key term - Free Energy

Definition

Free energy is a thermodynamic potential that measures the usable work obtainable from a system at constant temperature and pressure. It reflects the balance between the system's enthalpy and entropy, enabling predictions about the spontaneity of processes. Free energy plays a crucial role in understanding how molecular movements, distributions, and transitions contribute to macroscopic properties of systems.

5 Must Know Facts For Your Next Test

1. The change in free energy (ΔG) determines whether a reaction will occur spontaneously; if ΔG is negative, the process is spontaneous.
2. Free energy incorporates both energy contributions and disorder (entropy), making it essential for predicting equilibrium states in chemical reactions.
3. At equilibrium, the free energy of the system is at a minimum, indicating no net change in the concentration of reactants and products.
4. Free energy is influenced by temperature; as temperature increases, the entropy contribution to free energy becomes more significant.
5. The concept of free energy can be applied to various processes, including chemical reactions, phase transitions, and biological systems, highlighting its versatility.

Review Questions

• How does free energy relate to the spontaneity of chemical reactions?
  • Free energy is crucial in determining the spontaneity of chemical reactions through its change (ΔG). When ΔG is negative, it indicates that the reaction can proceed spontaneously towards products without external input. This relationship highlights how both enthalpic and entropic contributions influence whether a reaction will occur naturally under given conditions.
• Discuss how changes in temperature affect free energy and its implications for chemical equilibrium.
  • Changes in temperature directly influence free energy by altering the entropy term in its equation. As temperature increases, the entropic contribution becomes more prominent, which can shift ΔG values. This impact on free energy can result in different equilibrium positions for reactions, leading to varying concentrations of reactants and products at different temperatures.
• Evaluate the role of free energy in biological processes, particularly in metabolism.
  • In biological processes, free energy is pivotal for understanding metabolism. The concept explains how cells harness energy from nutrient breakdown through exergonic reactions that release free energy. This released energy drives endergonic reactions necessary for cellular functions. By analyzing pathways through changes in Gibbs free energy, one can assess how efficiently organisms convert nutrients into usable forms of energy to sustain life.

Related terms

Gibbs Free Energy:

A specific type of free energy that is defined as the difference between a system's enthalpy and the product of its temperature and entropy, used to determine the spontaneity of reactions.

Helmholtz Free Energy: Another form of free energy that is used primarily in systems at constant volume and temperature, defined as the internal energy minus the product of temperature and entropy.

Chemical Potential:

A measure of the change in free energy of a system when an additional particle is added, important for understanding phase transitions and reactions.