
please help ! 26. The freezing point depression of a solution of 1.45g sample of an...
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?
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
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?
Pure cyclohexane, C6H12, has a freezing point of 6.53 celcius. Its freezing point depression constant is: Kf=20.0 degrees celcius m^-1. A solution was made by taking 10.55g of an unknown nonelectrolyte and dissolving it in 125.0g of cyclohexane. The measured freezing point of the solution was -3.28 degrees Celsius. Calculate the molecular weight of the unknown substance.
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?
Find the freezing point depression of pure lauric acid-unknown solution. Find the molality of the unknown. Info: Kf= 4.40*C/moles solute Freezing point of pure lauric acid- 43.2*C and freezing point of solution- 42 *C Mass of unknown solid (nonelectrolyte)- 0.0612g, mass of lauric acid- 3.9321g
A 1.2436g sample of an unknown nonelectrolyte is dissolved in 10.9303g of benzophenone produces a solution that freezes at 43.2 degree C. If the pure benzophenonemelted at 48.1 degree C, what is the molecular weight of the unknown compound? The Kf for benzophenone is 9-8 degree C/m.
a) The freezing point of water, H2O, is 0.000 °C at 1 atmosphere. Kf(water) = 1.86 °C/m In a laboratory experiment, students synthesized a new compound and found that when 12.48 grams of the compound were dissolved in 246.0 grams of water, the solution began to freeze at -1.570 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? b) The freezing point of benzene, C6H6, is 5.500 °C...
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
What is the freezing point of a solution of 12.8 g of C10H8 dissolved in 500 g of benzene? The normal freezing point of pure benzene is 5.48 oC and its Kf is 5.12 oC/m.