SUMMARY
The change in Gibbs Free Energy (ΔG) at equilibrium is definitively 0, which leads to the relationship -ΔH = TΔS. This indicates that while a reaction is at equilibrium, enthalpy (ΔH) and entropy (ΔS) can still change during the process, as seen in the melting of ice at 0 degrees Celsius. The system can temporarily deviate from equilibrium when external heat is applied, such as with a Bunsen burner, but ultimately returns to equilibrium, reaffirming that G, H, and S are state functions relevant only at the initial and final states of the system.
PREREQUISITES
- Understanding of Gibbs Free Energy and its significance in thermodynamics
- Knowledge of state functions in thermodynamic processes
- Familiarity with enthalpy (ΔH) and entropy (ΔS) concepts
- Basic principles of chemical equilibrium
NEXT STEPS
- Study the implications of Gibbs Free Energy in chemical reactions
- Explore the relationship between enthalpy and entropy in thermodynamic processes
- Investigate the concept of chemical equilibrium and its applications
- Learn about state functions and their role in thermodynamics
USEFUL FOR
Chemistry students, thermodynamics enthusiasts, and professionals in chemical engineering or physical chemistry who seek to deepen their understanding of equilibrium processes and thermodynamic principles.