starting point. For a cyclic process, after one complete cycle, ΔU=0, but Q and W may not be zero.

25. Example: Cyclic Process W(CA) = − W(BC) = 0 W(AB) = W(ABCA) = + 0 - =+12kJ =

26. Heat Capacities of an Ideal Gas

27. Constant volume vs constant pressure

28. Ratio of Heat capacities γ

29. Adiabatic process

30. Adiabatic Process (Cont.)

31. Adiabatic Process Adiabatic processes obey the following relation:

32. Example: Adiabatic compression A box of monatomic gas at pressure 1atm is compressed from 6m3 to 2m3adiabatically, find the final pressure. What if the compression is isothermal but not adiabatic?

33. W for adiabatic processes By definition Q=0 for adiabatic processes. To find W, one can simply apply the First Law:

34. Work for Adiabatic Processes (Details)

35. Alternative method