When 64.8 g of sucrose was dissolved in 100g of water, the freezing temperature ofwater was measured as -3.52 \deg C. a) Find the freezing point depression constant ofwater. (Msucrose: 342.2965 g/mol) b) If 32 g of A is dissolved in 100 g of water, thefreezing point decrease is 8 \deg C. What is the molecular weight of substance A?

a) -.1862 °Ckg/mol b) 74.5 g/molExplanation:

Answered: When 64.8 g of sucrose was dissolved in…

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

If a 36.0-g sample of a molecular compound (i-1) is dissolved in 224.0 g of water, the freezing point of the solution was measured at - 0.94°C. What is the molar mass of the compound in g/mol? (K, for water is 1.858°C/m.) O 160 O 480 320 280
3) Calculate the freezing point (oC) of a solution of 15.46 g of acetone (CH3COCH3, MM = 58.08 g/mol) in 85.0 g of CCl4, whose normal freezing point is –23.0 oC. Given: P = 1 atmKf CCl4 = 29.8 oC/m a) –55.6 b) –93.3 c) 35.7 d) –76.4 e) 70.3 f) –116
A solution is made by dissolving 0.0607 kg of biphenyl (C₁₂H₁₀) in 350.0 mL of benzene (C₆H₆). a) If the boiling point of pure benzene is 80.1 °C, then what would be the boiling point of this solution in °C? (Kb for benzene is 2.53 °C/m and the density of benzene is 0.877 g/mL) b) If the vapor pressure of pure benzene is 24.4 kPa at 40.0 °C, then what will the vapor pressure of the solution be in kPa? (Consider biphenyl to be nonvolatile and the density of benzene is 0.877 g/mL) c) What would be the osmotic pressure (in atm) of this solution at 40.0 °C? (The density of benzene is 0.877 g/mL.)
What molality of NaCl is required to increase the boiling point of 500 g of water to 105°C? (K is on the cover sheet)
Moving to another question Wll tion 10 Calculate the molality of C2H5OH (molar mass = 46.068 g mol-1) in a water solution that is prepared by mixing 40.17 g of C2H5OH with 441.6 mL of H2U at 20 °C. (Density of water 1.00 g mL) (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) K Question 10 of 29 A Moving to another question will save this response. 211 * LO, %23 24 & 2. 3 8 delete 4 E R Y [O P ente S D F G K L. ret C- V alt alt option n command command option
When 0.4129 grams of menthol (MW: 156.27 g/mol) is dissolved in a certain amount of cyclohexane, the freezing point of the solution is lowered by 3.93 ∘C. The ?f constant for cyclohexane is as follows: ?f= 20.8 oC/m. Calculate the mass of the cyclohexane in grams.
What is the boiling point of a solution of 0.186 g of glycerol, C3 Hg O3, in 20.0 g of water? For water, K, = 0.512°C/ and 1.858°C, (Round your answer tO three decimal places.) Boiling point = °C What is the freezing point? Freezing point = °C
Pls answer number 13 and 14 with solution
KS- Latoya Johnson - Learn = O STATES OF MATTER Calculating molality molarity = 0 molality Explanation Say y google - Yahoo Search Results A student dissolves 8.5 g of resveratrol (C₁4H1203) in 475. mL of a solvent with a density of 1.04 g/mL. The student notices that the volume of the solvent does not change when the resveratrol dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits. Check 믐 X OxO y mohela loan status - Yahoo Search R... $ Public Service Loan Forgiveness Wa.... MacBook Air 1/3 Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A
Anthraquinone contains 80.8 % carbon, 3.8 % hydrogen and 15.4 %oxygen. The freezing point of camphor is lowered by 22.3 C when 1.32 g of anthraquinone is dissolved in 11.4 g camphor. (kf = 40.0 C/m, bp = 178.40 C)a. What is the empirical formula of anthraquinone?b. What is the molar mass of anthraquinone?c. What is the molecular formula of anthraquinone?
0.0851 kg of biphenyl (C H,) is dissolve in benzene (CH) to create a solution with a total volume of 350.0 mL. (Assume the change in volume is negligible) If the boiling point of pure benzene is 80.1 °C, then what would be the boiling point of this solution in °C? (Kb for benzene is 2.53 °C/m and the density of benzene is 0.877 g/mL)
Pls answer number 11 and 12 with solution

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