Exam-style application: In an AP Chemistry applications of thermodynamics setting, use delta G, delta H, delta S, Kelvin, Q versus K, delta G standard, and electrochemical cell potential. In a galvanic cell, which way do electrons flow? State the setup, compute carefully, and interpret the result.

Exam-style application: In an AP Chemistry applications of thermodynamics setting, use delta G, delta H, delta S, Kelvin, Q versus K, delta G standard, and electrochemical cell potential. What happens to the equilibrium constant $K$ of an exothermic reaction as temperature increases? Provide a concise written explanation.

Exam-style application: In an AP Chemistry applications of thermodynamics setting, use delta G, delta H, delta S, Kelvin, Q versus K, delta G standard, and electrochemical cell potential. Calculate $\Delta G$ for a reaction at 298 K where $\Delta H = -120$ kJ/mol and $\Delta S = -150$ J/(mol·K). State the setup, compute carefully, and interpret the result.

Exam-style application: In an AP Chemistry applications of thermodynamics setting, use delta G, delta H, delta S, Kelvin, Q versus K, delta G standard, and electrochemical cell potential. A reaction has $K = 4.5 \times 10^5$ at 298 K. What can be said about $\Delta G^\circ$? Provide a concise written explanation.

Exam-style application: In an AP Chemistry applications of thermodynamics setting, use delta G, delta H, delta S, Kelvin, Q versus K, delta G standard, and electrochemical cell potential. Relate cell potential to Gibbs free energy. If $E^\circ_{cell} = +1.10$ V for a 2-electron process, calculate $\Delta G^\circ$. (F = 96485 C/mol) State the setup, compute carefully, and interpret the result.

Exam-style application: In an AP Chemistry applications of thermodynamics setting, use delta G, delta H, delta S, Kelvin, Q versus K, delta G standard, and electrochemical cell potential. Identify the signs of $\Delta H$ and $\Delta S$ for a process that is spontaneous only at low temperatures. Provide a concise written explanation.