1.4 g of acetone dissolved in 100 g of benzene gave a solution which freezes at 277.12 K. Pure benzene freezes at 278.4 K. 2.8g of solid (A) dissolved in 100 g of benzene gave a solution which froze at 277.76 K. Calculate the molecular mass of (A).
A
562
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
462
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
362
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
232
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
Open in App
Solution
The correct option is D 232 Here compare both the cases and get the answer.
How?
Let’s find out.
We know that ΔT=Kf×W2×1000Mw2×w1
Where ΔT = Depression in freezing point Kf = Molal depression constant of benzene W2 = Mass of solute Mw2 = Molecular mass of solute W1 = Mass of solvent
Case I: (278.4−277.12)=Kf×1.4×100050×100 1.28Kf×1458.....(i)
Case II: (278.4−277.76)=Kf×2.8×1000MwA×100 0.64=Kf×28MwA
Dividing Eq. (i) by Eq. (ii), we get MwA=232