In thermodynamics , how ∆U, ∆H ,and ∆T can be zero for isothermal reversible expansion? Please answer me in detail . ?

Question

Answer

Del U depends on temperature for ideal gas.For isothermal process del T remains constant. so ,Del U nd del nrt both are 0.hence satisfies..

Answer

Yes.... and u also hv ∆H=∆U+nRT....as per this even Delta H becomes 0 fr isothermal process

Answer

Delta U is zero because in isothermal  process temperature  remains constant. By the same reason delta T is zero.

Answer

Isothermal Reversible Expansion

In thermodynamics, an isothermal reversible expansion refers to a process in which a system expands or contracts while maintaining a constant temperature. This type of expansion is often studied to understand the behavior of ideal gases and to determine the work done by or on the system.

∆U (Change in Internal Energy)

In an isothermal reversible expansion, the change in internal energy (∆U) of the system is zero. This is because the internal energy of an ideal gas depends only on its temperature, and since the temperature remains constant during the expansion, there is no change in internal energy.

Internal energy is a measure of the microscopic energy of the particles within the system, including their kinetic and potential energy. However, in an isothermal process, the change in internal energy is zero because the average kinetic energy of the gas particles remains constant.

∆H (Change in Enthalpy)

Similarly, in an isothermal reversible expansion, the change in enthalpy (∆H) of the system is also zero. Enthalpy is defined as the sum of the internal energy and the product of pressure and volume of the system.

Since the temperature remains constant during the expansion, the change in internal energy is zero as discussed earlier. Additionally, the pressure and volume of the system also change in such a way that the product of pressure and volume remains constant. As a result, the change in enthalpy is zero.

∆T (Change in Temperature)

During an isothermal reversible expansion, the change in temperature (∆T) of the system is also zero. This is because the process is specifically designed to maintain a constant temperature.

As the system expands or contracts, work is done on or by the system, and this work is responsible for the change in the system's internal energy. However, in an isothermal process, the work done is exactly balanced by the heat exchange with the surroundings, resulting in no net change in temperature.

Since the change in temperature is zero, it implies that the heat added to or removed from the system is precisely equal to the work done by or on the system. This balance between heat and work is achieved by slowly and reversibly changing the volume of the system while maintaining a constant temperature.

Conclusion

In summary, in an isothermal reversible expansion, the change in internal energy (∆U), enthalpy (∆H), and temperature (∆T) of the system are all zero. This is due to the constant temperature maintained during the process, which ensures that the average kinetic energy, as well as the product of pressure and volume, remain constant. Understanding these concepts is crucial in studying thermodynamics and the behavior of ideal gases.

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