Ethylene glycol, HOCH2CH20H, is a common automobile antifreeze. It is water soluble and fairly nonvolatile (boiling point = 197°C). Calculate the freezing point of a solution containing 759 0-g of this substance in 4868 g of water. (Cryoscopic constant of water = 1.86 °C/molal; Atomic Weight: C = 12.01 g/mol; H = 1.008 g/mol; O = 16.00 g/mol). Express your answer in two decimal places. Do not put the units.

Ethylene glycol, HOCH2CH20H, is a common automobile antifreeze. It is water soluble and fairly nonvolatile (boiling point = 197°C). Calculate the freezing point of a solution containing 759 0-g of this substance in 4868 g of water. (Cryoscopic constant of water = 1.86 °C/molal; Atomic Weight: C = 12.01 g/mol; H = 1.008 g/mol; O = 16.00 g/mol). Express your answer in two decimal places. Do not put the units.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

When 45.8 g of glycine (C₂H₂ NO₂) a are dissolved in 700. g of a certain mystery liquid X, the freezing point of the solution is 2.9 °C lower than the freezing point of pure X. On the other hand, when 45.8 g of iron(III) chloride are dissolved in the same mass of X, the freezing point of the solution is 4.4 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for iron(III) chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits. - 0 i = x10 G
When 5.71g of naphthalene is added to 152g of benzene the solution freezes at 3.98 degrees Celsius. What is the molar mass of naphthalene ? ( Freezing Point of pure benzene = 5.46 degrees Celsius and Kf of naphthalene = 5.07 degrees Celsius/ molal )
Help with the following question and round the answer to 1 sig fig
When 10.1 g of an organic compound known to be 54.53% C, 9.2% H, and 36.32% O by mass is dissolved in 677.6 g of cyclohexane, the freezing point is 3.07 °C. The normal freezing point of cyclohexane is 6.59 °C. What is the molecular formula for the organic compound? Assume that the organic compound is a molecular solid and does not ionize in water. Kf values for various solvents are given in the colligative constants table. molecular formula: CHO
Ethylene glycol, HOCH2CH2OH, is a common automobile antifreeze. It is water soluble and fairly nonvolatile (boiling point = 197°C). Calculate the freezing point of a solution containing 876 g of this substance in 4,658 g of water. (Cryoscopic constant of water = 1.86 °C/molal; Atomic Weight: C = 12.01 g/mol; H = 1.008 g/mol; O = 16.00 g/mol).
If the freezing point of the solution was observed to be -8.6 °C, and the normal freezing point of cyclohexane is 6.50 °C, what is the value of Kf for cyclohexane? 4.67 g of toluene in 67.8 g of cyclohexane The molar mass of toluene is 92.14 g/mol.
(a) A 2.300 molal solution of KCl is prepared. How many grams of KCl are present in a sample containing 5.000 kg of water? (b) Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g/mol) in 376 mL of water. Some possibly useful constants for water are Kf = 1.86°C/m and Kb = 0.512°C/m.
Analysis of a compound gave 39.50% C, 2.21% H, and 58.30% Cl. When 0.855 g of this solid was dissolved in 7.50 g of naphthalene, the solution had a freezing point of 78.0°C. The pure solvent freezes at 80.0°C; its molal freezing point constant is 6.8°C/m. What is the molecular formula of the compound?
Determine the vapor pressure of a solution prepared by dissolving 16.8 mol of non-volatile aspirin (MM = 180.15 g/mol) in 0.691 kg of CH3CH2OH (MM = 46.07 g/mol) at 25 °C. Pº ethanol 44.0 torr at 25 °C. Give the answer to 3 significant figures. Do not include units. =
The normal boiling point of a certain liquid X is 124.9 °C, but when 31. g of urea ((NH,) CO) are dissolved in 350. g of X, it is found that the solution boils at 127.0 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. 9. Round your answer to 2 significant digits. - 1 |°C• mol •kg
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
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.