wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

The boiling point of benzene is 353.23 K. When 1.80 g of a non-volatile solute was dissolved in 90 g benzene, the boiling point is raised to 354.11 K. Calculate the molar mass of the solute. (Kb for benzene is 2.53Kkgmol1)


A

58.0gmol1

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B

68.0gmol1

No worries! We‘ve got your back. Try BYJU‘S free classes today!
C

78.0gmol1

No worries! We‘ve got your back. Try BYJU‘S free classes today!
D

48.0gmol1

No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is A

58.0gmol1


Given values are:
Tbenzene=353.00K;Kb=2.53Kkgmol1
Tb(solution)=354.00k
Wsolute=1.80g
Wsolvent=90g
The elevation in boiling point,ΔTb=Tb(solution)Tb(solvent)
=354.11353.23
=0.88K
Molar mass of solute is given as
Mwsolute=Kb×1000×WsolventΔTb×Wsolvent
Mwsolute=2.53×1000×1.800.88×90=58.0gmol1
Hence, the molar mass of solute is 58.0gmol1


flag
Suggest Corrections
thumbs-up
3
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Abnormal Colligative Properties
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon