Question

When K (>/=/<) 1, ΔG° is positive and the reaction is spontaneous in the reverse direction under standard conditions. a) Greater than 1

b) Greater than or equal to 1
c) Less than 1
d) Less than or equal to 1

Answer 1

For a positive ΔG°, indicating a non-spontaneous forward reaction under standard conditions, the equilibrium constant K is less than 1, signifying that the reverse reaction is spontaneous and reactants are favored.

Step-by-step explanation:

The student's question is regarding the relationship between the equilibrium constant (K) and Gibbs free energy change (ΔG°) for a reaction under standard conditions. The equilibrium constant (K) helps determine the direction of spontaneity for a reaction. If ΔG° is positive, it indicates that the reaction is not spontaneous in the forward direction under standard conditions. According to the provided reference material, this would also mean that K is less than 1, favoring the reactants over the products. Hence, the reaction would be spontaneous in the reverse direction.