The discussion centers on the relationship between total work, internal energy change, and heat flow in thermodynamics. It establishes that total work executed on a system is the sum of mechanical work and internal energy change, with the equation Q = ΔU - W illustrating this principle. Specifically, if the change in internal energy (ΔU) is one-third of the total work (W), then two-thirds of the work is lost as heat flow (Q). This highlights the importance of understanding energy transfer in thermodynamic systems.
PREREQUISITESThis discussion is beneficial for students of physics, engineers working with thermodynamic systems, and anyone interested in the principles of energy transfer and conservation in physical processes.
It means that 2/3 of the work done on the system has escaped the system as heat flow.Anonymous119 said:Ok, if it says that change of internal energy is part(for example 1/3) of TOTAL work executed over system(body). Does it mean that is TOTAL work indeed sums of every single work(mechanical work+internal energy change+...) ?