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.)
Tf = 0 - (-13) = 13.0 °C
Kf = 1.86 °C/m
Tf = Kf x molality
13 = 1.86 x molality
molality = 6.99 m
moles of solute = molality x mass of solvent
= 6.99 x 5.0
= 34.95
mass = 34.95 x molar mass
= 34.95 x 62
= 2167 g
mass of ethylene glycol = 2167 g
Some ethylene glycol, HOCH2CH2OH , is added to your car’s cooling system along with 5.0 kg of water. If the freezing po...
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.
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).
What volume of ethylene glycol (HOCH2CH2OH, density = 1.12 g mL-1) must be added to 20.0 L of 112 of water (Kf = 1.86 °C kg mol-1) to produce a solution that freezes at -10 °C?
[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...
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.
please help solve this problem will rate you 14) The cooling system of a car contains a total of 5.50 L of solution, prepared by adding 1.25 L of ethylene glycol (CH2(OH)CH(OH)] to 4.25 L of water. The density of ethylene glycol is 1.11 g/ml. Calculate the new freezing point of this solution. For water, the Kr= 1.86 °C/m.
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...
Calculate and enter the freezing point depression of a solution of 73.2 g ethylene glycol (C2H602) in 561 g H20. Kffor H20 is 1.86 °C kg/mol. °C 1homework pts Submit Answer Tries 0/5 A solution which contains 43.6 g of an unknown molecular compound in 339 g of water freezes at -4.85°C. What is the molar mass of the unknown? g/mol
1. Ethylene glycol, formula C2H602, is used as antifreeze for automobiles and is sometimes mixed with water at a 1:1 ratio by volume and produces a solution with a density of 1.07 g/mbu Assume that the solution behaves ideally. Notes: at 25 °C the densities of water and ethylene glycol are 1.00 g/mL and 1.11 g/mL, respectively, the vapor pressures of water and ethylene glycol at 20 Care 17.54 torr and 0.06 torr, respectively, and Ky and K of water...
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