P solution = X solvent * P0solvent
28.6 = X solvent *31.1
X solvent = 28.6/31.1 = 0.92
no of moles of water(solvent) = W/G.M.Wt
= 350/18 = 19.44moles
mole fraction of solvent = no of moles of solvent/ total no of moles
0.92 = 19.44/19.44 + y
0.92(19.44+y) = 19.44
y = 1.69moles
molar mass of y = 86.8/1.69 = 51.4g/mole
Problem #4: At 29.6 °C, pure water has a vapor pressure of 31.1 torr. A solution...
4.) Pure water has a vapor pressure of 31.1 torr at 30.1 °C. A solution is prepared by adding 90.8 g of unknown substance which is a nonvolatile and non-electrolyte to 375.0 g of water. The vapor pressure of the resulting solution is 29.5 torr. Calculate the molar mass of the unknown substance.
The vapor pressure of pure water at 25.0 °C is 23.76 torr. The vapor pressure of a solution containing 5.40 g of a nonvolatile substance in 90.0 g of water is 23.32 torr. What is the molecular weight of the solute?
An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 11.5 kJ/mol separation of solvent 21.8 kJ/mol formation of solute-solvent interactions -86.7 kJ/mol solute...
a) The vapor pressure of pure water at 30°C is 31.8 torr. An aqueous solution of urea had a vapor pressure of 29.3 torrat the same temperature. What is the mole fraction of urea in the solution? b) How many grams of sucrose, C12H22O11(MW=342), must be dissolved in 552 g H2O (MW=18.016) to give a vapor pressure 2.0 torr lower than of pure H2O at 20°C? The VP of H2O at 20°C is 17.5 torr.
A solution containing ethylene glycol and water has a vapor pressure of 4.87 torr at 10°C. Pure water has a vapor pressure of 9.21 torr at 10°C. What is the mole fraction of ethylene glycol in the solution? Be sure to report your answer to the correct number of significant figures.
7. The vapor pressure of water at 25.0°C is 23.8 torr. Determine the mass of glucose (molar mass = 180 g/mol) needed to add to 500.0 g of water to change the vapor pressure to 23.3 torr. (20 points) Thyroxine, an important hormone that controls the rate of metabolism in the body, can be isolated from the thyroid gland. If 0.455 g of thyroxine is dissolved in 10.0 g of benzene, the freezing point of the solution is found to...
Predict the vapor pressure in torr at 25 degrees C of a solution prepared by mixing 16.8 g sodium phosphate with 87.15 mL of water. Assume the density of water to be 0.977 g/cm3 . The vapor pressure of pure water at 25 degrees is 23.76 torr
Explain2 The vapor pressure of a solution containing 73.6 g glycerin (C_3H_8O_3, Molar mass 92.094) in 120.7 g of ethanol (C_2H_5OH, Molar mass = 46.068) is 169.3 torr at 50.0 degree C Calculate the vapor pressure of pure ethanol at 40.0 degree C assuming that glycerin is a nonvolatile, nonelectrolyte solute in ethanol.
Glycerin, C3HgO3, is a nonvolatile liquid. What is the vapor pressure of a solution made by adding 163 g glycerin to 338 mL H20 at 39.8°C? The vapor pressure of pure water at 39.8°C is 54.74 torr and its density is 0.992 g/cm² Psoin 28 torr
Calculate the vapor pressure (in torr) at 293 K in a solution prepared by dissolving 19.28 g of the non-volatile non-electrolye urea {CO(NH2)2} in 195 g of water. The vapor pressure of water at 293 K is 17.54 torr. Enter your answer to 2 decimal places.