For b, the question is asking you to compare the pressures you calculated in a) with the given equilibrium vapor pressures. Basically, you need to see how your calculated pressures compare to the equilibrium pressures, i.e., are they higher or lower?
For c, the equilibrium vapor pressure values given in b) indicate the pressure exerted by the methyl alcohol at these temperatures. So, the pressure you calculated in a) represents the total pressure exerted by the vapor, which includes both the methyl alcohol and any other gases present in the flask. Therefore, to find the pressure exerted by the methyl alcohol only, you should use the equilibrium vapor pressure values provided in part b) for 35 and 45 degrees C.
For d, you don't need an equation. You just need to think about what physical states (solid, liquid or gas) are possible for methyl alcohol at the temperatures given (35 and 45 degrees C). You can refer to the boiling point of methyl alcohol (64.7 degrees C) and the freezing point of methyl alcohol (-97.8 degrees C) to help you determine the physical states present at these temperatures. At 35 and 45 degrees C, it is likely that both liquid and vapor phases of methyl alcohol are present since both temperatures are between the freezing and boiling points.