The discussion revolves around the concept of isothermal processes in thermodynamics, specifically focusing on the behavior of ideal gases, temperature constancy, and heat capacity at constant volume.
The conversation is active, with participants questioning assumptions about heat capacity and internal energy changes. Some guidance is provided regarding the relationship between heat flow and work in isothermal conditions, but no consensus has been reached on specific calculations or interpretations.
Participants are navigating the complexities of thermodynamic principles, particularly the definitions and implications of heat capacity and internal energy in the context of isothermal processes. There is an acknowledgment of the historical development of thermodynamic concepts and their implications for current understanding.
Unfortunately, thermodynamics was developed before everyone really understood what heat was. Heat, in thermodynamics, is really heat flow so the concept of storing "heat" doesn't really work.grscott_2000 said:Heat capacity is the ability of a system to store heat as the temperature changes. Ah... I think I see what you mean... Just because a systems temperature doesn't change, doesn't mean it doesn't have a heat capacity right? So I need to calculate the heat capacity at constant volume?
Correct. Are you trying to find the heat capacity of the gas at constant temperature?grscott_2000 said:If a system is isothermal it tells me that there is no change in temperature and therefore there is no change in the internal energy of the system.
I know that a change in internal energy = heat transfer + work. So if heat flow is applied to the system, then under normal conditions, the temperature would rise i.e, it would have greater internal energy. To prevent this, the volume would have to increase… Is this correct?