A 5.11 g sample of a compound is dissolved in 154.7 g of benzene. The freezing...
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?
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?
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
When 12.6-grams of an unknown compound is placed in 0.116-kg of benzene, the freezing point is changed by 2.34°C. The value of Kf= 4.90°C/m for benzene. Determine the molar mass of the unknown compound. Answer to 1 decimal place and include your units. Answer: Determine the molality of a solution when 32.3 grams of ethanol, C2H5OH (Molar mass = 46.08 g/mol) is dissolved in 0.947 kg of water. Answer to 2 decimal places. Answer: Find the freezing point of a...
When 20.0 grams of an unknown nonelectrolyte compound are dissolved in 500.0 grams of benzene, the freezing point of an unknown nonelectrolyte compound is 3.77 °C. The freezing point of pure benzene is 5.44 °C. What is the change in freezing point?
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
A solution made by dissolving 150.0 g of an unknown compound in 425.0 mL of benzene to make a solution which has a freezing point 18.6 °C lower than that of pure benzene. Kf for benzene is 5.12 °C/m and the density of benzene is 0.877 g/mL. b) The molality of the solution is 3.63. How many moles of the unknown compound were dissolved in the solution? C) what is the molar mass of the unknown compound?
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)
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is dissolved in benzene (C6H), an organic solvent. Use the data below to determine the molar mass of the substance. 8.65 g Mass of unknown compound Freezing point of solution Volume of benzene -10.21°C 35.0 mL 5.53°C Freezing point of benzene Density of benzene Kf for benzene 0.8765 g/mL 5.12°C/m Molar mass = 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?