find the molarity of bezene given the denisty of .8989 g/l and the boiling temp is 80.2 C and Kb= 2.53C kg/mol
You need to add the other details of the problem.
umm its says 5g of n2h4oc was dissolved in 100 gr of benzene
and the boiling temp is 82.3 C the 80.2 is for pure benzene
That helps. Will you check and tell me if you want the molality or the molarity?
Molarity
First note: Lower case letters won't get it in chemistry, unless they really ARE lower case. n2h4oc doesn't mean a thing to me. I will refer to it as the compound. Do you have a name for the n2h4oc?
Second note:I still don't understand the problem. The molarity of the compound can be determined without using the boiling point data. The molarity of the benzene (which I assume to be the solvent) makes no sense (unless the compound is the solvent).
N2H4OC its the solid being dissolved that's in the problem
You may not need the boiling point data i just figure i write it because it was in the problem
One more question? The solute USUALLY is the solid and the solvent USUALLY is the liquid. You want the molarity of the solid or the molarity of the benzene?
of benzene
I will assume when you say molarity of the benzene that you mean the molarity of the solution (which is benzene with the solution dissolved in it).
mols N2H4CO = grams/molar mass = 0.08333
mol.
molality = moles/kg solvent = 0.08333/0.1 kg solvent = 0.8333 m
Not you convert 0.8333 m to M.
Take 1 kg of the solution (which has a density of 0.8989 g/mL (surely it isn't g/L as in your initial post). That contains 0.8333*60 = 50 g N2H4CO. Add that to the 1000 g benzene and we have 50 g N2H4CO in 1050 g of the solution with a density of 0.8989 g/mL.
What is the volume of the solution?
volume = mass/density = 1050/0.8989 = 1,168 mL or 1.168 L. Then M = moles/L = ??. (0.8333/1.168). Check my work. This has been a confusing problem to me.