Kf Of Ethylene Glycol

The freezing point of water is $0.00^{‘circ} ‘mathrm{C}$ at 1 atmosphere. $’mathrm{K}_{‘mathrm{f}}$ for water is $1.86^{‘circ} ‘mathrm{C} / ‘mathrm{m} .$ A molecular substance that dissolves in water is antifreeze (ethylene glycol). If 11.35 grams of antifreeze, $’mathrm{CH}_{2} ‘mathrm{OHCH}_{2} ‘mathrm{OH}(62.10 ‘mathrm{g} / ‘mathrm{mol}),$ is dissolved in 272.3 grams of water, what are the molality and the boiling point of the solution?

question number 1 22 is a little confusing. It starts out by telling you the freezing point of water and gives you the KF value of water. But then it goes on and asks you to determine the boiling point of water, so Im not quite sure where they gave U. K F and the freezing point. But well answer the question as it was written, calculating the boiling point of a solution that contain an acquis solution that contains a given amount of ethylene glycol or antifreeze. So the change in the boiling point temperature will be equal toothy boiling point constant for water multiplied by the morality of the salute. In water. The boiling point constant is 0.0.52 degrees Celsius per morality. Morality then will be equal to the grams of the ethylene glycol divided by its Moeller Mass. That gives us moles ethylene glycol divided by the kilograms of water which we dont know, but we do know the grams so we can convert the grams into kilograms by dividing by 1000. This then gives us 10000.672 Malala ethylene glycol, so the new boiling point will be equal 2.52 multiplied by the morality 0.672 and we get 0.35 degrees Celsius, so the boiling point of water is normally 100 degrees. If the change in temperature is a plus 1000.35 then the new temperature will be 100.35 degrees Celsius. Get More Help with this Textbook

Solvent Boiling point (°C) Kf (°C⋅kg/mol)
Ethylene glycol 197.3 –3.11
Formic acid 101.0 –2.77
Naphthalene 217.9 –6.80
Nitrobenzene 210.8 –7.00

What exactly is the Molality Formula?

Molality may be calculated using the formula m = moles of solute per kilogramme of solvent. When dealing with molality problems, it is occasionally necessary to employ extra formulae in order to arrive at the ultimate solution. One formula that we should be familiar with is the density formula, which is d = m / v, where d denotes density, m denotes mass, and v is volume.

There were 36 related questions and answers found.

The Kf value for water is 1.86 degrees Celsius per kilogramme of molecular weight. 1.

What is the freezing point constant of ethylene glycol?

Pure ethylene glycol has a freezing point of -12.9 ° C and the freezing point of water is 0 ° C. Therefore, the freezing point of the solution should be below 0 ° C (which occurs is a decrease in the freezing point due to the colligative properties of adding solutions to a solvent, so the freezing point must decrease).

(Kf for CCl4 = 30. K kg / mol)


What is the freezing point depression constant of ethylene glycol?

Ethylene glycol is a chemical commonly used in many commercial and industrial applications including antifreeze and coolant. Ethylene glycol helps keep your car’s engine from freezing in the winter and acts as a coolant to reduce overheating in the summer.

Which solvent has highest KF value?

Breathing ethylene glycol vapors may irritate eyes and lungs but is unlikely to cause systemic toxicity. Ethylene glycol does not absorb well through the skin so systemic toxicity is unlikely. Eye exposure may lead to local adverse health effects but is unlikely to result in systemic toxicity.

What is the KF value of CCl4?

It is produced commercially from ethylene oxide, which is obtained from ethylene. Ethylene glycol is widely used as antifreeze in automobile cooling systems and in the manufacture of human-made fibres, low-freezing explosives, and brake fluid.

What happens to the freezing point of water when ethylene glycol is added?

The primary sources of ethylene glycol in the environment are disposal of used antifreeze and use of de-icing solutions at airports (ATSDR 2010; EPA 2000). The primary sources of ethylene glycol in the environment are from disposal of used antifreeze and use of de-icing solutions at airports.

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