Boiling Point Elevation/Freezing Point DepressionT = m Kwhere, for freezing point depression:T = T(pure solvent) - T(solution)and for boiling point elevation:T = T(solution) - T(pure solvent)m= (# moles solute / Kg solvent)Kb= boiling point elevation constant.Kf= freezing point depression constant.Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow.SolventFormulaKb(°C / m)Kf(°C / m) WaterH2O0.5121.86EthanolCH3CH2OH1.221.99ChloroformCHCl33.67 BenzeneC6H62.535.12Diethyl etherCH3CH2OCH2CH32.02 The boiling point of diethyl ether, CH3CH2OCH2CH3, is 34.500 °C at 1 atmosphere. Kp(diethyl ether) = 2.02 °C/mIn a laboratory experiment, students synthesized a new compound and found that when 13.52 grams of the compound were dissolved in 231.3 grams of diethyl ether, the solution began to boil at 34.933 °C. The compound was alsofound to be nonvolatile and a non-electrolyte.What is the molecular weight they determined for this compound ?g/mol The freezing point of water, H20, is 0.000 °C at 1 atmosphere. K(water) = -1.86 °C/mIn a laboratory experiment, students synthesized a new compound and found that when 14.51 grams of the compound were dissolved in 204.3 grams of water, the solution began to freeze at -2.198 °C. The compound was also foundto be nonvolatile and a non-electrolyte.What is the molecular weight they determined for this compound ?g/mol

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Boiling Point Elevation/Freezing Point Depression

T = m K

where, for freezing point depression:

T = T(pure solvent) - T(solution)

and for boiling point elevation:

T = T(solution) - T(pure solvent)

m	= (# moles solute / Kg solvent)
K_b	= boiling point elevation constant.
K_f	= freezing point depression constant.

K_b and K_f depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow.

Solvent	Formula	K_b(°C / m)	K_f(°C / m)
Water	H₂O	0.512	1.86
Ethanol	CH₃CH₂OH	1.22	1.99
Chloroform	CHCl₃	3.67
Benzene	C₆H₆	2.53	5.12
Diethyl ether	CH₃CH₂OCH₂CH₃	2.02

The boiling point of diethyl ether, CH3CH2OCH2CH3, is 34.500 °C at 1 atmosphere. Kp(diethyl ether) = 2.02 °C/m
In a laboratory experiment, students synthesized a new compound and found that when 13.52 grams of the compound were dissolved in 231.3 grams of diethyl ether, the solution began to boil at 34.933 °C. The compound was also
found to be nonvolatile and a non-electrolyte.
What is the molecular weight they determined for this compound ?
g/mol

The freezing point of water, H20, is 0.000 °C at 1 atmosphere. K(water) = -1.86 °C/m
In a laboratory experiment, students synthesized a new compound and found that when 14.51 grams of the compound were dissolved in 204.3 grams of water, the solution began to freeze at -2.198 °C. The compound was also found
to be nonvolatile and a non-electrolyte.
What is the molecular weight they determined for this compound ?
g/mol

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