An unknown soln of sugar in H2O boils at 102.4°C at 760 mm Hg pressure.?

Question

What mass of sugar would be contained per 1000g of water in this solution?

Answer 1

The elevation of the boiling point is

ΔTb = Kb*m

m=molality = mole solute/ kg solvent =>
m= mole solute *1000/G
where G is the mass of solvent in grams

also mole= g/MW where g is are the grams of solute and MW its molecular weight

so taking all of these into account we get

ΔTb= Kb*1000*g/(MW*G) =>

g= MW*G*ΔTb /(1000*Kb)=
= 342.3*1000* (102.4-100) / (1000*0.512)= 1604 g

Answer 2

760mm Hg is one atm or basically ISA sea level pressure. we know water boils at 100degrees C. so that leaves 2.4degrees remaining.