Let's start with 3 & 4
You want molar mass of solute - that means you need g/mole
I will also tell you that water's boiling pt / freezing pt constants are: 0.52 C/molal
and 1.86 C/molal
Why did they have to tell you that it was a nonionic solution? This is very important. I'll cover just the basics here: in order for water to boil it's molecules have to have enough energy to break it's surface tension and become a gas. Now if you throw some solute in there, they (solute particles) get in the way of the water and it requires more energy to get the water to boil. Thus the boiling pt increases. In order for water to freeze the molecules have to get closer together (I don't want to get into the structure for ice & the whole density thing), but let's just say that the water has to get closer together. If there is solute there, they get in the way. So more energy has to be lost, before the water will freeze. Thus, the freezing pt of the solution is lowered.
Both Ideas deal with the number of particles of solute in the solution. You have to know if the solute will break apart or stay together. Ionic substances will disassociate and form more particles than a molecule (covalently bonded & won't disassociate).
With this in mind you need to know if the solute is ionic or molecular, how to determine molality and freezing/boiling pt depression/elevation.
show some work on these questions and post again, I'm sure someone will help.
here's a website that might: http://dbhs.wvusd.k12.ca.us/webdocs/Solutions/BP-Elev-and-FP-Lower.html