Some ethylene glycol (OHCH2CH2OH) was added to your car's cooling system along with 5.0 kg of water.
a. if the freezing point of the solution is -15.0 degrees celcius, what mass in grams of glycol must have been added? Kf(H2O)=1.86 degrees celcius kg mol^-1.
b. What is the boiling point of the coolant mixture? Kb(H20) = 0.52 degrees celcius kg mol^-1.
some ehtylene glycol was added to yoru car's cooling system along with 5 kg of water
Some ethylene glycol, HOCH2CH2OH , is added to your car’s cooling system along with 5.0 kg of water. If the freezing point of the water–glycol solution is −13.0 °C, what mass of HOCH2CH2OH must have been added? (Kfp for H2O is −1.86 °C/m.)
a) If 1.95 mol of calcium chloride is added to 2.30 kg of water then what is the freezing point lowering and the freezing point of the solution (Kf = 1.86 ºC/m)? b) If 0.500 mol of NaCl is added to 500 mL of water then what is the boiling point elevation and the boiling point of the solution (Kb = 0.52 ºC/m)?
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).
#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...
[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...
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
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.
3. You prepare an antifreeze/coolant mixture by mixing 1.25 L of ethylene glycol (C2H602. density = 1.12 g/mL) with 2.50 L of water (H2O. density = 1 g/mL). What are the freezing pom and boiling point of your antifreeze/coolant? (K=1.86 °C/m, K-0.51 °C/m)
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