SUMMARY
The discussion centers on calculating the Gibbs Free Energy (ΔG) for the reaction CaCO3 <-> CaO + CO2 at 900K, where the equilibrium pressure of CO2 is 0.0423 atm. The calculated ΔG is 5656.3 cal/mol, and the equilibrium constant K is derived from the pressure value. The relationship between ΔG and K is established through the equation ΔG = -RTlnK, confirming that the equilibrium pressure directly influences the Gibbs Free Energy of the reaction.
PREREQUISITES
- Understanding of Gibbs Free Energy and its significance in chemical reactions
- Familiarity with the equation ΔG = -RTlnK
- Knowledge of equilibrium concepts in thermodynamics
- Ability to interpret standard Gibbs Free Energy of formation values from tables
NEXT STEPS
- Study the derivation and applications of the equation ΔG = -RTlnK
- Learn how to calculate standard Gibbs Free Energy of formation for various compounds
- Explore the relationship between equilibrium constants and reaction favorability
- Investigate the impact of temperature on Gibbs Free Energy and equilibrium constants
USEFUL FOR
Chemistry students, educators, and professionals involved in thermodynamics, particularly those studying reaction equilibria and Gibbs Free Energy calculations.