Introduction to Gibbs free energy | Applications of thermodynamics | AP Chemistry | Khan Academy

Recent questions

• What is Gibbs Free Energy?

  The Gibbs Free Energy, denoted as G, represents the energy available to do work in a system at constant temperature and pressure. It is a thermodynamic potential that combines enthalpy and entropy to predict whether a reaction will be spontaneous or non-spontaneous.

• How is delta G calculated?

  Delta G, the change in Gibbs Free Energy, is calculated using the formula delta G = delta H - (T * delta S), where delta H is the change in enthalpy, T is the temperature in Kelvin, and delta S is the change in entropy. This equation helps determine the spontaneity of a reaction based on the energy changes involved.

• What does delta G less than zero indicate?

  When delta G is less than zero, it signifies that a process is favored in the forward direction, indicating thermodynamic favorability. This condition suggests that the reaction will occur spontaneously, releasing energy in the process.

• What happens when delta G is greater than zero?

  If delta G is greater than zero, the process is favored in the reverse direction, indicating non-spontaneity in the forward direction. In this scenario, the reaction requires an input of energy to proceed, making it less likely to occur spontaneously.

• What is the significance of delta G at equilibrium?

  At equilibrium, when delta G equals zero, the process is balanced, and there is no net change occurring. This state indicates that the forward and reverse reactions are proceeding at equal rates, resulting in a dynamic equilibrium. The standard state conditions for substances play a crucial role in determining the equilibrium state of a reaction.