2 mole of an ideal gas expanded isothermally and reversibly form 1L to 10L at 300 K. What is the enthalpy change:Correct answer is '0'. Can you explain this answer?

Question

Answer

Explanation:

Background Information:

Ideal gases follow the ideal gas law: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the universal gas constant, and T is temperature. For an isothermal process, the temperature stays constant, so the ideal gas law becomes PV = constant. For a reversible process, the system goes through a series of equilibrium states.

Enthalpy Change:

The enthalpy change for an isothermal and reversible process is given by the formula ΔH = 0. This is because, for an isothermal process, the temperature remains constant, and therefore, the internal energy of the system also remains constant. For a reversible process, the system goes through a series of equilibrium states, and there is no net change in the internal energy of the system. As a result, the enthalpy change is zero.

Application to the Question:

In this question, 2 moles of an ideal gas are expanded isothermally and reversibly from 1L to 10L at 300 K. Since the process is isothermal and reversible, the enthalpy change is zero. Therefore, the correct answer is 0.

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