
When 0.49 g of a molecular compound was dissolved in 20.00 g of cyclohexane, the freezing...
When 151.mg of a certain molecular compound X are dissolved in 30.g of cyclohexane(C6H12), the freezing point of the solution is measured to be 1.7°C.Calculate the molar mass of X.
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
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 researcher dissolved 1.50 grams of an unknown compound in 75.0 grams of pure cyclohexane. The freezing point of the solution was measured to be 2.70 °C. Knowing the freezing point of cyclohexane is 6.50 °C and the freezing point constant is -20.2 °C kg/mol, calculate the molar mass of the unknown compound.
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 1.81 g of Vitamin K is dissolved in 25.0 g of camphor, the freezing point of the solution is lowered by 6.06 C. Look up the freezing paint and the Kf constant for camphor in the Colligative Constants table. Calculate the molar mass of Vitamin K.
An unknown sample weighs 0.2436 g was dissolved in 20.0 mL of cyclohexane (density = 0.779 g/mL). The freezing point depression (∆Tf) was 2.5°C. Calculate the molar mass of the unknown substance. (Kf = 20.5 °C/m) ∆Tf = Kf m where Kf is the freezing point depression constant and m is molality. 526 g/mol 1.50 g/mol 128 g/mol 2.44 g/mol
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
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 depression of a solution made by the addition of a nonionic unknown solute to benzophenone was used to determine the molar mass of the unknown. Data was collected for a solution containing 500. g of benzophenone with 5.0 ml of the unknown solute added. The density of the unknown solute was 6.18 g/ml. The K_f of benzophenone is 9.8 degree C M^-1. The freezing point of the benzophenone was determined to be 7.19 degree C. The freezing...