Thanks! Why would internal energy be equal for an ideal gas process??Chestermiller said:No. It means that u1=u2
For an ideal gas, the internal energy per unit mass is a unique physical property that depends only on the temperature, irrespective of the process. So, if the temperature is the same, the internal energy is the same.ScareCrow271828 said:Thanks! Why would internal energy be equal for an ideal gas process??
The gas behavior is considered ideal in Isotherm and Isenthelp processes because these processes involve constant temperature and no change in entropy, respectively. In an ideal gas, the particles do not interact with each other and there are no intermolecular forces, leading to predictable and consistent behavior.
The ideal gas law, PV = nRT, describes the relationship between pressure, volume, number of moles, and temperature of an ideal gas. This law is based on the assumptions of an ideal gas, such as the absence of intermolecular forces, and can accurately predict the behavior of gases in isothermal and isentropic processes.
No, real gases do not exhibit ideal behavior because they do not meet the assumptions of an ideal gas. In real gases, there are intermolecular forces and the particles do interact with each other, leading to deviations from ideal behavior.
The consequences of non-ideal behavior in gases can include deviations from the ideal gas law, differences in pressure and volume from predicted values, and the need for more complex equations to accurately describe the behavior of the gas. These deviations become more significant at high pressures and low temperatures.
When a gas deviates from ideal behavior, its behavior becomes more complex and less predictable. The gas may exhibit non-uniform properties, such as varying pressure and volume at different points within the system. In addition, the gas may experience phase changes or exhibit non-linear behavior, making it more difficult to accurately model and predict its behavior.