Final answer:
The Gibbs free energy (G), named after J. Willard Gibbs, predicts the direction of chemical reactions and determines equilibrium. It factors in enthalpy, temperature, and entropy. The Gibbs energy is linked to the equilibrium state, which maximizes entropy, and temperature influences the speed of reactions by affecting the energy barrier that molecules can surpass.
Step-by-step explanation:
Gibbs Free Energy and Chemical Reactions
Gibbs free energy, often abbreviated as G, was developed by J. Willard Gibbs. It's a thermodynamic potential that can predict the direction of a chemical reaction and determine the state of equilibrium. The Gibbs energy equation is given by G = H - TS, where H represents enthalpy, T temperature, and S entropy. The term ΔG, or change in Gibbs energy, indicates the amount of energy that is'shared and spread' which correlates with the increase in entropy.
The reaction Gibbs energy is the slope of the graph plotting Gibbs energy against the extent of reaction, reflecting the different compositions from pure reactants to pure products. During a reaction, the composition changes until equilibrium is reached. At equilibrium, the mixture of reactants and products has lower Gibbs energy than either pure state due to the increase in entropy. A reaction's ΔG can also help determine whether a reaction is spontaneous or not; if ΔG is negative, the reaction proceeds spontaneously.
Temperature also impacts chemical reactions. Reactions tend to occur more rapidly at higher temperatures as a larger fraction of molecules possess the kinetic energy necessary to surpass the energy barrier, as shown in energy distribution curves juxtaposed with potential energy diagrams.