What values of the equilibrium constant (K) and Gibbs free energy change (ΔG) are expected for a large positive standard cell potential (E°cell)?

• A. K > 1 and ΔG < 0
• B. K < 1 and ΔG < 0
• C. K = 1 and ΔG = 0
• D. K < 1 and ΔG > 0

Answer: (A)

Verified step by step guidance

1. Understand the relationship between the standard cell potential (E°cell), the equilibrium constant (K), and the Gibbs free energy change (ΔG). These are interconnected through thermodynamic equations.
2. Recall the Nernst equation at standard conditions: E°cell = (RT/nF) * ln(K), where R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred, and F is Faraday's constant. A large positive E°cell implies a large positive ln(K), which means K > 1.
3. Use the Gibbs free energy equation: ΔG° = -nFE°cell. A large positive E°cell results in a large negative ΔG°, indicating that the reaction is spontaneous under standard conditions.
4. Connect the concepts: A large positive E°cell suggests a strong tendency for the reaction to proceed in the forward direction, which corresponds to K > 1 and ΔG° < 0.
5. Summarize: For a large positive standard cell potential, the equilibrium constant K is greater than 1, indicating a product-favored reaction, and the Gibbs free energy change ΔG° is less than 0, indicating spontaneity.