Question

Dissolving 1.10 g of an unknown compound in 75.22 g of benzene reduces its freezing point from 5.53 \deg C to 4.92 \deg C. What is the molar mass of the unknown compound? Kf benzene = −5.12 \deg C. g/mol 4. If the freezing point depression of a 0.10 m aqueous solution of a solute can be expressed as \Delta Tf = −i0.186 \deg C. For the group of solutes given, which freezing points correctly matches the solutes dissolved in water? Kf for H2O = −0.186 \deg C/m A. CH3CH2OH, \Delta Tf = −0.930 \deg C B. MgSO4, \Delta Tf = −0.186 \deg C C. NH4NO3, \Delta Tf = −0.774 \deg C D. CaCl2, \Delta Tf = −0.558 \deg C E. C6H6, \Delta Tf = −0.297 \deg C

Name: dissolving 110 g of an unknown compound in 7522 g of benzene reduces its freezing point from 553 deg c to 492 deg c what is the molar mass of the unknown compound kf benzene 512 deg c gmol 4 24859
Uploaded: 2022-09-28T09:46:19-08:00
Duration: 5 min 14 s
Channel: Dj Tan
Description: dissolving 110 g of an unknown compound in 7522 g of benzene reduces its freezing point from 553 deg c to 492 deg c what is the molar mass of the unknown compound kf benzene 512 deg c gmol 4 24859

          Dissolving 1.10 g of an unknown compound in 75.22 g of benzene reduces its freezing point from 5.53 \deg C
to 4.92 \deg C. What is the molar mass of the unknown compound? Kf benzene = −5.12 \deg C.
g/mol
4. If the freezing point depression of a 0.10 m aqueous solution of a solute can be expressed as
\Delta Tf = −i0.186 \deg C. For the group of solutes given, which freezing points correctly matches the solutes
dissolved in water? Kf for H2O = −0.186 \deg C/m
A. CH3CH2OH, \Delta Tf = −0.930 \deg C
B. MgSO4, \Delta Tf = −0.186 \deg C
C. NH4NO3, \Delta Tf = −0.774 \deg C
D. CaCl2, \Delta Tf = −0.558 \deg C
E. C6H6, \Delta Tf = −0.297 \deg C

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Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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09/28/2022

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Dissolving 1.10 g of an unknown compound in 75.22 g of benzene reduces its freezing point from 5.53 \deg C to 4.92 \deg C. What is the molar mass of the unknown compound? Kf benzene = −5.12 \deg C. g/mol 4. If the freezing point depression of a 0.10 m aqueous solution of a solute can be expressed as \Delta Tf = −i0.186 \deg C. For the group of solutes given, which freezing points correctly matches the solutes dissolved in water? Kf for H2O = −0.186 \deg C/m A. CH3CH2OH, \Delta Tf = −0.930 \deg C B. MgSO4, \Delta Tf = −0.186 \deg C C. NH4NO3, \Delta Tf = −0.774 \deg C D. CaCl2, \Delta Tf = −0.558 \deg C E. C6H6, \Delta Tf = −0.297 \deg C