Which statement is TRUE for the reaction A + B $\leftrightarrow$ C + D if its K_eq for the reaction is 10⁴? A) When the reaction has reached equilibrium, there will be significantly more A and B than C and D in solution. B) The formation of A and B will proceed at a high rate. C) The value of $\Delta$G'° will be large and positive. D) All of the statements are true. E) None of the statements is true.

Question

Quizplus · Accepted Answer

The equilibrium constant (K_eq) is a measure of the extent to which a reaction proceeds to completion. A K_eq of 10^14 indicates a reaction that strongly favors the products (C and D), not the reactants (A and B), contradicting statements A and B. A large and positive ΔG° would indicate a non-spontaneous reaction, but a K_eq of 10^14 suggests the reaction is highly spontaneous in the direction of C and D formation, making statement C incorrect.

Which Statement Is TRUE for the Reaction a + B ↔\leftrightarrow↔

Which Statement Is TRUE for the Reaction a + B $\leftrightarrow$