Be sure to answer all parts. Ethylene glycol (EG), CH (OH)CH (OH), is a common automobile...
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Enter your answer in the provided box. A 249-ml benzene solution containing 2.55 g of an organic polymer has an osmotic pressure of 8.27 mm Hg at 19°C. Calculate the molar mass of the polymer. - g/mol Enter your answer in the provided box. Calculate the molality of a 5.93 M ethanol (C2H5OH) solution whose density is 0.9307 g/mL. Ethylene glycol (EG), CH2(OH)CH2 (OH), is a common automobile antifreeze. It is water soluble and...
Be sure to answer all parts. How many liters of the antifreeze ethylene glycol [CH2(OH)CH2(OH)] would you add to a car radiator containing 7.25 L of water if the coldest winter temperature in your area is -21.0°C? Calculate the boiling point of this water-ethylene glycol mixture. (The density of ethylene glycol is 1.11 g/mL.) What is the volume of antifreeze? L. What is the boiling point of the solution? oC
Ethylene Glycol [CH2(OH)CH2(OH)] is a common automobile antifreeze. Calculate the Freezing Point and boiling point of a solution containing 283g of ethylene glycol and 1035g of water. (Kb and Kf of water are .52 C/m and 1.86 C/m respectively.
Ethylene glycol is used in automobile radiators as an antifreeze. Use the following information to determine the freezing point of an antifreeze solution made by mixing 2.5 L of ethylene glycol with 2.5 L of water. Ethylene glycol is essentially nonvolatile and it does not dissociate in water. Molar mass of ethylene glycol = 62.1 g/mol; density of ethylene glycol = 1.11 g/mL; density of water = 1.00 g/mL; Kf for water = 1.86 degrees Celsius kg/mol
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5. Ethylene glycol (antifreeze, CH2(OH)CH2(OH)) has a regular boiling point of 197°C, what is the freezing point of a solution that has 982.91 mL of water and 390.2 g of ethylene glycol in i t? (cter)1.3 oC
Be sure to answer all parts. An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d - 1.114 g/mL; M-62.07 g/mol) and water (d = 1.00 g/mL) at 20°C. The density of the mixture is! 1.070 g/mL. Express the concentration of ethylene glycol as (a) volume percent %v/v (b) mass percent % w/w (c) molarity d) malality (b) mass percent (e) molarity (d) molality (e) mole fraction
How many liters of the antifreeze ethylene glycol [CH2(OH)CH2(OH)] would you add to a car radiator containing 5.50 L of water if the coldest winter temperature in your area is −20.0°C? Calculate the boiling point of this water-ethylene glycol mixture. (The density of ethylene glycol is 1.11 g/mL.) What is the volume of antifreeze? L What is the boiling point of the solution?
Antifreeze is ethylene glycol, C2H4(OH)2 and is made from ethylene which is produced from oil. It is miscible in water (i.e., dissolves in any proportion), does not dissociate in water, is toxic to drink (especially to dogs who like the sweet taste), but fortunately is biodegradable and at normal automobile operating temperatures, is not flammable. It can prevent freezing of the automobile cooling system down to -34oF and the advertisement says “winter - summer automobile coolant” — it also prevents...
[References] What volume of ethylene glycol (C2HO2), a nonelectrolyte, must be added to 12.0 L water to produce an antifreeze solution with a freezing point of-19.0°C? (The density of ethylene glycol is 1.11 g/cm°, and the density of water is 1.00 g/cm³. K, for water is 0.51°C•kg/mol and Kf is 1.86°C kg/mol.) Volume %3D What is the boiling point of this solution? Boiling point °C %3D 5 item attempts remaining Submit Answer Try Another Version [References] Consider an aqueous solution...
How many liters of the antifreeze ethylene glycol [CH_2(OH)CH_2(OH)] would you add to a car radiator containing 6.50 L of water if the coldest winter temperature in your area is -13 degree C? (The density of ethylene glycol is 1.11 g/mL. Assume the density of water at -13 degree C is 1.00 g/mL.) L Calculate the boiling point of this water-ethylene glycol mixture. degree C