Ethylene glycol, HOCH2CH2OH, is a common automobile antifreeze. It is water soluble and fairly nonvolatile (boiling point = 197°C). Calculate the freezing pointof a solution containing 885 g of this substance in 3,454 g of water. (Cryoscopic constant of water = 1.86 °C/molal; Atomic Weight: C = 12.01 g/mol; H = 1.008g/mol; O = 16.00 g/mol). Express your answer in two decimal places. Do not put the units.

Given mass of ethylene glycol 885g added to 3454g water Kf= 1.86°C/m We have to find freezing…

Answered: hylene glycol, HOCH2CH2OH, is a common…

Chemistry

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Chapter1: Chemical Foundations

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

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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, CH2OHCH2OH (62.10 g/mol), must be dissolved in 267.0 grams of water to reduce the freezing point by 0.400°C ? Refer to the table for the necessary boiling or freezing point constant. _______g antifreeze.
1. A student determines the molar mass of methanol, CH3OH by the same method used in this experiment. She found that the equilibrium temperature of ice and pure water was 0.4 ˚C. When she added 10.0 g of her sample (CH3OH), it fell to -5.4˚C. The mass of the solution was 101.8 g. What was the freezing point depression? What was the molality of CH3OH? How many moles of CH3OH are in the solution? Find the molar mass of CH3OH from the experimental data. How does it compare the value calculated from the periodic table?
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3) Calculate the freezing point (oC) of a solution of 15.46 g of acetone (CH3COCH3, MM = 58.08 g/mol) in 85.0 g of CCl4, whose normal freezing point is –23.0 oC. Given: P = 1 atmKf CCl4 = 29.8 oC/m a) –55.6 b) –93.3 c) 35.7 d) –76.4 e) 70.3 f) –116
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A solution is prepared by dissolving 2.00 g of glycerin (C3HgO3) in 201 g of ethanol (C2H5OH). The freezing point of the solution is °C. The freezing point of pure ethanol is -114.6°C at 1 atm. The molal-freezing-point-depression constant (K) for ethanol is 1.99°C/m. The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively. 0.322 O-114.8 O-116.6 -114.4 Ⓒ-112.6
A compound contains 42.9%C,2.4%H,16.6%N, and 38.1%O by mass. The addition of 3.16 g of this compound to 75 mL of cyclohexane (density is 0.779 g/mL) gives a solution with a freezing point of 0°C. The normal freezing point of cyclohexane is 6.5°C and its freezing point depression constant is 20.2°C/m. What is the empirical mass? A. 84 g/mol B. 88 g/mol C. 36 g/mol D. 55 g/mol E. 98 g/mol F. 44 g/mol
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
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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.
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hylene glycol, HOCH2CH2OH, is a common automobile antifreeze. It is water soluble and fairly nonvolatile (boiling point = 197°C). Calculate the free a solution containing 885 a of this substance in 3 454 g of water (Crvosconic constant of wate 1. 86 °C/molal: Atomic Weight: C 12.01 a/nmol: H