How many liters of the antifreeze ethylene glycol [CH_2(OH)CH_2(OH)] would you add to a car radiator...
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?
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
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
there's two questions :) Enter your answer in the provided box A solution is prepared by dissolving 396 g of sucrose (C12H2011) in 604 g of water. What is the vapor pressure of this solution at 30°C? (The vapor pressure of water is 31.8 mmHg at 30°C.) mmHg Be sure to answer all parts. How many liters of the antifreeze ethylene glycol (CH2(OH)CH (OH) would you add to a car radiator containing 5.75 L of water if the coldest winter...
The solubility of N2 in blood at 37°C and at a partial pressure of 0.80 atm is 5.6 x 10 mol/L. A deep- sea diver breathes compressed air with the partial pressure of N2 equal to 3.6 atm. Assume that the total volume of blood in the body is 4.7 L. Calculate the amount of N2 gas released (in liters at 37°C and 1.00 atm) when the diver returns to the surface of the water, where the partial pressure of...
In a radiator, the antifreeze is composed of 74.3% ethylene glycol with a density of 0.8 g / cm3 and 25.7% water. Find the density of the mixture if the percentages are in: (a) volume; (b) mass (It is neglected that the volume of the mixture is slightly less than the sum of the starting volumes.)
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
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
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)
8. Ethylene glycol, HO-CH2-CH2-OH, a nonelectrolyte, is added to the water in a radiator to give a solution containing 515 g of ethylene glycol in 565 g of water. a. What is the molality of this solution? b. What is the boiling point of this solution? (Kb = 0.512 °C kg/mol for water)