For a reaction that has an equilibrium constant of 6 × 10⁹,which of the following statements must be true? A)ΔS° is positive. B)ΔG° is negative. C)ΔG° is positive. D)ΔH° is negative. E)ΔH° is positive.

Question

Quizplus · Accepted Answer

For a reaction with an equilibrium constant (K) greater than 1 (6 × 10^19 in this case), ΔG° must be negative. This is because ΔG° = -RTlnK, and when K > 1, lnK is positive, making -RTlnK negative. This indicates that the reaction is spontaneous under standard conditions.

For a Reaction That Has an Equilibrium Constant of 6