Moving to another question will save this response. stion 13 A 11.44 gram sample of a compound with a molar mass of 124.0 g mol~1, when dissolved in 112.9 g of water, gave a solution which had a freezing point -1.46 "C. Calculate the experimental value of the van't Hoff factor. Kf for water = 1.86 °C m-1 (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 12.3 and 123 and 123.) MQuestion 13 of 29

Moving to another question will save this response. stion 13 A 11.44 gram sample of a compound with a molar mass of 124.0 g mol~1, when dissolved in 112.9 g of water, gave a solution which had a freezing point -1.46 "C. Calculate the experimental value of the van't Hoff factor. Kf for water = 1.86 °C m-1 (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 12.3 and 123 and 123.) MQuestion 13 of 29

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...

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A 7.50 g of solid compound RED was dissolved in 100 g water. The freezing point of the solution was found to be 1.20 °C lower than that of pure water (Kf = 1.86 °C/m). What is the molar mass (g/mol) of RED? TYPE THE VALUE ONLY (WITHOUT UNITS). Please show the solution
a). At what temperature would a 1.90 m NaCl solution freeze, given that the van't Hoff factor for NaCl is 1.9? Kf for water is 1.86 ∘C/m . Express your answer with the appropriate units. b). A 0.050 M solution of AlCl3 had an observed osmotic pressure of 3.85 atm at 20 ∘C . Calculate the van't Hoff factor i AlCl3. Express your answer numerically.
Hi, sorry about the unrelated Question I sent previously with the first one. It was related to a different question. a) Calculate and enter the freezing point depression of a solution of 52.4 g ethylene glycol (C2H6O2) in 364 g H2O.Kf for H2O is 1.86 °C kg/mol. b) A solution which contains 77.5 g of an unknown molecular compound in 342 g of water freezes at -5.18°C.What is the molar mass of the unknown? * I got 4.31 degrees celsius for A which was correct. I just need help with B.
A 0.520 g sample of an unknown nonelectrolyte compound is dissolved in 4.10 g of lauric acid (Kf = 3.90 °C/m). The freezing point depression is determine to be 4.20 °C. What is the molar mass of the compound?
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1.613 g sample of an unknown nonionizing molecular compound is added to 250.0 g of benzene(C6H6, MW = 78.11 g/mol). The normal freezing point of the solution is 0.17 C lower than the normalfreezing point of pure benzene. Based on this information, find the molecular weight of the unknowncompound. benzene = Kf = 5.12 kg x Degrees C/mol.
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