NEET Chemistry (general) MCQ Question
Which of the following statements regarding equilibrium and spontaneity are correct?
If ∆G° < 0, the reaction is spontaneous in the forward direction.
If K > 1, there are more reactants than products at equilibrium.
A negative value of ∆G° indicates products are favored at equilibrium.
If ∆G° > 0, the reaction cannot proceed in the forward direction under standard conditions.
Correct Answer
Detailed Explanation
According to the provided context, if ∆G° < 0, then the reaction is spontaneous and favors the formation of products, indicating K > 1. Option B is incorrect as K > 1 indicates more products than reactants, while statement C is true but redundant. Option D is misleading as a positive ∆G° indicates non-spontaneity under standard conditions, not that it cannot proceed at all.
Found an issue with this question?