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

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?)

A) The false statement is:

4. At 1 bar, a phase change can exist as an equilibrium at only one temperature.

B) The correct answer is:

5. None of the previous answers.

C) The false statement is:

4. ∆S provides a measure of useful work available from a chemical change.

A) To determine which statement is false, let's examine each option:

1. A spontaneous change occurs by itself without assistance. This statement is true. A spontaneous change is one that occurs naturally, without the need for external assistance.

2. The greater the statistical probability of a state, the greater is its entropy. This statement is also true. Entropy is a measure of the disorder or randomness in a system. The higher the statistical probability of a state, the more disorder there is, leading to a greater entropy.

3. A non-spontaneous change can only occur if it is driven by a spontaneous change. This statement is false. A non-spontaneous change can occur with assistance or external factors, such as adding energy or a catalyst. It does not necessarily require a spontaneous change to drive it.

4. At 1 bar, a phase change can exist as an equilibrium at only one temperature. This statement is true. At a specific pressure, a phase change between two states (such as solid to liquid or liquid to gas) can occur at a specific temperature, known as the equilibrium temperature.

5. A reaction cannot proceed in the forward direction at all if its ∆G° is positive. This statement is true. ∆G° represents the change in Gibbs free energy under standard conditions. If ∆G° is positive, it means that the reaction is not favorable in the forward direction and will not proceed spontaneously.

Based on this analysis, the false statement is:

3. A non-spontaneous change can only occur if it is driven by a spontaneous change.

B) Let's examine the options for the vaporization of water:

1. ∆H = ∆S. This statement is not necessarily true for the vaporization of water. ∆H represents the change in enthalpy, which is related to the heat transfer during a process, while ∆S represents the change in entropy. The relationship between ∆H and ∆S depends on the specific conditions of the process.

2. ∆G is negative at low temperatures, positive at high temperatures. This statement does not accurately describe the behavior of ∆G during the vaporization of water. The sign of ∆G depends on the temperature and pressure conditions, as well as the specific values of ∆H and ∆S.

3. ∆H and ∆S are positive. This statement is true for the vaporization of water. When water vaporizes, both ∆H and ∆S are positive. Heat is absorbed (endothermic process) and the disorder of the system increases, resulting in a positive change in entropy.

4. ∆H, ∆S, and ∆G are positive at all temperatures. This statement is not true. As mentioned, the signs of ∆H, ∆S, and ∆G depend on the specific conditions of the process and can vary with temperature.

Based on this analysis, the correct answer is:

3. ∆H and ∆S are positive.

C) Let's evaluate the statements about entropy:

1. An increase in entropy favors spontaneity. This statement is true. An increase in entropy indicates an increase in disorder or randomness, which is often associated with a spontaneous process.

2. S=0 at 0 K for any pure perfect crystalline substance. This statement is true. At absolute zero temperature, the particles in a crystalline substance are in their lowest energy state, resulting in minimal disorder and an entropy value of zero.

3. S is proportional to the statistical probability (randomness) of a system. This statement is true. Entropy is a measure of the statistical probability of the different microstates of a system. The higher the probability of different arrangements, the greater the entropy.

4. ∆S provides a measure of useful work available from a chemical change. This statement is false. ∆S represents the change in entropy during a process and does not directly determine the useful work available. ∆G (Gibbs free energy) is the thermodynamic quantity that provides information about the 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. This statement is generally true. In most cases, the entropy of a gas is greater than that of a liquid because gases have more freedom of motion and a greater number of possible energy states.

Based on this analysis, the false statement is:

4. ∆S provides a measure of useful work available from a chemical change.