Chemistry Class: Systems Outside Equilibrium

Key Concepts

• Systems Outside Equilibrium
  • Discussion on delta G (Gibbs Free Energy)
  • Use of the equation: ΔG = ΔG⁰ + RT ln(Q)
  • Introduction to electrochemistry and the Nernst Equation

Important Equations

• Gibbs Free Energy Equation

  • [ ΔG = ΔG^0 + RT \ln(Q) ]
  • Explanation that ΔG or E is non-zero when the system is outside equilibrium.
  • At equilibrium, these values are zero.

• Nernst Equation

  • Used in electrochemistry to relate the reduction potential of a cell to the standard electrode potential, temperature, and activities.

Main Theme

• Non-Equilibrium Systems
  • Systems are outside equilibrium when ΔG or E is non-zero.
  • Non-zero values indicate that the system is not at equilibrium.

Reaction Rates

• Discussion on taking further steps to understand systems outside equilibrium by exploring reaction rates.
• Interest in not just the energy extractable from a chemical reaction, but also the speed at which the reaction occurs.

Future Exploration

• Begin exploring the rates of reactions and their implications in systems outside equilibrium.