Glycerol HOCH2CH(OH)CH2OH is anonvolatile, water-soluble material. Its density is 1.25 g/mL.Predict the vapor pressure...
Glycerol HOCH2CH(OH)CH2OH is a
nonvolatile, water-soluble material. Its density is 1.25 g/mL.
Predict the vapor pressure of a solution of 251 mL of glycerol, in
394 mL of water, at the normal boiling point of water.
The vapor pressure of water at 45oC is 71.88 mmHg.
What is the vapor pressure of a sugar
(C12H22O11) solution made by
dissolving 54.18 g of sugar in 85.56 g of water?
The vapor pressure of ethonal (C2H5OH) is 672torr at
75°C. The vapor pressure of water is 289torr at the same
temperature.
Ethonal and water forms solution that behave like ideal solution.
Calc vapor pressure of ethonal and water above the solution at
75°C.
1) At 24 C the vapor pressure of water is 3 kPa. The vapor
pressure of water over a sample is 2 kPa, what is the water
activity of the sample?
2) The water activity above a saturated NaCl solution is 0.75.
If a sample is enclosed in a jar with the NaCl solution and
equilibrium is achieved, what is the water activity of the sample?
NaCl and the sample are in separate containers within the jar.
At 35ºC, the vapor pressure of pure water is 42.2 torr.
Calculate the vapor pressure of water at this temperature in a
solution that has a concentration of 6.5 M of NaCl. The density of
the solution is 1.09 g/mL
Given that the vapor pressure of water is 17.54 Torr at 20 °C,
calculate the vapor-pressure lowering of aqueous solutions that are
2.50 m in (a) sucrose, C12H22O11, and (b) calcium chloride. Assume
100% dissociation for electrolytes.
Given that the vapor pressure of water is 17.54 Torr at 20 °C,
calculate the vapor-pressure lowering of aqueous solutions that are
2.30 m in (a) sucrose, C12H22O11, and (b) aluminum chloride. Assume
100% dissociation for electrolytes.
Part A)
Calculate the vapor pressure of water above a solution prepared by
dissolving 29.5 g of glycerin in 140 g of water at 343 K
Part B) Calculate the mass of ethylene glycol that must be added to
1.00 kg of ethanol to reduce it's vapor pressure by 11.0 torr at
35° C. The vapor pressure of pure ethanol at 35°C is 1.00×10^2
torr.
Calculate the vapor pressure of water above a solution prepared
by dissolving 27.0 g of glycerin (C3H8O3) in 135 g of water at 343
K. (The vapor pressure of water at 343 K is 233.7 torr.)
Ph2o=?
Calculate the mass of ethylene glycol (C2H6O2) that must be
added to 1.00 kg of ethanol (C2H5OH) to reduce its vapor pressure
by 9.00 torr at 35∘C. The vapor pressure of pure ethanol at
35∘C is 1.00×102 torr.
m=?