Lecture 18: Case Study in Reacting Gas Mixtures  Introducing the Nernst Equation  Summary and Q&A
TL;DR
Analyzing the behavior of reacting systems of ideal gases and their composition using Gibbs free energy plots, and introducing the Nernst equation for electrochemistry.
Questions & Answers
Q: How does the composition of a reacting system of ideal gases affect the equilibrium conditions and driving forces?
The composition of the system, expressed as the number of moles of C (nC), determines the Gibbs free energy and the position of the reaction equilibrium. The reaction will proceed in the direction that minimizes the Gibbs free energy, and the equilibrium composition can be determined by plotting the Gibbs free energy versus composition.
Q: Is the reaction A + B > 2C exothermic or endothermic?
The reaction is exothermic, as evidenced by the shift of the equilibrium towards the left when the temperature is increased.
Q: How can the enthalpy of the reaction be estimated from the given data?
By calculating the equilibrium composition in terms of moles of C, and using Dalton's law to determine the partial pressures of each component, the change in the equilibrium constant with respect to temperature can be determined. From this, the enthalpy of the reaction can be estimated using the Nernst equation.
Q: How does the Nernst equation combine electrostatics and chemistry?
The Nernst equation relates the change in Gibbs free energy of an electrochemical reaction to the electrostatic work of moving charge across a potential difference. It combines the electrostatic potential (E) with the chemical reaction quotient (q) to calculate the cell voltage (epsilon) for a given redox reaction.
Summary & Key Takeaways

The lecture focuses on analyzing reacting systems of ideal gases, specifically the reaction of A + B > 2C, using plots of Gibbs free energy versus composition.

The composition of the system can be expressed in terms of a single variable, nC, and the equation can be plotted to determine equilibrium conditions and driving forces.

The lecture then introduces the Nernst equation, which combines electrostatics and chemistry to describe cell voltages in electrochemical reactions.