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Problem #14: Calculate the vapor pressure of a solution made by dissolving 21.80 g of glucose (molar mass = 180.155 g/mol) in 460.0 g of H 2 O at 30.0 °C. (The vapor pressure of the pure solvent is 31.82 mmHg at 30.0 °C.)
Practice problems on the colligative properties of solutions covering the freezing point depression, boiling point elevation, vapor pressure, and osmotic pressure of solutions prepared with nonelectrolytes as well as ionic compounds.
Problem solutions. 1. Calculate the vapor pressure of a mixture containing 252 g of n-pentane (Mw = 72) and 1400 g of n-eptane (Mw = 100) at 20oC. The vapor pressure of n-pentane and n-eptane are 420 mm Hg and 36 mm Hg respectively.
12 lip 2023 · Calculate the vapor pressure of an aqueous solution containing 30.2% ethylene glycol by mass, a concentration commonly used in climates that do not get extremely cold in winter. Given: identity of solute, percentage by mass, and vapor pressure of pure solvent. Asked for: vapor pressure of solution. Strategy:
The vapor pressure calculator helps you learn about phase transition, latent heat, the Clausius-Clapeyron equation and other parts of thermodynamics and chemistry.
1.) Calculate the vapor pressure in torr of a solution that is made by dissolving 59.51 grams of glucose (C6H12O6) in 112.2 mL of water at 26.7 oC. The vapor pressure of pure water at 26.7 oC is 26.271 torr and the density of water at that temperature is 0.99669 g/mL. First we need to find the mole fraction of the solvent (water).
13 lut 2023 · The vapor pressure over a solution of urea (CH 4 N 2 O) is 291.2 mm Hg. The vapor pressure of pure water at the same temperature is 355.1 mm Hg. Calculate the mole fraction of urea in the solution. Don’t forget that Raoult’s law (as written above) is in terms of the mole fraction of water!
