The vapor pressure of water at a given temperature is 530 torr. What is the vapor...
1) The vapor pressure of pure water at 120 °C is 1250 torr. A solution of aniline and water has a vapor pressure of 1.2 atm at 120 °C. Assuming that Raoult’s law is obeyed, what is the mole fraction of aniline in the solution? Please show work. ----------------------------------------------------------------------- 2) Consider the following solutions, all in 1.0 kg of water: 1 mol of KBr, 1.5 mol CuCl2, 2 mol CH3COOH, and 1.5 mol CoCl3. The correct order for the respective...
Water has a vapor pressure of 47.1 torr at 37 oC. What is the vapor pressure of water over a solution that is made by dissolving 50.0 g of glycerin, C3H8O3, in 100.0 mL of water at 37 oC? The density of water at 37 oC is 0.993 g/mL. Please show all steps clearly :)
q16 An aqueous solution containing glucose has a vapor pressure of 19.9 torr at 25°C. What would be the vapor pressure of this solution at 45°C? The vapor pressure of pure water is 23.8 torr at 25°C and 71.9 torr at 45°C. Vapor pressure torr If the glucose in the solution were substituted with an equivalent amount (moles) of NaCl, what would be the vapor pressure at 45°C? Vapor pressure torr
The following data was obtained: atmospheric pressure: 752 torr water vapor pressure: 22 torr height of water column: 158 mm Calculate the partial pressure of the dry gas. Density of mercury if 13.6 g/cm3 and assume the desnity of the solution is 1.00 g/cm3/
If at a given temperature, the vapor pressure above pure benzene is 200.0 Torr and above pure toluene is 40.50 Torr and the mole fraction os toluene is 0.575, what is the partial pressure of each gas above the solution and what is the mole fraction of each gas in the vapor?
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.
The vapor pressure if ethanol (C2H5OH) is 672 torr at 75°C. The vapor pressure of water is 289 torr at the same temperature. Calculate the mole fraction of ethonal and water in a solution that is 12% ethanol by volume. Can any one help me step-by-step with this?
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...
What would be the vapor pressure of water at 96°C above a solution made by dissolving 21.69 g of potassium nitrate, KNO3, in 267.8 g of water? The vapor pressure of pure water at this temperature is 657.6 mmHg. Assume complete dissociation of solute.
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?