If ΔG is small and positive, which of the following statements is true? So before we solve this question, realize that we're dealing with reversible reactions, so they can go in the forward direction or the reverse direction. Now they're telling us ΔG is small, so that means it's close to 0 and it's positive, so that means it's slightly greater than 0, which means it's non spontaneous. And when we say that, we mean non spontaneous in the forward direction.
But remember we're dealing with reversible reactions when we talk about Gibbs free energy. So if you're non spontaneous in the forward direction, that means that you are spontaneous in the reverse. So let's see what makes the most sense. So it's positive. So that means it's going to be non spontaneous in the forward, which means that A&B are out because they wouldn't be spontaneous. In the forward. It will be spontaneous though in the reverse, which is what we said.
But now is it far from equilibrium or near equilibrium? Remember ΔG? When it's equal to zero we are at equilibrium. Since ΔG is small, that means it's a number that's pretty close to 0. So that means we would be near equilibrium. This would mean that option D is the correct answer.