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Equilibrium Processes in Gases: Laws and Characteristics

This text explores different types of equilibrium processes in gases, including isochoric, isobaric, isothermal, and adiabatic processes. It discusses the laws governing these processes and their characteristics such as work done, heat transfer, and changes in volume. The graphic summary on a PV diagram illustrates the different process types and their relationships.

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Equilibrium Processes in Gases: Laws and Characteristics

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  1. Equilibrium Processes in Gases 1. law: V=const. Processes in Ideal Gases Q Equilibrium process: Quasi-static process which transforms the system through states of thermal equilibrium Slow (almost unchanging) with respect to the typical relaxation times of a system Equilibrium processes are represented by lines in the state space Constant volume (isochoric) processes: 0 No work done

  2. 1. law: P=const. m Q Constant pressure (isobaric) processes P=const. Isothermal processes Work done @ T=const. T=const.

  3. 1. law: Adiabatic processes: No heat heat transfer in or out of the system Q=0 How to realize an adiabatic process very good insulation 1 or no time for heat to be exchanged rapid changes in volume 2 0 V0 Note: although the constant volume specific heat appears, expression applies to any process that starts and ends in equilibrium In the limit V0 First order differential equation V0

  4. Solution of by integration with with different from constant above

  5. What is the work done in an adiabatic equilibrium process during entire adiabatic process Starting at P0 and V0

  6. Thigh Tlow Graphic summaryof various processes on a PV diagram: Constant pressure (isobaric) process Constant volume (isochoric) process adiabatic process Q=0 Constant temperature (isothermal) process Isotherms for reference Adiabat steeper than isotherm

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