Two moles of an ideal gas is expanded isothermally and...

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litres at $300 \mathrm{~K}$. The enthalpy change (in $\mathrm{kJ}$ ) for the process is [2004S]
(a) $11.4 \mathrm{~kJ}$
(b) $-11.4 \mathrm{~kJ}$
(c) $0 \mathrm{~kJ}$
(d) $4.8 \mathrm{~kJ}$

Key Concepts

Reversible Process

A reversible process is an idealized thermodynamic process that happens infinitely slowly so that the system remains in thermodynamic equilibrium at all times. This type of process is characterized by the absence of dissipative effects, allowing the system and its surroundings to be returned to their initial states with no net change.

Enthalpy

Enthalpy is a thermodynamic quantity defined as the sum of the internal energy of a system and the product of its pressure and volume (H = U + PV). For ideal gases, because internal energy is solely a function of temperature, an isothermal process results in no change in enthalpy, assuming the gas behaves ideally.

Ideal Gas

An ideal gas is a theoretical gas whose molecules have no interactions and occupy no volume. Its behavior is well described by the ideal gas law (PV = nRT), meaning that properties such as pressure, volume, and temperature are interrelated in a predictable way. For ideal gases, internal energy and enthalpy depend solely on temperature, not on pressure or volume.

Isothermal Process

An isothermal process is one in which the temperature of the system remains constant throughout. In the context of an ideal gas, this implies that the internal energy remains constant, since it is a function only of temperature. Thus, even though the gas may expand or contract, the energy change associated with these temperature-dependent properties is zero.

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