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13 Dec 2019

Preston, ethylene glycol, is the liquid dissolved in water used in automobile cooling systems. Find the vapor pressure of a 2.000 L solution that was prepared mixing equal volumes of antifreeze and water together at 100 degrees Celsius. Assume this solution obeys ideal conditions(Raoult's law). Hint: you will need to find the density for each solute and solvent present in the solution at 100 degrees Celsius.

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Jean Keeling
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17 Dec 2019

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Related questions

1)calculate the molality of a 1.69 M ethanol (C2H5OH) solutionwhose density is 0.9731g/mL?

2) Ethylene glycol (EG), Ch2(OH)CH2(OH), is common automobileantifreeze. It is water soluble and fairly volitile (bp 197 C)Calculate the boiling pt and freezing pt of asolution containing595.5g of ethylene glycol in 3021g water. the molar mass of EG is62.01g/mol

3)A solution of 0.790 g of an organic compound in 100.0g ofbenzene has a freezing pt of 5.196 celsius. What are the molalityof the solution and the molar mass of the solute? The normalfreezing pt of benzene is 5.500 celcius and the Kf for benzene is5.12 celcius/m

4) calculate the amount of water in grams that must be added toeach of the following sunstances to produce indicatewdsolution:

a)9.50g urea (NH2)2CO in the p[reperation of 19.1 percent bymass solution :________g

b)24.8g of MgCl2 in the preperation of 3.7 percent masssolution: _______g

5)the solubility of CO2 in water at 25 celsius and 1atm is 0.034mol/L. What is itys solubility at a partial pressure in air of0.00035 atm? assume that CO2 obeys Henry's Law

6)a solution is prepared by dissolving 386g of sucrose(c12H22O11) in 704g of water. What is the vapor pressure of thissolution at 30 celsius? ( the vapor pressure of water is 31.8mmHgat 30 celsius)

7)the vapor pressure of ethanol (c2h5oh) at 20 celcius is44mmHg, and the vapor pressure of mathanol (ch3oh at the sametemperature is 94mmHg. A mixture of 30.01g of methanol and 48.7g ofethanol is prepared and can be assumed to behave as an idealsolution. calculate the vapor pressure of methanol and ethanolabove this solution at 20 celcius. Calculate the mol fraction ofmethanol and ethanol in the vapor above this solution at 20celcius.

1. The vapor pressure of ethanol (C2H5OH) at 20°C is 44 mmHg, and the vapor pressure of methanol (CH3OH) at the same temperature is 94 mmHg. A mixture of 28.1 g of methanol and 45.9 g of ethanol is prepared and can be assumed to behave as an ideal solution.

Calculate the vapor pressure of methanol and ethanol above this solution at 20°C. Be sure to report your answers to the correct number of significant figures.

Ethanol: ____mmHg

Calculate the mol fraction of methanol and ethanol in the vapor above this solution at 20°C.

Methanol _____

Ethanol _____

2.

Be sure to answer all parts.

How many liters of the antifreeze ethylene glycol

[CH2(OH)CH2(OH)] would you add to a car radiator containing 7.50 L of water if the coldest winter temperature in your area is −20.5°C? Calculate the boiling point of this water-ethylene glycol mixture. (The density of ethylene glycol is 1.11 g/mL.)


What is the volume of antifreeze?

L

What is the boiling point of the solution?

°C

3. Calculate the percent by mass of the solute in each of the following solutions:


(a) 5.03 g of NaBr in 71.1 g of solution

% NaBr

(b) 32.5 g of KCl in 183 g of water

% KCl

(c) 3.81 g toluene in 33.1 g benzene

% toluene

1.

When a solute is added to a liquid, the boiling point of the resulting solution is __________ than the freezing point of the pure liquid.

A. no different

B. higher

C. lower

2.

When a solute is added to a liquid, the boiling point of the resulting solution is __________ than the freezing point of the pure liquid.

A. higher

B. no different

C. lower

3.

Solution properties are defined as _______________ if the property depends solely on the number of particles of solute and solvent in the solution, not the identity of the solute.

A. vapor pressure

V.colligative

chemical

hydrogen bonding

4.

The advantage of using ________________ rather than the more commonly used unit of ___________________ is that it is independent of temperature effects on density (and thus, volume) of the solution

A. molarity, ppb

B. molarity, % mass

C. molality, molarity

D. molarity, ppm

5.

If a 6.75 g sample of NaCl were dissolved in 8.41 kg of methanol, the molality would be ___________________ m.

A. 0.0137

B. 1.602

C. 0.803

D. 0.0445

6.

The only information needed to determine the freezing point depression of a non-electrolyte is ______________________________ and _________________________________. f

A. the freezing point constant for the solvent, the temperature

B. the boiling point constant, the boiling point elevation

C. the delta T, the color of the most concentrated sample

D. the molality of the solute, the Kf of the solvent

7.

An aqueous solution boils at 100.50oC. What is the freezing point of the solution? Kb(H2O) = 0.51 oC/m; Kf(H2O) = 1.86 oC/m

A. 0.50 oC

B. -0.50 oC

C. -1.82 oC

D. -5.50 oC

8.

Bromoform has a normal freezing point of 7.80 oC and its Kf = 14.4 oC/m. A solution of 2.58 g of an unknown in 100 g of bromoform freezes at 5.43 oC. What is the molecular weight of the unknown?

A. 18.02 g / mol

B. 0.165 g / mol

C. 156 g / mol

D. 44.01 g / mol

9.

Calculate the freezing point of 0.200 m solution of fructose, C6H12O6, a) in water (boiling point, 0 oC), and b) in acetic acid (boiling point, 16.6 oC). Kf(water) = 1.86 oC/m and Kf(acetic acid) = 3.9 oC.

A. -0.372 oC and 15.8 oC

B. -0.958 oC and 12.3 oC

C. 3.221 oC and 0.875 oC

D. -4.124 oC and 0.0035 oC

10.

Calculate the boiling point, in Celsius, at 1atm of a solution containing 30.0 of cane sugar (molecular weight = 342 g / mol) and 150 g of water.

A. 100.30

B. 103.00

C. 99.7

D. 301.00

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