Benzene is a common industrial solvent (molar mass: 78.11 g/mol). Its normal freezing point is 5.50 °C and its freezingpoint depression constant is Kf = -5.12 °C/m. Determine the freezing point (in °C with 3 significant figures) for thesolution prepared by mixing 3.82 g of anthracene (C14H10; molar mass = 178.23 g/mol) and 51.4 g of benzene.

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Answered: Benzene is a common industrial solvent…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A compound contains 42.9%C,2.4%H,16.6%N, and 38.1%O by mass. The addition of 3.16 g of this compound to 75 mL of cyclohexane (density is 0.779 g/mL) gives a solution with a freezing point of 0°C. The normal freezing point of cyclohexane is 6.5°C and its freezing point depression constant is 20.2°C/m. What is the empirical mass? A. 84 g/mol B. 88 g/mol C. 36 g/mol D. 55 g/mol E. 98 g/mol F. 44 g/mol
5. The vapor pressure of benzene is 73.03 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in benzene is TNT. Calculate the vapor pressure of the solution at 25 °C when 12.12 grams of TNT, C,H;N;Os (227.1 g/mol), are dissolved in 155.7 grams of benzene. benzene = CHs = 78.12 g/mol.
The normal freezing point of a certain liquid X is 4.60°C, but when 40.g of iron(III) nitrate (FeNO33) are dissolved in 350.g of X the solution freezes at 3.7°C instead. Use this information to calculate the molal freezing point depression constant Kf of X. Be sure your answer is rounded to the correct number of significiant digits.
Pure napthalene freezes at 80.6oC and has a freezing point depression constant of 6.9oC/m. The freezing point of a solution containing 7.27 g of an unknown non-ionizing compound in 62.18 g of napthalene is 69.5oC. What is the molar mass of the unknown compound?
A solution consisting of 0.240 mol of methylbenzene, C6H5CH3, in 252 g of nitrobenzene, C6H5NO2, freezes at –0.7°C. Pure nitrobenzene freezes at 6.0°C. What is the freezing-point depression constant of nitrobenzene?
What is the mole fraction of propanol, CH3CH2CH2OH, in the vapor phase from a solution consisting of a mixture of propanol and isopropanol, (CH3)2CHOH, at 25.00 °C, if the total pressure above the solution is 35.29 torr? The vapor pressures of pure propanol and NaN at 25.00 °C are 20.90 torr and 45.20 torr, respectively.
The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is aspirin.Calculate the vapor pressure of the solution at 25 °C when 10.17 grams of aspirin, C9H8O4 (180.1 g/mol), are dissolved in 151.7 grams of diethyl ether.diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol.
The normal freezing point of a certain liquid X is 0.60°C, but when 0.14 kg of barium hydroxide (BaOH2) are dissolved in 900.g of X the solution freezes at −1.6°C instead. Use this information to calculate the molal freezing point depression constant Kf of X. Round your answer to 2 significant digits.
When 224. mg of a certain molecular compound X are dissolved in 45.0 g of cyclohexane (C6H₁2), the freezing point of the solution is measured to be 6.5 °C. Calculate the molar mass of X. If you need any additional information on cyclohexane, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 1 significant digit.
22.7 g of an unknown molecular solute is dissolved in 4.11 moles of phenol (C6H6O), causing the freezing point of phenol to decrease by 3.93 °C. Calculate the molar mass of the solute. For phenol, the molar mass is 94.11 g/mol and Kf = 6.84 °C/m.
The molal boiling point elevation constant K = 1.15 °C·kg⋅mol the solution boils at 145.4 °C. Calculate the boiling point of pure X. Be sure your answer has the correct number of significant digits. °C x10 1 for a certain substance X. When 14.4 g of urea Ś ((NH,),CO) (NH₂) CO) are dissolved in 150. g of X,
Determine the freezing point depression of a solution that contains 30.7 g glycerin (C 3H 8O 3, molar mass = 92.09 g/mol) in 376 mL of water. Some possibly useful constants for water are K f = 1.86°C/ m and K b = 0.512°C/ m. 2.18°C 0.654°C 3.33°C 1.65°C 0.887°C

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