At 37 °C, a solution of 47.2 g of a non-volatile solute dissolved in 109 mL of ethanol (C2H5OH, molar mass 46.07 g/mol) has a vapour pressure of 95.0 mmHg. Pure ethanol has a vâpour pressure of 115 mmHg and a density of 0.775 g/mL at this temperature. Determine the molar mass of the non-volatile solute.

The concentration of dissolved argon in water exposed to gaseous argon at a partial pressure of 101.3 kPa at 20 \deg C is 1.5 x 10-3 mol/L. Use Henry's law to determine the solubility of argon when its partial pressure is 50.3 kPa.

It is desired to prepare 2.5 m^3 of a 60 mol percent methanol - water solution. Determine the volumes of methanol and water required to be mixed at ambient temperature given that the partial molar volumes of methanol and water are 58.3x10^-6m^3/mol and 17.2 x 10 m^3/mol respectively. The density of the methanol is 782.51 kg/m^3. Do not use chatgpt. Thank you!

The partial pressure of a solution of 175 g of CaCl2 in 975 g of water at 25 0C is torr. Given that the density of the solution is 1.10 g/mL and the partial pressure of pure water at 25 °C is 23.76 torr

You dissolve 45.0 grams of Camphor [molar mass  (152.237 g = 1 mole)] in 336 grams of ethanol [ molar mass ( 46.069 g = 1 mole)].  What is the mole fraction of ethanol (solvent) of this solution.

The solubility of Ne in water at 25 °C is 2.1 × 10⁻⁴ M when the partial pressure of Ne is 0.20 atm. What is the value of the Henry's law constant for Ne?

9.)  Using the data below (tabulated at 25 °C), what is the vapor pressure, in kilopascals (kPa), of a solution formed by mixing 5.37 mol of iodomethane (CH3I) with 4.27 mol of trichloromethane (CHCl3) at 25 °C? Assume ideal behavior. Substance Vapor Pressure (kPa) Iodomethane 53.9 Trichloromethane 26.2

A researcher prepares a new compound and uses freezing point depression measurements to determine the molar mass of the compound.  He dissolves 1.852 g compound in 75.00 g of cyclohexane.  Cyclohexane has a freezing point of 6.50 °C and a freezing point depression constant of 20.2°C kg/mol.  The freezing point of the solution is measured as 2.65°C.  Calculate the molar mass of the new compound. Record your answer to 3 sig figs

Glycerin 1C3H8O32 is a nonvolatile nonelectrolyte with a density of 1.26 g>mL at 25 °C. Calculate the vapor pressure at 25 °C of a solution made by adding 50.0 mL of glycerin to 500.0 mL of water. The vapor pressure of pure water at 25 °C is 23.8 torr (Appendix B), and its density is 1.00 g>mL.

1-propanol (n-propanol) and 2-propanol (isopropanol) form ideal solutions in all proportions. Calculate the partial pressure and the mole fraction (y) of the vapor phase of each component in equilibrium with each of the given solutions at 25 °C. Pprop=20.9 Torr and Piso = 45.2 Torr at 25 °C. A solution with a mole fraction of Xprop = 0.238. Pprop= Piso = yprop= Viso = A solution with a mole fraction of Xprop = 0.476. Pprop= Piso = yprop= Viso = A solution with a mole fraction of Xprop = 0.714. Pprop= Piso = yprop= Viso = Torr Torr Torr Torr Torr Torr