The equation Delta(U) = Cvdelta(T) is universally applicable to ideal gases, as the internal energy (U) is solely a function of temperature (T). This principle holds true regardless of whether the gas is undergoing constant volume or variable volume processes, such as expansion or compression. The discussion highlights that even in scenarios where pressure changes, the internal energy remains unaffected, reinforcing the ideal gas behavior. This understanding is crucial for thermodynamics and the study of ideal gases.
PREREQUISITESStudents and professionals in physics and engineering, particularly those focusing on thermodynamics, ideal gas behavior, and energy transfer processes.
The internal energy of an ideal gas is a function only of temperature. We know this because, if you have a real gas at low pressure in half of a rigid container and vacuum in the other half, and you break the seal, after the system has re-equilibrated at a lower pressure, the temperature does not change. This shows that the internal energy does not depend on pressure. A real gas in the limit of low pressures is what we refer to as an ideal gas.Lairix said:I don't understand how Delta(U) = Cvdelta(T) is always true for Ideal Gases...Shouldn't this only be true for constant volume processes? Yet it seems to be used even when a gas is expanding or being compressed...
Any ideas...Thanks in advance.