First law of thermodynamics

1. First law of thermodynamics

2. Thermal systems Classical mechanics • Thermal systems: • - deals with many individual objects • - conceptually different from mechanical systems • - don’t know the position, velocity, and energy of • any molecules or atoms or objects • - can’t perform any calculation on them • Sacrifice microscopic knowledge of the system, • using macroscopic parameters instead • - volume (V) • - temperature (T) • - pressure (P) • - number of particles (N) • - energy (E), etc. • Macroscopic systems with many individual objects: • - processes are often irreversible • - arrow of time does exist • - energy conservation is not enough to describe • the thermal states Thermal system

3. reservoir Heat Work Thermodynamic systems Isolated systemscan exchange neither energy nor matter with the environment. reservoir Heat Work Open systemscan exchange both matter and energy with the environment. Closed systems exchange energy but not matter with the environment.

4. Idea gas model Lattice model for solid state materials • The ideal gas model • all the particles are identical • the particles number N is huge • the particles can be treated as point masses • the particles do not interact with each other • the particles obey Newton’s laws of motion, but their motion is random • collisions between the particles are elastic The ideal gas equation of state: kB= 1.38  10-23 J/K

5. Internal energy • The internal energy of a system of N particles, • U, is all the energy of the system that is • associated with its microscopic components • when view from a reference frame at rest • with respect to the object. • Internal energy includes: • - kinetic energy of translation, rotation, and • vibration of particles • - potential energy within the particles • - potential energy between particles • Internal energy is a state function – it depends • only on the values of macroparameters (the • state of a system) For a non-ideal gas: For an ideal gas (no interactions): Monatomic: Diatomic:

6. Heat Heat and work are both defined to describe energy transferacross a system boundary. • Heat (Q): the transfer of energy across the boundary of a system due to a temperature difference between the system and its surroundings. • - Q > 0: temperature increases; heating process • - Q < 0: temperature decreases; cooling process • - (C: heat capacity) • Heat transfer mechanisms • - conduction: exchange of kinetic energy between • microscopic particles (molecules, atoms, and • electrons) through collisions • - convection: energy transfer by the movement of a • heated substance such as air • - radiation: energy transfer in the form of electromagnetic • waves • Work (W): any other kind of energy transfer across boundary heat

7. Quasi-static processes • Quasi-static (quasi-equilibrium) processes: • Sufficiently slow processes, and any intermediate state can be considered as at thermal equilibrium. The macro parameters are well-defined for all intermediate states. • The state of a system that participates in a quasi-equilibrium process can be described with the same number of macro parameters as for a system in equilibrium. • Examples of quasi-static processes: • - isothermal: T = constant • - isovolumetric: V = constant • - isobaric: P = constant • - adiabatic: Q = 0

8. Work done during volume changes Quasi-static process at each infinitesimal movement Work done by the gas as its volume changes from Vi to Vf

9. P i Pi f Pf Vi Vf V Work done during volume changes (cont.) • dV > 0: the work done on the gas is negative • dV < 0: the work done on the gas is positive In thermodynamics, positive work represents a transfer of energy out of the system, and negative work represents a transfer of energy into the system. P-V diagram The work done by a gas in the expansion is the area under the curve connecting the initial and final states

10. Work and heat are not state functions c a b • a. isobaric • b. isovolumetric a. isovolumetric b. isobaric isothermal • Because the work done by a system depends on the initial and final states and • on the path followed by the systems between the states, it is not a state function. • Energy transfer by heat also depends on the initial, final, and intermediate states • of the system, it is not a state function either.

11. When heat enters a system, will it increase the system’s internal energy? • When work is done on a system, will it increase the system’s internal energy? It depends on the path!

12. reservoir Heat Work The first law of thermodynamics • Two ways to exchange energy between a system • and its surroundings (reservoir): • heat and work • Such exchanges only modify the internal energy of • the system • The first law of thermodynamics: conservation of energy Q > 0: energy enters the system Q < 0: energy leaves the system W > 0: work done on the system is negative; energy leaves the system W < 0: work done on the system is positive; energy enters the system • For infinitesimal processes:

13. P i, f V Several examples Isolated systems: Adiabatic processes Cyclic processes Insulating wall initial state = final state Expansion: U decreases Compression: U increases The internal energy of an isolated systems remains constant Energy exchange between “heat” and “work”

14. reservoir During an isovolumetric process, heat enters (leaves) the system and increases (decreases) the internal energy. Heat Idea gas isovolumetric process Isovolumetric process: V = constant P 2 1 (CV: heat capacity at constant volume) V1,2 V

15. reservoir Heat Work During an isobaric expansion process, heat enters the system. Part of the heat is used by the system to do work on the environment; the rest of the heat is used to increase the internal energy. Idea gas isobaric process P Isobaric process: P = constant 2 1 (CP: heat capacity at constant pressure) V1 V2 V

16. Idea gas isothermal process 1 P Isothermal process: T = constant 2 V1 V2 V During an isothermal expansion process, heat enters the system and all of the heat is used by the system to do work on the environment. During an isothermal compression process, energy enters the system by the work done on the system, but all of the energy leaves the system at the same time as the heat is removed.

17. Idea gas adiabatic process Adiabatic process: Q = 0 P 2 1 V2 V1 V Idea gas: Adiabatic process:

18. Idea gas adiabatic process P 2 1 , and divided by let V2 V1 V

19. Idea gas adiabatic process P 2 1 V2 V1 V For monatomic gas,

20. Idea gas adiabatic process P 2 1 V2 V1 V or

21. Idea gas adiabatic process P 2 1 V2 V1 V During an adiabatic expansion process, the reduction of the internal energy is used by the system to do work on the environment. During an adiabatic compression process, the environment does work on the system and increases the internal energy.

22. Summary • Internal energy, heat, and work: • - internal energy is the energy of the system; a state function • - heat and work are two ways to exchange energy between the system • and the environment. They are not state functions and depend on the path • The first law of thermodynamics connects the internal energy with heat and • work: Quasi-static process Character isovolumetric V = constant isobaric P = constant isothermal T = constant adiabatic