10 grams of a non-volatile and non- dissociating solute is dissolved in 200 grams of benzene. The resulting solution boils at a temperature of 81.2°C. Normal boiling point of benzene: 80.1°C Kb benzene: 2.53°C/mol What is the molality of the solution? * Your answer here will be used for the next item/s. Your answer What is the molar mass of the solute?

10 grams of a non-volatile and non- dissociating solute is dissolved in 200 grams of benzene. The resulting solution boils at a temperature of 81.2°C. Normal boiling point of benzene: 80.1°C Kb benzene: 2.53°C/mol What is the molality of the solution? * Your answer here will be used for the next item/s. Your answer What is the molar mass of the solute?

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

Calculate the molar mass of your unknown compound. Data to Use: Concentration (in molality) of unknown solution: 0.0098 m Mass of Cyclohexane (Pure Solvent): 7.726 g Mass of Unknown Compound: 0.302 Freezing Point for Cyclohexane (Pure Solvent): 8.0 degrees Celsius Freezing Point for Unknown Solution: 7.8 degrees Celsius
Which of the following is TRUE about solutions? Select one: please explain why true and why false Solute-solvent interactions will alwaysbe greater than individual solute-solute and solute-solvent interactions When solute-solute molecules are weakly bonded, the temperature of solution will decrease upon mixing Dissolution is favorable when solute-solvent interactions are stronger than solute-solute and solvent-solvent interactions. When solute molecules are strongly attracted to each other, ∆Hsolution> 0
A solution of 0.690 g of an organic compound in 100.0 g of benzene has a freezing point of 5.248°C. What are the molality of the solution and the molar mass of the solute? The normal freezing point of benzene is 5.500°C and the Kf for benzene is 5.12°C/m. Solve for: molality = molar mass =
A 0.32 M aqueous solution of an unknown solute has a density of 1.08 g/mL. The molar mass of the solute is 146.8 g/mol. What is the molality of this solution? Report your answer in mol/kg and round to the second decimal place.
Calculate the freezing point of a solution containing 74.0 g of eucalyptol (C10H8O) solute dissolved in 0.600 kg of CHCl3. The freezing point of pure CHCl3 is -63.5 oC. CHCl3 has a Kf of 4.68 oC/molality. -64.9 oC -67.5 oC -48.3 oC -58.0 oC -69.0 oC -62.1 oC -59.5 oC -78.7 oC
When potassium phosphate is added to water the boiling point increases 50°C. What is the molality of the solution of the solution if the Kbp for water is 0.512°C/m?
Arrange the boiling points of the aqueous solutions, relative to pure water. Assume complete dissociation for the ionic compounds. Highest boiling point H,0 0.13 m K,SO4 0.15 m NaCl 0.18 m C12H„011 0.25 m C12H011 Lowest boiling point Answer Bank help contact us terms of use
Fill in the values for the table. The molar mass of NaCl is 58.443 g/mol Mass of NaCl (g) Mass of solution (g) Volume of solution (mL) Boiling point (C) Mass of water (g) % NaCl (%) Density of Solution (g/mL) Moles of NaCl (mol) Molarity (mol/L) Molality (mol/kg) 0.0000 9.9451 10.00 99.8 c 1.0090 100.3998 100.00 100.4 2.4904 101.4023 100.00 100.8 5.0063 103.2222 100.00 101.5 5.1559 103.0978 100.00 102.1 6.0024 103.4004 100.00 101.1 6.3477 104.9210 100.00 102.7 7.4815 104.5044 100.00 101.8 10.0041 106.2007 100.00 102.1 10.2103 106.6904 100.00 102.8
A solution is prepared at 28°C and its concentration is expressed in three different units: percent by mass, molality, and molarity. If the solution is then heated to 77°C. Which, if any, of these concentration units will change? If none, answer "none".
A newly developed adhesive is found to be a nonelectrolyte upon dissolving in water. A prepared solution has a concentration of 0.843 M. Convert the concentration to molality. The density of the solution is 1.313 g/mL. The molar mass of the compound is 138.3 g/mol. Report your answer to the thousandths place and do not include unit
A solution made by dissolving 150.0 g of an unknown compound in 375.0 mL of benzene to make a solution which has a freezing point 18.6 °C lower than that of pure benzene. Kf for benzene is 5.12 °C/m and the density of benzene is 0.877 g/mL. What was the molality of the solution?
A solution made by dissolving 150.0 g of an unknown compound in 425.0 mL of benzene to make a solution which has a freezing point 18.6 °C lower than that of pure benzene. Kf for benzene is 5.12 °C/m and the density of benzene is 0.877 g/mL. What was the molality of the solution? How many moles of the unknown compound were dissolved in the solution? What is the molar mass of the unknown compound?