Enthalpy differential

The fundamental thermodynamic relations are fundamental equations which demonstate how the important thermodynamic quantities depend on variables that are measurable experimentally.

Notation:

1. \(d\) denotes an exact, path-independent differential.

Notes:

1. Entropy, pressure, and particle count are so called natural variables of enthalpy as a thermodynamic potential.

2. For a system with more than one type of particles, the last term can be represented as a sum over all types of particles, i.e. \(\sum_i \mu_i \, d N_i\).

Conditions:

1. The system is in thermal equilibrium with its surroundings.

2. The system is composed of only one type of particles, i.e. the system is a pure substance.

Links:

1. Wikipedia.

enthalpy_change

Infinitesimal change in enthalpy of the system.

Symbol:

dH

temperature

temperature of the system.

Symbol:

T

Latex:

\(T\)

Dimension:

temperature

entropy_change

Infinitesimal change in entropy of the system.

Symbol:

dS

volume

Volume of the system.

Symbol:

V

pressure_change

Infinitesimal change in pressure inside the system.

Symbol:

dp

chemical_potential

Chemical potential of the system.

Symbol:

mu

Latex:

\(\mu\)

particle_count_change

Infinitesimal change in the number of particles in the system.

Symbol:

dN

law

dH = T * dS + V * dp + mu * dN

Latex:

\[dH = T \, dS + V \, dp + \mu \, dN\]