A 0.0619 g quantity of Ethylene glycol (antifreeze) represents the mass of 6.00 X 10^20 molecules. What is the molar mass of the compound?
A 0.0619 g quantity of Ethylene glycol (antifreeze) represents the mass of 6.00 X 10^20 molecules....
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?
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
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)?
Ethylene glycol (antifreeze) has a density of 1.11 g/m Cm^3, What is the mass in grams of 361 mL of ethylene glycol? Express your answer with the appropriate units. What is the volume in liters of 3.60 kg of ethylene glycol? Express your answer with the appropriate units.
An aqueous antifreeze solution is 31.0 % ethylene glycol (C2 H4 O2) by mass. The density of the solution is 1.05 g/cm3. Calculate the molality, molarity and mole fraction of the ethylene glycol Molality mol/kg Molarity mol/L 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 I % v/v (b) mass percent % w/w (c) molarity м (d) molality (e) mole fraction
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...
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
Determine the mass of ethylene glycol dissolved in 253 g of an 25.2 % ethylene glycol solution. g ethylene glycol
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.)