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pashok25 [27]
3 years ago
8

Calculate the vapor pressure (in torr) of a 35°C solution of ethanol and propanol where the mole fraction of propanol is .75. As

sume Ideal behavior P°ethanol35=100torr P°propanol35=36torr
Chemistry
1 answer:
ASHA 777 [7]3 years ago
7 0

The vapor pressure (in torr) of a 35°C solution : 52 torr

<h3>Further explanation</h3>

Given

x propanol = 0.75

P°ethanol=100 torr

P°propanol=36 torr

Required

the vapor pressure

Solution

Raoult's Law

P solution = xA.P°A +xB.P°B

x ethanol = 1- 0.75 = 0.25

Input the value :

P solution = 0.25 x 100 + 0.75 x 36

P solution = 25 + 27

P solution = 52 torr

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determine the freezing point depression of a solution that contains 30.7 g glycerin (c3h8o3, molar mass
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The freezing point depression of a solution containing 30.7 g of glycerin  is  calculated as -1.65°C

Equating :

It is given that,

Given mass of glycerin is = 30.7 grams (Solute)

Volume of water = 376 mL

K_{f}or molar -freezing-depression point is = 1.86°C/m

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Now, to work out the value, the mass of water should be known. Thus, to calculate, the formula used will be:

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Using the formula of melting point depression, the equation becomes:

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Since, glycerin is a non-electrolyte, the Van't Hoff factor will be 1.

Substituting the values in the above equation:

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T_{s} = -1.65°C

Thus, the freezing point depression of a solution is  -1.65°C

<h2 />

Freezing point depression

Freezing point depression is a colligative property observed in solutions that results from the introduction of solute molecules to a solvent. The freezing points of solutions are all less than that of the pure solvent and is directly proportional to the molality of the solute

Is melting point elevation or depression?

Boiling point elevation is that the raising of a solvent's boiling point due to the addition of a solute. Similarly, melting point depression is the lowering of a solvent's freezing point due to the addition of a solute. In fact, because the boiling point of a solvent increases, its melting point decreases

Learn more about freezing point depression :

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