A solution made up of a non-volatile solute in water at 60 °C has a pressure of 130.0 torr. The partial pressure of water is 149.4 torr at 60 °C. What is the mole fraction of the solute? Xsolute = [?] Remember: Psolution = Xsolvent · Psc - . 22 International Academy of Science. All Rights Reserved. X, solute DELL solvent Enter

A solution made up of a non-volatile solute in water at 60 °C has a pressure of 130.0 torr. The partial pressure of water is 149.4 torr at 60 °C. What is the mole fraction of the solute? Xsolute = [?] Remember: Psolution = Xsolvent · Psc - . 22 International Academy of Science. All Rights Reserved. X, solute DELL solvent Enter

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

In a 50.0-g aqueous solution of methanol, CH, O, the mole fraction of methanol is 0.190. What is the mass of each component? mass of CH,O: g CH,O mass of water: g H,0
* 00 les When 634, mg of a certain molecular compound X are dissolved in 60. g of cyclohexane (CH,), the freezing point of the solution is measured to be 6.0 °C. Calculate the molar mass of X. If you need any additional information on cyclohexane, 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. OLX Check Save For Later Submit Assignment O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility EPIC MacBook Pro esc F8 F10 F11 F2 F4 F5 F7 & # $ 2 5. 6. 4. 7. 3. R tab A G os lock C. B. command option control option command
10.Give one example in which a high concentration of a solute is beneficial and one example in which it is harmful 11. Many chemicals that are potentially toxic or harmful to the environment have maximum allowable concentration levels set by government legislation. (a) If the chemical is dangerous, should the limit be zero? (b) Is a zero level theoretically possible? (c) Is a zero-level measurable? (d) If a nonzero limit is set, in your opinion, how should this limit be chosen?
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
The molal freezing point depression constant K, 1.95 °C-kg-mol of X, the solution freezes at 0.4 °C. Calculate the freezing point of pure X. Be sure your answer has the correct number of significant digits. 0rc X 1 for a certain substance X. When 17.0 g of urea a ((NH,),CO) are dissolved in 200. g
A solution was prepared by dissolving 200.0 g of KClKCl in 285 g of water. Calculate the mole fraction of KClKCl. (The formula weight of KClKCl is 74.6 g/molg/mol. The formula weight of water is 18.0 g/molg/mol.) Express the mole fraction of KCl to two decimal places.
3. 2 g of NacI is dissolved in 500 g of water at 35°C. Determine the ff: PNacI • 2.16 cm a. Boiling point elevation b. Freezing point depression C. Vapor pressure of the solution d. Osmotic pre ssure
cvg.cengagenow.com OWLV2 | Online teaching and learning resource from Cengage Learning [Review Topics] [References] Use the References to access important values if needed for this question. The boiling point of chloroform, CHCl3, is 61.70 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in chloroform is estrogen (estradiol). A student dissolves 11.36 grams of estrogen, C₁8H24 O2 (272.4 g/mol), in 170.7 grams of chloroform. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Ethanol Chloroform Benzene Formula H₂O CH3 CH₂OH CHC13 C6H6 Diethyl ether CH3 CH2 OCH2 CH3 The molality of the solution is The boiling point of the solution is Kb (°C/m) Kf (°C/m) 0.512 1.86 1.22 1.99 3.67 2.53 2.02 m. °C. 5.12 +88
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
You must mix 168 g of carbon disulfide (CS2, 76.13 g/mol) with acetonitrile (CH3CN, 41.06 g/mol) to create a solution that has a total vapor pressure of 292 torr at 25°C. Calculate the number of grams of CH3CN required. Substance Vapor Pressure at 25°C (torr) Carbon disulfide 357 Acetonitrile 89.5
A 5.67 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: Kf for benzene = 5.12°C/m.) Ignore significant figures for this problem. 4.52 g/mol А. 56.9 g/mol В. 114 g/mol С. 28.5 g/mol D. OE. 228 g/mol
At a certain temperature the vapor pressure of pure thiophene (C,H,S) is measured to be 0.37 atm. Suppose a solution is prepared by mixing 106. g of thiophene and 93.4 g of acetyl bromide (CH,COB1). Calculate the partial pressure of thiophene vapor above this solution. Round your answer to 2 significant digits. Note for advanced students: you may assume the solution is ideal. atm