Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change ( in kJ) for the process is
Question
Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change ( in kJ) for the process is
Solution
The enthalpy change for an ideal gas in an isothermal process is zero. This is because the change in enthalpy (∆H) is equal to the heat added to the system at constant pressure. However, in an isothermal process, the temperature is constant, and therefore, the internal energy of the system does not change. Since the change in internal energy (∆U) is equal to the heat added minus the work done by the system (Q - W), and ∆U is zero, the heat added to the system must equal the work done by the system. Therefore, the change in enthalpy, which is equal to the heat added at constant pressure, is also zero.
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