0.230 g of a compound is dissolved in 10 g of cyclohexane. the solution freezes at 5.12 degrees celcius. calculate the molecular weight of the compound. the freezing point of pure benzene is 5.455 degrees Celsius and the kf = 5.065 degrees Celsius/ m
0.230 g of a compound is dissolved in 10 g of cyclohexane. the solution freezes at...
The freezing point of a solution of 1.104 g of an unknown nonelectrolyte dissolved in 36.81 g of benzene is 1.08°C. Pure benzene freezes at 5.48°C and its Kf value is 5.12°C/m. What is the molecular weight of the compound?
A 1.20 g sample of an unknown compound is dissolved in 60.0 g of benzene. The resulting solution freezes at 4.92 degree C. Calculate the molecular weight of the unknown. Pure benzene freezes at 5.45 degree C\ K_f for benzene is 5.12 degree C/m
The freezing point of a solution that contains 1.00 g of an unknown compound, (A), dissolved in 10.0 g of benzene is found to be 2.17 oC. The freezing point of pure benzene is 5.48 oC. The molal freezing point depression constant of benzene is 5.12 oC/molal. What is the molecular weight of the unknown compound?
What is the molar mass of a nonpolar molecular compound if 6.34 g dissolved in 53.4 g benzene begins to freeze at 2.81 °C? The freezing point of pure benzene is 5.50 °C and the freezing point depression constant, Kf, is -5.12 °C/m. A. 2.26 x 10-4 g/mol B. 0.226 g/mol C. 12.1 g/mol D. 226 g/mol
A 2.50 g sample of naphthalene, C10H8, was dissolved in 100 g of benzene. What is the freezing point of the solution? The freezing point of pure benzene is 5.45 degrees Celsius; Kf=5.07 degrees Celsius/m. The molar mass of C10H8 is 128.17 g/mol The answer is supposed to be 4.46 degrees Celsius. How did they get there?
A nonvolatile, non-dissociating solute was dissolved in 12.0 g of benzene (C6H6). The freezing point of the solution was measured as 1.3 °C, while pure benzene freezes at 5.5 °C. If pure benzene has a vapor pressure of 75 torr, what is the vapor pressure of this solution. For benzene, Kf = 5.12 °C/m and Kb = 2.53 °C/m.
1.0345 g of palmitic acid dissolved in 8.7545 g of stearic acid. Calculate the freezing point of the solution. The molar mass of palmitic acid is 256.48 g/ mol. The molal freezing point constant , Kf for stearic acid is 4.5 degrees C/ m and pure stearic acid freezes at 69.3 degrees Celsius.
please help ! 26. The freezing point depression of a solution of 1.45g sample of an unknown nonelectrolyte dissolved in 25.00 mL of benzene(density d=0.879 g/mL) is 1.28°C. Pure benzene has Kf value of 5.12°C/m. What is the molecular weight of the compound? (10 points)
1.A solution that contains 15.581 grams of benzene (molar mass = 78.1 g/mol) in 420 g of cyclohexane freezes at a temperature 9.50 ºC below the freezing point of pure cyclohexane. Calculate the molar freezing point depression constant, Kf, for cyclohexane. 2. The molar boiling point elevation constant for water is 0.512 ºC/m. What is the boiling point of a solution containing 673 g of water and 78.0 g of CaCl2? 3. A solution containing 32.0 g of an unknown...
1a: 19.930 g of a non-volatile solute is dissolved in 395.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 90°C the vapour pressure of the solution is 521.11 torr. The vapour pressure of pure water at 90°C is 525.80 torr. Calculate the molar mass of the solute (g/mol). 1b: Now suppose, instead, that 19.930 g of a volatile solute is dissolved in 395.0...