Thermodynamic Processes and Energy Changes Quiz

The First Law of Thermodynamics states that energy conservation holds, i.e., the total energy of an isolated system remains constant.

An adiabatic process is one where there's no exchange of heat between the system and its surroundings.

Work is not a state function in thermodynamics because it depends on the path taken during a process.

Entropy is measured in Joules per Kelvin (J/K) in the International System of Units.

The First Law of Thermodynamics states that the total energy of an isolated system remains constant.

Enthalpy is a state function because it depends only on the initial and final states of the system.

Isothermal process occurs at constant temperature, allowing for heat exchange to maintain the temperature.

The first law of thermodynamics states that the total energy of an isolated system remains constant; it cannot be created or destroyed, only transformed.

In an adiabatic process, there's no heat exchange between the system and its surroundings.

The Third Law of Thermodynamics states that the entropy of a perfect crystal approaches zero as the temperature approaches absolute zero.

The change in internal energy (∆U) is the sum of heat (Q) absorbed by the system and work (W) done on the surroundings, i.e., ∆U = Q - W.

An isochoric process, also known as constant volume process, involves no change in volume, hence no work is done.

The second law of thermodynamics states that the entropy of an isolated system never decreases, ΔS ≥ 0.

In an adiabatic process, there's no exchange of heat, hence the internal energy remains constant.

The change in internal energy (∆U) is equal to the heat (Q) absorbed by the system minus the work (W) done by the system.