SUMMARY
The net change of internal energy of the gas is zero in the scenario described due to the principles of thermodynamics. When the gas is heated at constant volume, energy is introduced as heat (dQ), which increases pressure. This energy is then converted into work (pdV) as the gas expands, but when the gas contracts freely at constant pressure and temperature, it loses an equivalent amount of energy through work (p(V2-V1)). Thus, the energy gained and lost balance each other out, resulting in no net change in internal energy.
PREREQUISITES
- Understanding of the first law of thermodynamics
- Familiarity with concepts of heat transfer and work in thermodynamic systems
- Knowledge of gas laws and behavior under constant volume and pressure conditions
- Basic principles of internal energy in thermodynamics
NEXT STEPS
- Study the first law of thermodynamics in detail
- Explore the concept of internal energy in ideal gases
- Learn about isothermal and isochoric processes in thermodynamics
- Investigate the implications of free expansion in thermodynamic systems
USEFUL FOR
Students and professionals in physics, particularly those studying thermodynamics, as well as engineers and scientists involved in energy systems and gas behavior analysis.