A solvent (molar mass = 98.2 g mol-¹) has a vapour pressure of 4930 Pa at 20 °C; at 50 °C this increases to 1.94 x 104 Pa. A mass of 12.8 g of an unknown solute is dissolved in 100.0 g of the solvent. Assume the solute has negligible vapour pressure. Estimate the normal boiling point of the solution.

A solvent (molar mass = 98.2 g mol-¹) has a vapour pressure of 4930 Pa at 20 °C; at 50 °C this increases to 1.94 x 104 Pa. A mass of 12.8 g of an unknown solute is dissolved in 100.0 g of the solvent. Assume the solute has negligible vapour pressure. Estimate the normal boiling point of the solution.

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 128IP: Some nonelectrolyte solute (molar mass = 142 g/mol) was dissolved in 150. mL of a solvent (density =...

See similar textbooks

Similar questions

Some nonelectrolyte solute (molar mass = 142 g/mol) was dissolved in 150. mL of a solvent (density = 0.879 g/cm3). The elevated boiling point of the solution was 355.4 K. What mass of solute was dissolved in the solvent? For the solvent, the enthalpy of vaporization is 33.90 kJ/mol, the entropy of vaporization is 95.95 J/K mol, and the boiling-point elevation constant is 2.5 K kg/mol.
Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution of CCl4 and C6H6 at 25C. The vapor above the solution is collected and condensed. Using the following data, determine the composition in mole fraction of the condensed vapor. Substance Gfo C6H6(l) 124.50 kJ/mol C6H6(g) 129.66 kJ/mol CCI4(l) 65.21 kJ/mol CCI4,(g) 60.59 kJ/mol
There is a 15.85% by mass aqueous KCl (molecular weight 74.5513 g mol–1) solution at 25 °C. The density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Could you please find osmotic pressure?
(b) Surface sanitizers were prepared using ethyl alcohol/water and isopropyl alcohol/water solutions. An experiment was done to determine which composition would be most effective and as such two solutions were formulated: 70 % v/v ethyl alcohol and 70 % v/v isopropyl alcohol. Calculate the vapour pressure of these solutions and use your answer to reason which combination would stay on the surface longer. P° (Ethyl alcohol) = 12.4 kPa P° (Isopropyl alcohol) = 4.4 kPa P° (Water) = 2.4 kPa
The osmotic pressu re of an aqueous solution of urea at 300 K is 150 kPa. Calculate the freezing point of the same solution.
An ideal-dilute solution of chloroform and ethanol with a mole fraction of ethanol in the liquid phase Xeth = 0.9900 has a total vapour pressure of p = 17795 Torr. The vapour pressure of pure ethanol at this temperature is p*eth = 172.76Torr. (a) Use Raoult's law to calculate the partial pressure of ethanol in the vapour phase. (b) Hence determine the partial pressure of chloroform in the vapour phase . (c) Also calculate the mole fractions of chloroform and ethanol in the vapour phase. (d) Calculate the Henry's law constant for chloroform, Kchl at this temperature.
The partial molar volumes of water and ethanol in a solution with H₂O = 0.45 at 25 °C are 17.0 and 57.0 cm³ mol-¹, respectively. -1 Part A AV = Calculate the volume change upon mixing sufficient ethanol with 8.20 mol of water to give this concentration. The densities of water and ethanol are 0.997 and 0.7893 g cm 5, respectively, at this temperature. Express your answer to two significant figures and include the appropriate units. Submit μÅ Value Request Answer Units Review | Constants I Periodic Table . ?
A polymer of large molar mass is dissolved in the organic solvent m-cresol (C7H8O) at 25 °C, and the resulting solution rises to a final height of 13.4 cm above the level of the pure solvent, as solvent molecules pass through a semipermeable membrane into the solution. If the solution contains 5.24 g polymer per liter, calculate the molar mass of the polymer. Take the density of the solution to be 1.03 g cm-3.
A and B form ideal solution. If mole fraction of A in the solution is xĄ, what will be its mole fraction in vapour state? (vapour pressure of pure A and B are respectively P° and P) B
Vapour-liquid equilibrium of a two-component ideal solution of trichloroethene (C₂HC13) and trichloromethane (CHC13) is established at 25 °C. The mole fraction of CHCl3 in the vapour phase is 0.36. What is the mass fraction of C₂HCl3 in the liquid phase? Round your answer to two significant figures. The vapour pressures of trichloroethene and trichloromethane at 25 °C are: Pvap.C2HC13= 73.0 mmHg Pvap,CHC13= 199.1 mm Hg Number g C₂HCl3/g solution
SHOW COMPLETE SOLUTION AND WRITE LEGIBLY Predict the ideal solubility of lead in bismuth at 280 °C given that its melting point is 327 °C and its enthalpy of fusion is 5.2 kJ mol-1 .
The solubility of alum in 25 mL 1.4 M KOH plus 10 mL 9 M H2SO4 (our solution) is approximately 1.0 g at 1.0 °C, and 1.7 g at 6.0 °C. Estimate the amount of alum left in the solution if the temperature of the solution at the time of filtration was 5.0oC