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Ideal gas

Ideal gas. Assumptions P articles that form the gas have no volume and consist of single atoms. Intermolecular interactions are vanishingly small. Ideal gas. Equations of state PV= NkT P= pressure V= volume N=number of particles of gas k= B oltzmann Constant= 1.38x10 -23 J/K

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Ideal gas

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  1. Ideal gas • Assumptions • Particles that form the gas have no volume and consist of single atoms. • Intermolecular interactions are vanishingly small.

  2. Ideal gas Equations of state PV=NkT P= pressure V= volume N=number of particles of gas k= Boltzmann Constant= 1.38x10-23J/K K=Kelvin temperature

  3. Ideal gas Equations of state PV=nRT P= pressure V= volume n=number of moles of gas R= Universal Gas Constant= K=Kelvin temperature

  4. Ideal gas Avogadro’s number

  5. Ideal gas Relationship between Avogadro’s number, Universal Gas constant, and Boltzmann constant.

  6. Kinetic –molecular theory • Many molecules are in a container and they behave like point particles.(No volume) • The molecules move around randomly, and obey Newton’s laws. • The only interactions that the molecules undergo are elastic collisions with each other and the walls of the container.

  7. Kinetic –molecular theory Pressure is a result of the molecules colliding with the walls of the container. As the number of molecules or thir average speed increases, the pressure increases.

  8. Kinetic –molecular theory Results of kinetic-molecular theory.

  9. Kinetic –molecular theory Results of kinetic-molecular theory.

  10. Kinetic –molecular theory Internal energy of an ideal monatomic gas..

  11. Kinetic –molecular theory Other gas laws – the amount of gas does not change

  12. Laws of Thermodynamics The first Law of Termodynamics – If U is the internal energy of a system, than DU=Q-W. If Q>0 System gains heat If Q<0 System loses heat If W>0 Work is done by the system If W<0 Work is done on the system

  13. Laws of Thermodynamics The first Law of Thermodynamics – If U is the internal energy of a system, than DU=Q-W

  14. Table 18-1Signs of Q and W

  15. Figure 18-1The Internal Energy of a System

  16. Figure 18-2Work and Internal Energy

  17. Laws of Thermodynamics At constant pressure, the work done by or on a system is W=PΔV The area under a PV curve represents work. If a process occurs at a constant volume, the work done during the process is 0.

  18. Figure 18-5A Constant-Pressure Process

  19. Example 18-2Work Area

  20. Laws of Thermodynamics Isothermal processes – these are processes that take place at a constant temperature. PV=constant

  21. Figure 18-8Isotherms on a PV Plot

  22. Laws of Thermodynamics Adiabatic processes – these are processes that take place without heat entering or leaving the system.

  23. Figure 18-9An Isothermal Expansion

  24. Figure 18-10aAn Adiabatic Process

  25. Figure 18-10bAn Adiabatic Process

  26. Conceptual Checkpoint 18-2 Page 578Which is the adiabatic curve?

  27. Figure 18-14A Comparison Between Isotherms and Adiabats

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