kindly post different questions separately. please rate
Please help I will rate :) Enter your answer in the provided box. A 249-ml benzene...
Be sure to answer all parts. Ethylene glycol (EG), CH (OH)CH (OH), is a common automobile antifreeze. It is water soluble and fairly nonvolatile (b.p. 197°C). Calculate the boiling point and freezing point of a solution containing 557.5 g of ethylene glycol in 2881 g water. The molar mass of ethylene glycol is 62.07 g/mol. Boiling point: Freezing point: I °C
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...
please help me answer this question with steps thank you. 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. 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
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?
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
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.
Enter your answer in the provided box. A solution of 1.55 g of solute dissolved in 25.0 mL of H20 at 25°C has a boiling point of 100.850°C. What is the molar mass of the solute if it is a nonvolatile nonelectrolyte and the solution behaves ideally (d of H20 at 25°C = 0.997 g/mL)? g/mol
3. What is the boiling point of an antifreeze/coolant solution made from a 40% mixture of ethylene glycol (CHO) in water? Density of CHO is 1.11 g/mL and its molar mass is 62.07 g/mol. Kb= 0.52°C/m Answer: 106.2°C
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...