how many grams of of ethylene glycol are needed per kilogram of water to protect the radiator fluid against freezing down to -10C

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1. How many grams of ethylene glycol, C2H4(OH)2, are needed per kilogram of water to protect radiator fluid against freezing down to -10Â°C?

2. For benzene, C6H6, the freezing point constant, Kf, is 5.12 K oC/m and its normal freezing point is 5.5Â°C. What is the freezing point of a solution containing 100.0 g of benzene and 20.0 g of naphthalene (C10H8)?

3. When 5.0 g of an unknown substance is dissolved in 100.0 g of water, the freezing point of the solution decreases by 1.5Â°C. What is the molar mass of the unknown substance if the compound does not dissociate to form ions in solution?

4. If 2.00 moles of a substance is dissolved in 1.00 kg of water, the freezing point of the solution decreases by 7.44Â°C. Does this substance dissociate to form ions in solution? Explain why.

5. Calculate the freezing point of a 0.2 m CaCl2 aqueous solution, assuming it dissociates completely to form ions in solution.

A common antifreeze for car radiators is ethylene glycol, CH2(OH)CH2(OH). How many liters of ethylene glycol would you add to 5.6 L of water in the radiator if the coldest day in winter is -12Â°C? How much will the amount of ethylene glycol you calculated elevate the boiling point of the fluid in the radiator? Kf for water is 1.86 mol-1 kg and Kb is 0.51 K mol-1 kg. Assume a water density of 1 kg/L, a density of ethylene glycol of 1.11 g cm-3 and ethylene glycol boiling point of 470 K.

How many grams of ethylene glycol (automobile antifreeze,C2H6O2) dissolved in 3.10kg of water is needed to lower thefreezing point of water in an automobile radiator to

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how many grams of of ethylene glycol are needed per kilogram of water to protect the radiator fluid against freezing down to -10C

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