- #1
abdossamad2003
- 68
- 4
Why is this equation (red sign) written in constant volume and not in constant pressure?
This is totally incorrect. Irrespective of the process, the internal energy of an ideal gas depends only on temperature, and not volume.abdossamad2003 said:
See, e.g., here: https://en.wikipedia.org/wiki/Internal_energy#Internal_energy_of_the_ideal_gas. ##C_V## is the coefficient of proportionality between internal energy on one hand and number of moles and temperature of the gas on the other hand.abdossamad2003 said:
Adiabatic processes involve no heat exchange with the surroundings, which means the internal energy of the system remains constant. When dealing with adiabatic processes, it is more common to use constant volume because it simplifies the calculations and allows for a clearer understanding of the changes in the system's energy.
Using constant volume in the equation for adiabatic processes allows us to focus on the changes in the system's internal energy without the complication of work done against a varying pressure. This simplification helps to isolate the effects of the process on the system's energy state.
While adiabatic processes are typically analyzed using constant volume, they can technically occur at constant pressure as well. However, using constant volume simplifies the calculations and provides a clearer picture of the energy changes within the system.
Adiabatic processes involve no heat exchange with the surroundings, while isothermal processes occur at a constant temperature. This means that adiabatic processes result in changes in the system's internal energy, while isothermal processes maintain a constant internal energy state.
Adiabatic processes are important in thermodynamics because they allow us to study the changes in a system's internal energy without the complicating factor of heat exchange. By isolating the effects of work done on or by the system, we can better understand the behavior of gases and other systems under adiabatic conditions.