The point detailed in the question is the triple point of water on the phase diagram. At the triple point all three phases of a chemical coexist; as such the correct answer is solid, liquid, and gas. 

A physical change is a process where the physical properties of a substance are changed.  Here water undergoes a phase change from the more disordered liquid state to the more ordered solid state, which is indeed a physical change.  A chemical change describes when a substance undergoes a change in the identity of its constituent molecules.  Here although the water has gone from the liquid phase to the solid phase it is still composed only of water molecules so a chemical change has not occured.  Entropy describes the degree to which a system is ordered.  Here we do have a change in entropy becasue the liquid water was more disordered than the solid water. 

This is a description of condensation from the gas phase to the liquid phase, then freezing from the liquid phase to the solid phase.

At a pressure of one atmosphere, carbon dioxide can only exist in the solid phase or the gaseous phase. Solid carbon dioxide will sublimate at standard conditions.

Raising the temperature will simply make the carbon dioxide sublimate at a faster rate. In order to allow the solid carbon dioxide to melt into the liquid phase, the carbon dioxide must be subjected to a greater amount of pressure. This will shift equilibrium away from the gaseous state and toward the liquid state.

Whenever you see a problem like this, immediately draw a mental point on the phase diagram to establish your starting conditions. In our case, the conditions fall in the range of the liquid phase of the water. This allows us to eliminate some of our answer options.

Next, determine what change is occuring and on which axis the change is occuring. We are decreasing pressure, so you are going to need to move down on the y-axis towards 0. Draw an imaginary line from the initial point to where the final point should be. In our case, the final pressure is extremely small. This point is not on the y-axis, but we can use our inference/inductive skills to determine that we will pass through the solid phase (ice) as we approach the gas phase (water vapor). Even if you didn't know the water would become vaporized, based on the graph you knew that the liquid phase had to be followed by the solid phase, and only one answer choice has that option. 

We know that the temperature is well below selenium's boiling point, but because we do not know its melting point, we cannot be certain if the temperature has dropped low enough for the element to be a solid.

When matter changes from one physical state (solid, liquid, gas, or plasma) to a different physical state, a phase change is defined to have occurred.

When a solid changes to a gas, the phase change that occurred is defined as sublimation:

Solid  Gas

When the opposite occurs and a gas changes to a solid, the phase change is defined as deposition:

Gas  Solid

When a liquid changes to a gas, the phase change that occurred is defined as vaporization. It is worth noting that there are two types of vaporization: evaporation (when the phase change occurs below the boiling point for the substance) and boiling (when the phase change occurs at or above the substance's boiling point).

Liquid  Gas

When the opposite occurs and a gas changes to a liquid, the phase change is defined as condensation:

Gas  Liquid

When a liquid changes to a solid, the phase change that occurred is defined as freezing:

Liquid  Solid

When the opposite occurs and a solid changes to a liquid, the phase change is defined as melting:

Solid  Liquid

When a gas changes to a plasma, the phase change that occurred is defined as ionization:

Gas  Plasma

When the opposite occurs and a plasma changes to a gas, the phase change that occurred is defined as recombination.

Plasma  Gas

Some may find it easiest to remember the phase changes by memorizing them in pairs. For example freezing and melting both refer to phase changes between solids and liquids. Once that is memorized, the possible phase changes that you have to choose from is reduced from 8 to 2. Also, it may be helpful to think that all the phase changes involving a decrease in entropy (increase in order) deposition, condensation, freezing, and recombination sound like more orderly words than the phase changes involving an increase in entropy (decrease in order) sublimation, vaporization, melting and ionization.

This question is asking us about the effect that elevation has on the boiling point of water. In order to answer this, we need to have a fundamental understanding of what boiling is, and how it can be affected by factors such as elevation.

Boiling is a type of phase transition in which a liquid is converted into a gas. During this transition, the boiling point is defined as the temperature at which the vapor pressure of the liquid is exactly equal to the atmospheric pressure. Therefore, if the atmospheric pressure is lowered, which happens at increased elevations, then it becomes easier for the liquid to evaporate into the gas phase. Consequently, less energy (and a lower temperature) is needed to push the liquid into the gas phase. As a result, the boiling point of the solution is lowered at increased elevations.

The equation for boiling point elevation is .

Since all of the solutions are aqueous, we do not need to consider the boiling point elevation constant () when comparing the solutions. The two factors we need to consider are molality () and the van't Hoff factor () of the solute.

Glucose will not ionize in solution, sodium chloride will make two ions in solution, and magnesium chloride will make three ions in solution.

When multiplying the molality by the van't Hoff factor, we can determine that the magnesium chloride solution will elevate the boiling point by the highest number.

Since the glucose is nonvolatile, we can use the boiling point elevation equation to solve for the new boiling point.

Since glucose does not ionize in water, the van't Hoff factor is simply 1 for this problem. The molality can be found by the moles of solute per kilogram of solvent.

This means that the boiling point for the water will be elevated by 1.03^oC with the addition of the glucose. Since pure water has a boiling point of 100^oC, the boiling point for this solution is 101.03^oC.