Answer
(a) spontaneous at low temperatures and non-spontaneous at high temperatures.
(b) non-spontaneous at all temperatures.
Work Step by Step
(a) Since the number of moles of gas decreases, the change in entropy $\Delta S$ is negative.
With $\Delta H\lt0$ and $\Delta S\lt0$, this reaction should be spontaneous at low temperatures and non-spontaneous at high temperatures.
(b) Since the number of moles of gas decreases, the change in entropy $\Delta S$ is negative.
With $\Delta H\gt0$ and $\Delta S\lt0$, this reaction should be non-spontaneous at all temperatures.