Internal energy is the sum of all different types of energies associated with atoms and molecules such as electronic energy (Ee), nuclear energy (En), chemical bond energy (Ec), potential energy (Ep) and kinetic energy (Ek).
U = Ee + En + Ec + Ep + Ek
Change in internal energy can be when
The case in which a change of state is brought by doing work and transfer of heat,
Change in internal energy = heat absorbed + work done on the system
This gives the first law of thermodynamics:
Energy can neither be created nor be destroyed, although it may be changed from one form to another.
Pressure-volume work:
Work done when the gas expands or contracts against the external pressure (atmospheric pressure) is the pressure-volume work.
w = -PV
When the volume of a cylinder increases against a constant external pressure, V is positive and w is negative. So, as the volume of the cylinder expands, work is done on the surroundings by the system. Then the volume of a cylinder decreases under a constant external pressure, V is negative and w is positive. So, as the volume of the cylinder contracts, work is done on the system by the surroundings.
Free exapansion:
Expansion of a gas in vacuum (external pressure = 0) is called free expansion. No work is done whether the process is reversible or irreversible.
wirrev = -pexV = 0
We know that, U = q + w
For process at constant volume, U = qv , where qv is the heat supplied at constant volume.
Some important formulae:
Enthalpy:
Change in enthalpy (H) is a measure of heat evolved or absorbed in a reaction or process at constant temperature and constant pressure.
H = qp = U + pV
When H is negative, then reaction is exothermic, i.e. evolving heat.
When H is positive, then reaction is endothermic, i.e. absorbing heat.
At constant volume, ΔV = 0, then ΔH = ΔU = qv
So, qp = qv + pV
or qp = qv +ngRT
where ng represents number of moles of gaseous products minus the number of moles of gaseous reactants.