How would the boiling point of a pure sample of water compare to the boiling point of a solution made from ethylene glycol and water?

The boiling point of water will be lower than the boiling point of the solution made from ethylene glycol and water.

Explanation:

It is all related to the colligative properties, in this case we talk about boiling point elevation.

The colligative properties are four: osmotic pressure, boiling point elevation, freezing point depression and lowering vapor pressure.

They all depends on the solute.  As we add more solute, the colligative property will change according to the relationship between the pure solvent and the solution. In boiling point elevation, the boiling point of the solution will be higher, the osmotic pressure will be also higher and in freezing point depression and lowering vapor pressure, solution will has a lower freezing point and a lower vapor pressure.

Relation between the colligative properties:

ΔTf / Kf = ΔTb / Kb = ΔP / P = π / R.T

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be