When 0.354 g of an unknown nonelectrolyte compound was dissolved in 12.5 g of benzene a solution was formed that froze at 4.46°C. Calculate the molar mass of the unknown compound. The freezing point of benzene is 5.48°C, and the K, of benzene is 5.12 °C/Molal. From the table of unknowns below, select the compound based on your calculated molar mass. Using this value calculate percent error. PLEASE SHOW ALL WORK. You must type your work in the space below. Name Average Molar Mass Kerosene 170 g/mol 2-Propanol 60.1 g/mol Ethyl alcohol 46.1 g/mol 1-methylnapthalene 142.2 g/mol Gasoline 100-105 g/mol

When 0.354 g of an unknown nonelectrolyte compound was dissolved in 12.5 g of benzene a solution was formed that froze at 4.46°C. Calculate the molar mass of the unknown compound. The freezing point of benzene is 5.48°C, and the K, of benzene is 5.12 °C/Molal. From the table of unknowns below, select the compound based on your calculated molar mass. Using this value calculate percent error. PLEASE SHOW ALL WORK. You must type your work in the space below. Name Average Molar Mass Kerosene 170 g/mol 2-Propanol 60.1 g/mol Ethyl alcohol 46.1 g/mol 1-methylnapthalene 142.2 g/mol Gasoline 100-105 g/mol

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

The freezing point of 57.08 g of a pure solvent is measured to be 50.83 ºC. When 2.86 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 48.78 ºC. Answer the following questions ( the freezing point depression constant of the pure solvent is 7.33 ºC·kg solvent/mol solute). Be sure to use the appropriate number of sig figs What is the molality of the solution? How many moles of solute are present? What is the molecular weight of the solute?
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
The presence of a nonvolatile solute causes the freezing point of a solution to be lower than that of the pure solvent. Because freezing point depression depends only on solute concentration and not on the identity of the solute, freezing point depression can be used to determine the molar mass of a solute. The freezing point of a solution prepared by dissolving 127.3 mg of caffeine in 10.0 g of camphor is lower than that of pure camphor (Kf = 39.7°C/m) by 2.61°C. What is the molar mass of caffeine? Elemental analysis of caffeine yields the following results: 49.49% C, 5.15% H, 28.87% N, and the remainder O. What is the molecular formula of caffeine? List the elements in the order given by the elemental analysis.
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?
Suppose that you add 21.1 g of an unknown molecular compound to 0.250 kg of benzene, which has a Kf of 5.12 °C/m. With the added solute, you find that there is a freezing point depression of 2.86 °C compared to pure benzene. What is the molar mass (in g/mol) of the unknown compound?
When 2.85 g of a certain molecular compound X are dissolved in 85. g of dibenzyl ether ((CH₂CH₂)₂O), the freezing point of the solution is measured to be 2 -1.2 °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 the correct number of significant digits. X x10 Ś
We mixed some ethylene glycol with 346 g water to reduce the equilibrium vapor pressure of water from 23.76 Hg to 22.5 Hg at 25°C. The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution. What is the boiling point of this solution? (Hint: find the molality first, and for water, kb = .510 m/°C; boiling point of water: 100.0°C.)
The solubility of a compound (molar mass = 175 g/mol) in water is found to be 7.75 grams per 100.0 grams of water at 25oC. Calculate the molality of the compound in a saturated aqueous solution at 25oC. Your answer should have 3 significant figures. Do not include the units with your answer, but the units should be molality.
A solution is made by dissolving 0.563 mol of nonelectrolyte solute in 821 g of benzene. Calculate the freezing point, Tf, and boiling point, Tp, of the solution. Constants can be found in the table of colligative constants. T = 1.97896467722 °C 78.3650548112 °C Incorrect