18) Compute the vapor pressure of an ideal solution containing 92.1 g of glycerin, C,H,(OH),, and 184.4 g of ethanol, C,H,OH, at 40 °C. The vapor pressure of pure ethanol is 0.178 atm at 40 °C. Glycerin is essentially nonvolatile at this temperature. Since the solvent is the only volatile component of this solution, its vapor pressure may be computed per Raoult's law as: Psolution=XsolventP solvent First, calculate the molar amounts of each solution component using the provided mass data. 92.18C3HS(OH)3×ImolCsH:(OH}»92.094;C>H<(OH)=1.00molC3Hs(OH)3184.4gC2HsOH×ImolC:H:OH46.069;C:Hs OH=4.000molC2HsOH Next, calculate the mole fraction of the solvent (ethanol) and use Raoult's law to compute the solution's vapor pressure. XC:HSOH=4.000mo(1.00mol+4.000mol)=0.800Psolution=XsolventP solvent=0.800×1.78atm=0.142atm
18) Compute the vapor pressure of an ideal solution containing 92.1 g of glycerin, C,H,(OH),, and 184.4 g of ethanol, C,H,OH, at 40 °C. The vapor pressure of pure ethanol is 0.178 atm at 40 °C. Glycerin is essentially nonvolatile at this temperature. Since the solvent is the only volatile component of this solution, its vapor pressure may be computed per Raoult's law as: Psolution=XsolventP solvent First, calculate the molar amounts of each solution component using the provided mass data. 92.18C3HS(OH)3×ImolCsH:(OH}»92.094;C>H<(OH)=1.00molC3Hs(OH)3184.4gC2HsOH×ImolC:H:OH46.069;C:Hs OH=4.000molC2HsOH Next, calculate the mole fraction of the solvent (ethanol) and use Raoult's law to compute the solution's vapor pressure. XC:HSOH=4.000mo(1.00mol+4.000mol)=0.800Psolution=XsolventP solvent=0.800×1.78atm=0.142atm
Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:18) Compute the vapor pressure of an ideal solution containing
92.1 g of glycerin, C,H,(OH),, and 184.4 g of ethanol, C,H,OH,
at 40 °C. The vapor pressure of pure ethanol is 0.178 atm at 40
°C. Glycerin is essentially nonvolatile at this temperature.
Since the solvent is the only volatile component of this solution,
its vapor pressure may be computed per Raoult’s law as:
Psolution=XsolventP solvent
First, calculate the molar amounts of each solution component
using the provided mass data.
92.19C3H5(OH)3×ImolC3Hs(OH)s92.0949C:Hs(OH)s=1.00molC3Hs(OH)3184.4gC2HsOH×1molC2HsOH46.0698C:Hs
OH=4.000molC2HsOH
Next, calculate the mole fraction of the solvent (ethanol) and use
Raoult's law to compute the solution’s vapor pressure.
XC:HSOH=4.000mol(1.00mol+4.000mol)=0.800Psolution=XsolventP solvent=0.800x1.78atm=0.142atm
|Learn By Doing
e A solution contains 15.00 g of urea, CO(NH,), (a nonvolatile
solute) and 0.100 kg of water. If the vapor pressure of pure
/water at 25 °C is 23.7 torr, what is the vapor pressure of the
solution?
First, calculate the mole fraction of the water.
X120 =
Now use the mole fraction of the water to calculate the vapor
pressure of the solution.
P.
torr
solution
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At 40.0 °C the vapor pressure of pure water is 55.3 torr. A
saturated sucrose, C„H„O, is prepared by dissolving 238
g of sucrose in 100 g of water. What is the vapor pressure
of the saturated sucrose solution?
P.
=
solution
torr
A solution contains 20.00 g of urea, CO(NH,),, a
nonvolatile compound, dissolved in o.150 kg of water. If
the vapor pressure of pure water at 25 °C is 23.7 torr, what
is the vapor pressure of the solution?
P.
=
solution
torr
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