A 4.914-g sample of a mixture of cyclohexane (C6H12) and naphthalene (C10H8) is dissolved in 66.40 of benzene (C6H6). The freezing point of the solution is 1.90°C. Calculate the mass percent of the mixture. (See the table for constants.) Normal Normal Solvent Boiling Point (°C/m) Freezing K (°C/m) Point Water 100 0.52 0.0 1.86 Benzene 80.1 2.53 5.5 5.12 Ethanol 78.4 1.22 -117.3 1.99 Acetic Acid 117.9 2.93 16.6 3.90 Cyclohexane 80.7 2.79 6.6 20.0 Naphthalene 80.6 6.9 208 5.95 Cyclohexane %☐ Naphthalene %

A 4.914-g sample of a mixture of cyclohexane (C6H12) and naphthalene (C10H8) is dissolved in 66.40 of benzene (C6H6). The freezing point of the solution is 1.90°C. Calculate the mass percent of the mixture. (See the table for constants.) Normal Normal Solvent Boiling Point (°C/m) Freezing K (°C/m) Point Water 100 0.52 0.0 1.86 Benzene 80.1 2.53 5.5 5.12 Ethanol 78.4 1.22 -117.3 1.99 Acetic Acid 117.9 2.93 16.6 3.90 Cyclohexane 80.7 2.79 6.6 20.0 Naphthalene 80.6 6.9 208 5.95 Cyclohexane %☐ Naphthalene %

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...

See similar textbooks

Similar questions

A solution is prepared by condensing 3.89 L of a gas, measured at 28.1°C and 727 mmHg pressure, into 59.3 g of benzene. Calculate the freezing point of this solution. The normal freezing point of benzene is 5.5°C and benzene has a molar freezing-point depression constant of 5.12 °C/m. °C
4. A 6.06-gram sample of a compound is dissolved in 250. grams of benzene. The freezing point of this solution is 1.02°C below that of pure benzene. What is the molar mass of this compound? (Note: Kę for benzene = 5.12°C/m.)
The boiling point of a solution of 1.056 moles of an electrolyte dissolved in 1399 g of benzene is 83.76 °C. What is the van't Hoff factor for this solution if pure benzene boils at 80.11 °C and its Kb value is 2.53 °C/m?
An ethylene glycol solution contains 21.2 g of ethylene glycol (C2H6O2) in 85.4 mL of water. Determine the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.)
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.
Ethylene glycol (C₂H₆O₂) is used as an additive to the water in your automobile to lower its freezing point. A solution of ethylene glycol in water has a freezing point of -8.10 °C. What is the mole fraction of ethylene glycol in this solution? (Kf for water is 1.86 °C･kg/mol).
A solution contains napthalene (C10H8) dissolved in hexane (C6H14) at a concentration of 10.85% napthalene by mass. Calculate the vapor pressure at 25 degrees celsius of hexane above the solution. The vapor pressure of pure hexane at 25 degrees celsius is 151 torr.
1.613 g sample of an unknown nonionizing molecular compound is added to 250.0 g of benzene(C6H6, MW = 78.11 g/mol). The normal freezing point of the solution is 0.17 C lower than the normalfreezing point of pure benzene. Based on this information, find the molecular weight of the unknowncompound. benzene = Kf = 5.12 kg x Degrees C/mol.
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
The normal boiling point of methanol is 64.7°C. A solution containing a nonvolatile solute dissolved in methanol has a vapor pressure of 670. torr at 64.7°C. What is the mole fraction of methanol in this solution? Mole fraction =
A solution is made using 16.7 percent by mass CH2Cl2 in CHCl3. At 30 °C, the vapor. pressure of pure CH2Cl2 is 490 mm Hg, and the vapor pressure of pure CHCl3 is 260 mm Hg. The normal boiling point of CHCl3 is 61.7 °C. What is the molality of CH2Cl2 in the solution?
Ethylene glycol (C₂H₆O₂) is used as an additive to the water in your automobile to lower its freezing point. A solution of ethylene glycol in water has a freezing point of -5.80°C. What is the mole fraction of ethylene glycol in this solution? (Kf for water is 1.86°C･kg/mol).