Please explain. Thank you. (8) An antifreeze solution is prepared by mixing 719 mL of ethyl-...
A solution of antifreeze is prepared by mixing 21.0mL of ethylene glycol (d = 1.11 g/mL; molar mass = 62.07 g/mol) with 50.0 mL H2O (d = 1.00 g/mL) at 25°C. If the density of the antifreeze solution is 1.07 g/mL, what is its molarity (M)?
An solution of antifreeze is prepared by mixing 21.0mL of ethylene glycol (d = 1.11 g/mL; molar mass = 62.07 g/mol) with 50.0 mL H2O (d = 1.00 g/mL) at 25°C. If the density of the antifreeze solution is 1.07 g/mL, what is its molarity?
please explain #8 and #9. show all work. thank you 8. An antifreeze solution is prepared by adding 50.0 mL of ethylene glycol, C2H602 (density = 1.12 g/mL) to 50.0 g of water. Calculate the freezing point of this solution. 9. Which has the highest boiling point? (all solutions are in the same solvent) 1.0 M Co(NO3)2 2.0 M KCI 0.5 M C2H4O2
An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d=1.114 g/mL; M= 62.07 g/mol) and water (d=1.00 g/mL) at 20°C. The density of the mixture is 1.070 g/mL. Express the concentration of ethylene glycol as (a) volume percent I % v/v (b) mass percent % w/w (c) molarity м (d) molality (e) mole fraction
An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d=1.114 g/mL;M=62.07 g/mol) and water (d=1.00 g/mL) at 20°C. The density of the mixture is 1.070 g/mL. Express the concentration of ethylene glycol as (a) volume percent 50v/v (b) mass percent 52.05w/w (c) molarity 0.0089 (d) molality 0.0083 (e) mole fraction
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
Be sure to answer all parts. An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d - 1.114 g/mL; M-62.07 g/mol) and water (d = 1.00 g/mL) at 20°C. The density of the mixture is! 1.070 g/mL. Express the concentration of ethylene glycol as (a) volume percent %v/v (b) mass percent % w/w (c) molarity d) malality (b) mass percent (e) molarity (d) molality (e) mole fraction
A solution of antifreese is prepared by mixting 34.0mL of ethylene glycol (d=1.11g/mL; molar mass =62.07 g/mol) with 50.0 mL H20 (d=1.00 g/mol) at 25 degrees celsius. if the density of the antifreeze solution is 1.07 g/ mL, what is the molarity?
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?
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...