Free Energy and the Equilibrium Constant

What is the algebraic relationship between the standard Gibbs free energy change (ΔG°) and the equilibrium constant (K) for a chemical reaction?

• ΔG° = RT / lnK

• ΔG° = -RT lnK

• ΔG° = K / (RT)

• ΔG° = RT + lnK

A chemical reaction exhibits a positive standard Gibbs free energy change (ΔG°). What does this imply about the reaction's spontaneity and the favored direction at equilibrium?

• The reaction is spontaneous and favors the formation of products.

• The reaction is non-spontaneous and favors the formation of products.

• The reaction is spontaneous and favors the formation of reactants.

• The reaction is non-spontaneous and favors the formation of reactants.

If the equilibrium constant (K) for a reversible reaction is significantly greater than 1, what can be inferred about the reaction's state at equilibrium?

• The concentration of reactants is much higher than products.

• The reaction is non-spontaneous under standard conditions.

• The concentration of products is much higher than reactants.

• The reaction is at equilibrium with equal concentrations of reactants and products.

Cellular respiration is an exergonic process that releases a substantial amount of free energy. How is this released energy typically utilized within biological systems?

• It is directly converted into kinetic energy for cellular movement.

• It is stored as thermal energy to regulate body temperature.

• It is coupled with endergonic reactions, such as the synthesis of ATP from ADP and inorganic phosphate.

• It is transformed into electromagnetic radiation for intercellular communication.