3. A 5.00 gram sample of lauryl alcohol is dissolved in 100 g of benzene (k,=5.10 °C/m). The normal freezing point of benzene is 5.50°C while the solution froze at -1.78°C. What is the molecular weight of lauryl alcohol?

A 5.00 gram sample of lauryl alcohol is dissolved in 100 g of benzene (Kf = 5.10 degrees C/m). The normal freezing point of benzene is 5.50 degrees Celsius while the solution froze at -1.78 degrees Celsius. What is the molecular weight of lauryl alcohol ?

When 225. of urea (CH,N,0) are dissolved in 1200. g Oof a certain mystery g liquid x, the freezing point of the solution is 8.4 °c lower than the freezing point of pure x. On the other hand, when 225. g of sodium chloride are dissolved in the same mass of x, the freezing point of the solution is 14.5 °C lower than the freezing point of pure x. olo Ar Calculate the van't Hoff factor for sodium chloride in x. Be sure your answer has a unit symbol, if necessary, and is rounded to the correct number of significant digits. i = |

The freezing point of water H₂O is 0.00 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in water is antifreeze (ethylene glycol). How many grams of antifreeze, CH₂ OHCH₂OH (62.10 g/mol), must be dissolved in 268.0 grams of water to reduce the freezing point by 0.450 °C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb(°C/m) Kf(°C/m) Water H₂O 0.512 Ethanol CH3 CH₂ OH 1.22 Chloroform CHCl3 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 Mass= g 1.86 1.99 5.12

Benzene is a common industrial solvent (molar mass: 78.11 g/mol). Its normal freezing point is 5.50 °C and its freezing point depression constant is Kf = -5.12 °C/m. Determine the freezing point (in °C with 3 significant figures) for the solution prepared by mixing 3.82 g of anthracene (C14H10; molar mass = 178.23 g/mol) and 51.4 g of benzene.

6. Ethylene glycol [CH₂(OH)CH₂(OH)] is a common automobile antifreeze. It is water soluble and fairly nonvolatile (b.p. 197°C). Calculate (a) the freezing point and (b) the boiling point of a solution containing 268 g of ethylene glycol in 1015 g of water.

4. A 6.06-gram sample of a compound is dissolved in 250. grams of benzene. The freezing point of this solution is 1.02°C below that of pure benzene. What is the molar mass of this compound? (Note: Kę for benzene = 5.12°C/m.)

5. A 2.50 g sample of naphthalene, C₁0H8, was dissolved in 100 g of benzene. What is the freezing point of the benzene solution? The freezing point of pure benzene is 5.45°C and its Kf is 5.07°C/m.

2. When 7. 94 g of xylene was added to 132.5 g of cyclohexane, the freezing point of the solution was  -4.9 degrees celsius. What is the molar mass of xylene?

when 7.94 g of xylene was added to 132.5 g of cyclohexane, the freezing point of the solution was -4.9 C. what is the molar mass of xylene?