In a redox reaction, which equilibrium direction does the more positive E° value move?

In a redox reaction, the E° value, or standard electrode potential, is a critical factor. A more positive E° value indicates a stronger tendency for that half-reaction to gain electrons, meaning it acts as a stronger oxidizing agent.

When considering the direction of equilibrium in a redox reaction, a more positive E° suggests that the half-reaction that is most favorable for reduction (gaining electrons) is occurring. Therefore, the equilibrium will shift to the right, favoring the formation of products from reactants. This shift indicates that the reaction is more likely to proceed in the direction where species with higher standard potentials are formed.

In summary, the correct answer illustrates the principle that a more positive E° indicates a stronger tendency for reduction, leading to a rightward shift in the equilibrium of the reaction.