Hey guys! I have answers, but am confused. Please and thanks for any help!

Question

A) Which of the following is false?
1.A spontaneous change occurs by itself without assistance.
2.The greater the statistical probability of a state, the greater is its entropy.
3.A non-spontaneous change can only occur if it is driven by a spontaneous change.
4.At 1 bar, a phase change can exist as an equilibrium at only one temperature.
5.A reaction cannot proceed in the forward direction at all if its ∆G° is positive
(My maybe work: I think the answer is 3 because a non-spontaneous change could be driven by like energy, right?)

B) Vaporization of a sample of water is an example of a process for which
1.∆H = ∆S.
2.∆G is negative at low temperatures, positive at high temperatures.
3.∆H and ∆S are positive.
4.∆H, ∆S, and ∆G are positive at all temperatures.
5.None of the previous answers.
(Maybe work: I think possibly this is an equilibrium process, so the answer would be 1?)

C) Which statement is not true about entropy, S?
1.An increase in entropy favors spontaneity.
2.S=0 at 0 K for any pure perfect crystalline substance.
3.S is proportional to the statistical probability (randomness) of a system.
4.∆S provides a measure of useful work available from a chemical change.
5.For a given substance, the entropy of a gas is greater than the entropy of a liquid.
(My maybe work: I think the answer is 4 because I believe deltaG is what provides a measure of useful work available for change?)