In free expansion, no work is done and no heat is exchanged, so the internal energy remains constant.

In an adiabatic compression, work is done on the gas, which increases its internal energy.

The First Law of Thermodynamics establishes the conservation of energy principle, stating that energy cannot be created or destroyed.

In an isobaric process, the work done by the gas is given by W = PΔV, where P is the pressure and ΔV is the change in volume.

The work done by a gas during expansion against a constant external pressure is given by W = PΔV, where P is the pressure and ΔV is the change in volume.

The work done by a gas during expansion at constant pressure is given by W = PΔV.

During isothermal expansion, the work done by the gas is equal to the heat absorbed, as the internal energy remains constant.

In an isochoric process, the volume remains constant, so no work is done by the system (W = PΔV = 0).

In an isochoric process, the volume remains constant, so no work is done by the system (W = PΔV = 0).

The work done by the system during expansion against a constant external pressure is given by W = PΔV.

In an isochoric process, the volume remains constant, which means no work is done on or by the gas. Therefore, the work done is zero.

An adiabatic process is one in which no heat is exchanged with the surroundings. Compressing a gas in a piston without heat exchange is an example.

A static process does not involve any change in state variables, hence it is not considered a thermodynamic process.

All the listed processes are governed by the First Law of Thermodynamics, so the answer is 'None of the above'.

The first law states that energy is conserved, and heat cannot spontaneously flow from cold to hot without work being done.

The first law of thermodynamics is a statement of conservation of energy, applicable to all thermodynamic systems.