Question

33.56 g of fructose (C6H12O6) and 18.88 g of water are mixed to obtain a 40.00 ml

solution.

a. What is this solution's density?

b. What is the mole fraction of fructose in this solution?

c. What is the solution's average molar mass?

d. What is the specific molar volume of the solution?

Answer 1

A. density of solution = mass/volume

= avg molar mass/volume = 42.30 / 0.040 = 1057.6 gm/L

moles of fructose = mass/molar mass = 33.56/180.16 = 0.186 moles

moles of water = 18.88/18 = 1.048 moles

B. moles fraction of fructose = 0.186 / 0.186+1.048 *100 = 0.15

mole fraction of water = 1.048/1.048+0.186 = 0.85

C. average molar mass = mole fraction*molar mass ] sum of all component

0.15*180.16 + 0.85*18 = 42.304 gms

D. specific molar volume = Volume / moles = 40/0.186 + 1.048 = 32.41 ml