GA certain liquid.I has a normal boiling point of 102.60 °C and a boiling point elevation constant K₂ = 0.85 °C-kg-mol¹. A solution is prepared by dissolvingsome ammonium sulfate ((NH4)2SO4) in 400. g of X. This solution boils at 103.8 °C. Calculate the mass of (NH4)2SO4 that was dissolved.Be sure your answer is rounded to the correct number of significiant digits.g☐ x10

To calculate the mass of (NH4)2SO4 that was dissolved in the solution, need to follow these steps:1.…

Answered: G A certain liquid.I has a normal…

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 water is 0.00 °C at 1 atmosphere. A student dissolves 11.60 grams of cobalt(II) sulfate CoSO4, (155.0 g/mol), in 279.3 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kb(C/m) Kf(C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is m. The freezing point of the solution is °C.
Determine the boiling point (in °C) of a solution that contains 45.5 g of MgCl2 dissolved in 685 mL of ethanol (density = 0.789 g/mL). Pure ethanol has a boiling point of 78.3°C and a Kp = 1.07°C/m. %3D
The freezing point of water is 0.00 °C at 1 atmosphere. A student dissolves 11.60 grams of cobalt(II) sulfate CoSO4, (155.0 g/mol), in 279.3 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kb(C/m) Kf(C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is m. The freezing point of the solution is °C.
A chemist is given a nonelectrolyte white powder for analysis. 38.7 g of this substance isdissolved in 100.0 g of water. It is determined that the resulting solution freezes at –4.0°C.Additionally, the elemental composition of the substance is identified and found to be 40.0%C, 6.7% H and 53.3 % O by mass. Find the molecular formula of this unknown white powderusing these experimental evidences (Kf of water: 1.86°C/m, C: 12 g/mol, H: 1 g/mol, O: 16g/mol)
The normal boiling point of a certain liquid X is 140.50 °C, but when 32.3 g of alanine (C,H,NO,) are dissolved in 250. g of X the solution boils at 141.7 °C instead. Use this information to calculate the molal boiling point elevation constant K, of Х. Round your answer to 2 significant digits. olo °C·kg Ar K, = [] mol
5. When 10 g of a certain substance was dissolved in 100 g of water, the boiling point of water became 101.02 ° C. What is the molar mass of this substance? Ebullioscopic elevation Kb = 0.51 K · kg / mol.
The freezing point of benzene, C6H₁, is 5.50 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in benzene is DDT. A student dissolves 11.78 grams of DDT, C14H9 C15 (354.5 g/mol), in 252.1 grams of benzene. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Ethanol Chloroform Benzene Formula H₂O CH3 CH₂ OH CHC13 C6H6 Diethyl ether CH3 CH₂ OCH2 CH3 The molality of the solution is The freezing point of the solution is Kb (°C/m) Kf (°C/m) 1.86 1.99 0.512 1.22 3.67 2.53 2.02 m. °C. 5.12
The molal boiling point elevation constant K,=0.90 °C·kg mol 1 for a certain substance X. When 26. g of urea ((NH.),CO) CO are dissolved in 650. g of X, the solution boils at 137.9 °C. Calculate the boiling point of pure X. Be sure your answer has the correct number of significant digits. °C x10
A 83.5 g sample of a nonelectrolyte is dissolved in 250.1 g of water. The solution is determined to have a boiling point of 102.3 °C. What is the molar mass of the compound? (Kb for water is 0.510 °C/m).
A solution is made by dissolving 38.750 g of sample of an unknown, nonelectrolyte compound in water. The mass of the solution is exactly 500.0 g. The boiling point of this solution is 100.220∘C. What is the molecular weight of the unknown compound?
At a certain temperature the vapor pressure of pure water is measured to be 233. mmHg. Suppose a solution is prepared by mixing 131. g of water and 71.8 g of acetic acid (HCH,CO2). Calculate the partial pressure of water vapor above this solution. Round your answer to 3 significant digits. Note for advanced students: you may assume the solution is ideal. | mmHg x10
The normal freezing point of a certain liquid X is 5.20 °C, but when 41. g of urea (CH,N,O) are dissolved in 750. g of X the solution freezes at 2.5 °C instead. Use this information to calculate the molal freezing point depression constant K, of Х. Round your answer to 2 significant digits. °C·kg x10 K, = 0 mol

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS