A solution is prepared by dissolving 4.39 g of ordinary sugar (sucrose, C12H011, molecular weight = 342 amu) in 38.3 g of water. Calculate the freezing point of the solution. Sucrose is a nonvolatile nonelectrolyte. Solvent T ("C) T:("C) (°C kg/mol) (°C kg/mol) Benzene, C,Hs 80.1 2.53 5.5 5.10 Camphor, C10H16O 204 5.95 176 37.7 Cyclohexane, C&H12 80.88 2.79 6.50 20.2 Nitrobenzene, C H5 NO2 210.8 5.24 5.7 8.1 Water, H20 100.0 0.512 0.00 1.86 °C

A solution is prepared by dissolving 4.39 g of ordinary sugar (sucrose, C12H011, molecular weight = 342 amu) in 38.3 g of water. Calculate the freezing point of the solution. Sucrose is a nonvolatile nonelectrolyte. Solvent T ("C) T:("C) (°C kg/mol) (°C kg/mol) Benzene, C,Hs 80.1 2.53 5.5 5.10 Camphor, C10H16O 204 5.95 176 37.7 Cyclohexane, C&H12 80.88 2.79 6.50 20.2 Nitrobenzene, C H5 NO2 210.8 5.24 5.7 8.1 Water, H20 100.0 0.512 0.00 1.86 °C

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

12.57 Pheromones are compounds secreted by the females of many insect species to attract males. One of these compounds contains 80.78 percent C, 13.56 percent H,and 5.66 percent O. A solution of 1.00 g of this pheromone in 8.50 g of benzene freezes at 3.37°C. What are the molecular formula and molar mass of the compound? (The normal freezing point of pure benzene is 5.50°C.)
An aqueous solution is 15.2% copper (II) chloride (CuCl2) and has a density1.089 g/mL (a) What is the molality (m) of this solution? (b) What is the mole fraction (ΧB) of CuCl2 in this solution? (c) What is the molarity (M) of this solution?
An antifreeze solution is prepared by mixing 1.00 L of water and 946 mL of ethylene glycol, C,H,O2 (molar mass = 62.07 g/mol). Calculate: (a) the mass percent of ethylene glycol in the mixture; (b) the mole fraction of ethylene glycol in the solution, and (c) the molality of ethylene glycol in the solution. (d) Determine the freezing point and boiling point of the solution. (Assume density of water = 1.00 g/mL; Kf= 1.86°C/m; K = 0.512°C/m; density of EG = 1.114 g/mL)
A solution is prepared by mixing 50.0 mL of ethanol (C2H5OH; molar mass = 46.068 g/mol) in 100.0 mL of water at 20°C. The density of water and ethanol at 20°C are 1.00 g/mL and 0.789 g/mL, respectively. What is the molality of ethanol? (A) 0.086 m (B) 0.094 m (C) 1.24 m (D) 8.56 m
A chemist is studying small organic compounds for theirpotential use as an antifreeze. When 0.243 g of a compound isdissolved in 25.0 mL of water, the freezing point of the solutionis -0.201°C. (a) Calculate the molar mass of the compound (dof water 1.00 g/mL). (b) Analysis shows that the compoundis 53.31 mass % C and 11.18 mass % H, the remainder being O.Calculate the empirical and molecular formulas of the com-pound. (c) Draw a Lewis structure for a compound with this for-mula that forms H bonds and another for one that does not.
An antifreeze solution contains 1.00 kg of ethylene glycol (C2H6O2; molar mass = 62.07 g/mol) in 1.25 kg of water. Determine: (a) the molal concentration (m) of ethylene glycol; (b) the freezing point of solution, and (c) the boiling point of solution. (The freezing point depression constant, Kf = 1.86oC/m; the boiling point elevation constant, Kb = 0.512oC/m, where m = molal concentration).
A solution is prepared by dissolving 8.28 g of ordinary sugar (sucrose, C12H22011, molecular weight = 342 amu) in 34.7 g of water. Calculate the freezing point of the solution. Sucrose is a nonvolatile nonelectrolyte. Solvent T("C) T:(°C) (°C kg/mol) (°C kg/mol) Benzene, C, Hs 80.1 2.53 5.5 5.10 Camphor, C10 H160 204 5.95 176 37.7 Cyclohexane, CH12 80.88 2.79 6.50 20.2 Nitrobenzene, 210.8 5.24 5.7 8.1 Cg H5 NO2 Water, H20 100.0 0.512 0.00 1.86 -7.812 X °C
(d) Determine the freezing point and boiling point of the solution. (Assume density of water = 1.00 g/mL; Kf= 1.86oC/m; Kb= 0.512oC/m; density of EG = 1.114 g/mL
A sports drink formulation can be prepared by mixing the ingredients in the quantities shown in the table below. Calculate the freezing point of this drink formulation. (Kffor water is 1.86 °C kg mol-1 and the molar mass of sucrose is 342.3 g mol-¹). Ingredient Mass (g) NaCl 1.2 0.49 KCI Sucrose (C12H22011) 60 1000 water O a. -0.38 °C O b.-0.43 °C O c. -0.10 °C O d. -0.32 °C O e. -0.75 °C Which ONE of the following saturated aqueous salt solutions will contain the highest total concentration of ions at 25°C? a. AgCl = 1.8 x 10-10) (Ksp (Ksp = 3.9 × 10-11) O b. CaF2 OC. Ag2CO3 O d. COCO3 (Ksp (Ksp = 1.0 x = 8.1 x 10-12) 10-10) The highest amount of solid Cul2 will dissolve in 1.0 L of an aqueous solution of: a. 0.5 M CaCl2 b. 0.5 M Cu(NO3)2 O c.0.5 M Cul2 O d. 0.5 M NH4I O e. 0.5 M CuCl2
Pentane (C5H12) and hexane (C6H14) form ideal solution. At 25oC the vapor pressure of pentane and hexane are 511 torr and 150. torr, respectively. A solution is prepared by mixing 30.0mL pentane (density = 0.63g/mL) with 45.0mL hexane (density = 0.66 g/mL). (a) What are the mole fractions of pentane and hexane, respectively,in the solution? (b) What isthe total vapor pressure of the solution at 25oC? (c) What are the mole percent of pentane and hexane, respectively, in the vapor phase at 25oC? (Molar mass of pentane and hexane are: 72.15 g/mol and 86.17 g/mol, respectively.)
Do not give handwriting solution.
When 4.59 g of a certain molecular compound X are dissolved in 35. g of dibenzyl ether ((C%H,CH,),°). the freezing point of the solution is measured to be 0.9 °C. Calculate the molar mass of X. If you need any additional information on dibenzyl ether, 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. 0 00 0.0 X x10