What is Internal Energy-Definition And Example

The sum of all forms of molecular energies (kinetic energy and potential energy) of a substance is called Internal Energy.

Internal energy

In thermodynamics, we usually take the ideal gas as a working substance. As the molecules of an ideal gas are point masses, so they exert no force on one another. Thus the internal energy of an ideal gas system is generally the translational K.E of its molecules.

Since the temperature of a system is the average K.E of its molecules. Therefore, for an ideal gas system, the internal energy is directly proportional to its temperature.

Internal energy is a broad property. A thermodynamic process that defines internal energy is the transfer of matter or energy as heat or thermodynamic work. These processes are measured by changes in a wide range of system variables, such as entropy, volume, and molar composition. In many cases, it is not necessary to consider all the energies of the system itself, such as the static rest mass energies of its constituent materials.

A system is said to be closed if the movement of matter is impeded by an impermeable enclosing wall, and the first law of thermodynamics dictates that the change in internal energy is the energy input into the system as heat, and the system is its local area.

A system is said to be isolated if the surrounding walls do not allow matter or energy to pass through it, and its internal energy cannot change.

How to change internal energy

When a substance is heated, the energy of its atoms increases. It means that the heat is converted into internal energy. But internal energy can also be increased without giving heat to the system, such as when two bodies are rubbed, their internal energy is increased due to the work done. When an object slides over any surface and comes to rest due to frictional forces, the mechanical work done on the system or by the system is partially converted into internal energy.

Independent of path:

Internal energy does not depend on the path but it depends on the initial and final states of the system.

Internal energy Example

Consider a system that changes from P_a, and V_a, to P_b, and V_b, such that.

P_a =Initial Pressure

P_b=Final Pressure

V_a=initial volume

V_b=final volume

Experimentally it has been proved that the change in internal energy remains the same and does not depend on paths C₁ and C2. The internal energy of a system is denoted by ‘U.’ Like gravitational P.E., we always take the change in internal energy and not its absolute value.

ΔU=U_b – U_a

U_a=initial internal energy

U_b=final internal energy.