**Text Transcription for Educational Website:**A solution containing 6.314 g of a non-volatile organic solute dissolved in 100.00 g of toluene boils at 384.72 K at 1 bar of pressure. The boiling point of pure toluene is 383.75 K and Δ_vapH = 38.06 kJ/mol for benzene.(a) What is the boiling point elevation constant for toluene? (units: kg·K/mol)(b) What is the molar mass (g/mol) of the unknown solute?**Explanation:**This problem involves the concept of boiling point elevation, which is a colligative property of solutions. Such properties depend on the number of solute particles in a solution, not their identity. Since toluene is the solvent, and a non-volatile solute is involved, its boiling point increases when the solute is added. The problem asks for the boiling point elevation constant, a value unique to toluene, and for the molar mass of the solute, which requires calculation.No graphs or diagrams are present to be explained further.

Answer: When a non-volatile is dissolved in a solvent it causes an elevation in the boiling point of…

A solution containing 6.314 g of a non-volatile organic solute dissolved in 100.00 g of toluene boils at 384.72 K at 1 bar of pressure. The boiling point of pure toluene is 383.75 K and AvapH = 38.06 kJ/mol for benzene. (a) What is the boiling point elevation constant for toluene? (units: kg.K/mol) (b) What is the molar mass (g/mol) of the unknown solute?

A solution containing 6.314 g of a non-volatile organic solute dissolved in 100.00 g of toluene boils at 384.72 K at 1 bar of pressure. The boiling point of pure toluene is 383.75 K and AvapH = 38.06 kJ/mol for benzene. (a) What is the boiling point elevation constant for toluene? (units: kg.K/mol) (b) What is the molar mass (g/mol) of the unknown 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

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)
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).
5.152g of Na2CO3(s) is added to 75.0mL of water at 21.20°C. When the dissolution is complete, the final temperature of the solution is measured at 25.00°C. The final volume of the solution is 75.8mL, and the density of water at 21.20°C is 0.99798g/mL. Identify the strongest intermolecular force present in Na2CO3(s): and in water:
What mass in mg hydrogen gas,(2.016 g/mol) is dissolved in 3.82×102 mL of water of water when the partial pressure of hydrogen above the water is 0.57 atm at 25 °C? The Henry's constant for hydrogen gas in water at 25 °C is 7.8×10-4 M/atm.Provide your answer rounded to three significant figures.
(a) Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. CaCl₂(s) Cal₂(s) Lattice Energy -2247 kJ/mol -2059 kJ/mol * Explain. ΔΗ soln -46 kJ/mol -104 kJ/mol *Lattice energy is defined as the energy change for the process M*(g) + X¯(g) → MX(s). calcium chloride 2201 calcium iodide 1955 XkJ/mol X kJ/mol (b) Based on your answers to part (a), which ion, CI or I, is more strongly attracted to water? chloride iodide The enthalpy of hydration for CaCl₂ is more exothermic than for Cal2. Any differences must be due to differences in hydrations between CI and I¯.
Given the following mixture of two compounds 45.00 mL of X (MW =80.00 g/mol)(density 0.893 g/mL) and 885.00 mL of Y (55.00 g/mol))(density 1.280 g/mL). The freezing point of pure Y is 54.00 degrees C. The molal freezing constant is 4.757 degrees C/m. What is the freezing point of the solution.
2) Calculate the vapor pressure caused by the addition of 100.0 g of nonvolatile solid naphthalene (C10H8, 128.17g/mol) into 500.0 g of benzene (C,H6, 78.11g/mol). The vapor pressure of pure benzene at this condition is 42.8 torr.
9.) Using the data below (tabulated at 25 °C), what is the vapor pressure, in kilopascals (kPa), of a solution formed by mixing 5.37 mol of iodomethane (CH3I) with 4.27 mol of trichloromethane (CHCl3) at 25 °C? Assume ideal behavior. Substance Vapor Pressure (kPa) Iodomethane 53.9 Trichloromethane 26.2
Do not give handwriting solution.
When 98.9 g of glycine (C₂H5NO₂) are dissolved in 900. g of a certain mystery liquid X, the freezing point of the solution is 4.7 °C lower than the freezing point of pure X. On the other hand, when 98.9 g of iron(III) nitrate = (Fe(NO3)3): are dissolved in the same mass of X, the freezing point of the solution is 5.4 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits. i= 0