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Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to 4 kg of water to prevent it from freezing at − 6 o C will be ( K f for water = 1.86 K k g m o l − 1 , and molar mass of ethylene glycol = 62 g m o l − 1 )
What is the molar concentration of an aqueous solution that contains 26.81% ethylene glycol by mass (MM = 62.07 g/mol)? The density of the solution is 1.04 g/mL. An aqueous solution of ethylene glycol (C_2H_6O_2) is 40% ethylene glycol by mass, and has a density of 1.05 g/mol. What are the molarity, molality, and mole fraction of the solution?
What mass of ethylene glycol (molar mass 62.0 g m o l − 1) must be added to 5.50 kg of water to lower the freezing point of water from 0 0 C to - 10.0 0 C? (K_f f o r w a t e r = 1.86 K k g mol^{-1}$).
Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to 4 kg of water to prevent it from freezing at − 6 o C will be (K f for water = 1.86 K k g m o l − 1, and molar mass of ethylene glycol = 62 g m o l − 1) 804.32 gm; 400.00 gm; 204.30 gm; 304.60 gm
The freezing point of a solution 50 c m 3 of ethylene glycol in 50 g water is found to be − 34 ∘ C. Assuming ideal behaviour, calculate the density of ethylene glycol (K f f o r H 2 O = 1.86 K k g m o l − 1) Given: Molar mass of Ethylene glycol = 62 g m o l − 1
The coolant usually contains a solution of antifreeze prepared by mixing equal volumes of ethylene glycol C 2 H 4 (O H) 2 and water. The density of ethylene glycol is 1.113 g c m − 3. Thus, the freezing point of the mixture is: (K f o f H 2 O = 1.86 K k g m o l − 1)
The coolant usually contains a solution of antifreeze prepared by mixing equal volumes of ethylene glycol C 2 H 4 (O H) 2 and water. The density of ethylene glycol is 1.113 g c m − 3. Thus, the freezing point of the mixture is: (K f o f H 2 O = 1.86 K k g m o l − 1)
Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to 4 kg of water to prevent it from freezing at − 6 o C will be : ( K f for water = 1.86 K kg/mol and molar mass of ethylene glycol = 62 g mol − 1 )
Ethylene glycol has a molar mass of 62.07 g/mol. It is miscible in water due to hydrogen bond formation with water molecules. Like all carbon compounds, ethylene glycol burns to form carbon ...
Mass of ethylene glycol which should be added to 4 kg of water to prevent it from freezing at − 6 o C will be : ( K f for water = 1.86 K kg/mol and molar mass of ethylene glycol = 62 g mol − 1 )