دالة الحالة، التفاضلات الدقيقة وغير الدقيقة

A state function is a thermodynamic property that depends solely on the system's current state, not on how it arrived there. Examples include internal energy (U), enthalpy (H), and entropy (S), represented by capital letters. Whether a system follows a linear or complex path, its state function values remain identical at the same initial and final conditions.

Path functions depend on the specific route a system takes between states, while state functions do not. Work (w) and heat (q) are path functions, represented by lowercase letters, and their values vary depending on the process pathway. In contrast, state functions like internal energy remain constant regardless of the path taken.

Exact differentials, like dU for internal energy, integrate to give path-independent values. Inexact differentials, like δw and δq for work and heat, integrate to give path-dependent values. When integrated, dU yields the change in internal energy (ΔU), while δw and δq yield absolute amounts of work and heat that depend on the process path.

Internal energy is a state function, depending only on initial and final states, not the process type. When a system transitions from adiabatic to nonadiabatic expansion while maintaining the same starting and ending states, the change in internal energy stays identical. However, the individual values of heat and work redistribute between the two paths.

For a cyclic process where the system returns to its initial state, the cyclic integral of any state function equals zero. This reflects the path-independent nature of state functions. Conversely, cyclic integrals of path functions like heat and work are not necessarily zero, since these quantities depend on the specific process pathway.

This notation convention distinguishes between two fundamental thermodynamic property types. Capital letters (U, H, S) denote state functions that depend only on system state. Lowercase letters (w, q) denote path functions whose values depend on the process route. This symbolic distinction helps clarify whether a quantity is path-independent or path-dependent.

Infinitesimal changes are represented as δw, δq, and dU respectively. The δ symbol denotes inexact differentials for work and heat, indicating path-dependence. The d symbol denotes the exact differential for internal energy, indicating path-independence. When integrated, δw and δq yield absolute amounts dependent on the process, while dU yields the change in internal energy independent of path.