How does Gibbs free energy relate to work?
Just so, what does Gibbs free energy tell us?
The Gibbs free energy of a system at any moment in time is defined as the enthalpy of the system minus the product of the temperature times the entropy of the system. The Gibbs free energy of the system is a state function because it is defined in terms of thermodynamic properties that are state functions.
One may also ask, why is Gibbs energy important? Being able to calculate the Gibbs free energy is important because you can use it to determine how likely a reaction is to occur. Negative enthalpy and positive entropy favor a reaction going forward. When it is zero, the reaction is at equilibrium.
Herein, what is the difference between Gibbs free energy and standard free energy?
Free energy or Gibbs function is by definition g = h - Ts, where h is enthalpy (J/kmol), T is absolute temperature (K) and s is entropy (J/kmol. Standard (or absolute) enthalpy is defined as that based on a reference wherein the value is zero for the elemental substances.
Why Gibbs free energy is negative?
Explanation: Gibbs free energy is a derived quantity that blends together the two great driving forces in chemical and physical processes, namely enthalpy change and entropy change. If the free energy is negative, we are looking at changes in enthalpy and entropy that favour the process and it occurs spontaneously.