2. An automobile mechanic mixes ethylene glycol with water to make a solution of automobile antifreeze. This mixture contains 1104 g of ethylene glycol and 1.50 kg of pure water. What is the freezing point of this solution in degrees Celsius? (Assume 1 atm pressure.)
3. A zoologist combines NaCl with pure water for use in an outdoor aquatic facility. She makes the salt/water mixture by dissolving 15.0 kg of NaCl and 400.0 kg of pure water. What is the freezing point of this solution in degrees Celsius? (Assume 1 atm pressure.)
2. An automobile mechanic mixes ethylene glycol with water to make a solution of automobile antifreeze....
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
#5 Ethylene glycol (C2H6O2) is used as an antifreeze. How many grams of ethylene glycol must be added to 1.0 L of water to reduce the freezing point of the glycol-water mixture to -10.0 degrees C? The freezing point depression constant of water is 1.86 (deg/molal).
A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of 9.78% of ethylene glycol with a density of 1.0108 g/mL. The freezing point depression constant for water (solvent for all solutions) is Kf=-1.86 percent celsius kg/mol and the boiling point elevation constant is Kb=0.512 degrees celsius kg/mol. The density of neat water at 20.0 degrees celsius is 0.9982 g/mL. Answer the following: 1. What is the molarity of the solution? 2. What is the...
How many liters of the antifreeze ethylene glycol would you add to a car radiator containing 6.50 L of water if the coldest winter temperature is -28.0 degrees Celsius? Calculate the boiling point of this water-ethylene glycol mixture. (Then density of ethylene glycol is 1.11g/mL) Liters of antifreeze _______ L Boiling point of solution_________ Celsius degrees
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.
An ethylene glycol solution contains 30.0g of ethylene glycol (C2H6O2) in 95.6mL of water. (Assume a density of 1.00 g/mL for water.) 1.Determine the freezing point of the solution. Express you answer in degrees Celsius 2.Determine the boiling point of the solution. Express you answer in degrees Celsius.
An ethylene glycol solution contains 14.2 g of ethylene glycol (C2H6O2) in 83.4 mL of water. A.Calculate the freezing point of the solution. (Assume a density of 1.00 g/mL for water.) Express your answer in degrees Celsius using three significant figures. B. Calculate the boiling point of the solution. Express your answer in degrees Celsius using two decimal places.
Radiator antifreeze solutions are commonly a mixture of ethylene glycol (C2H6O2) and water and has a minimum freezing point of -51.0 °C. How much ethylene glycol do you need to add to 500 grams of water to reach -51.0 °C? Kf 1.86
Antifreeze is an 50% by mass aqueous solution of the non-electrolyte ethylene glycol (C2H6O2). What is the freezing point of this solution? The Kf for water is 1.86oC∙kg∙mol−1 and assume a density of 1.00g/mL.
Ethylene glycol (C₂H₆O₂) is used as an additive to the water in your automobile to lower its freezing point. A solution of ethylene glycol in water has a freezing point of -4.10°C. How many grams of ethylene glycol must be added to 1000 g of this solution to lower the freezing point to -11.00 °C? (Kf for water is 1.86°C・kg/mol).