A student determines the molar mass of methanol, CH3OH by the same method used in this experiment. She found that the equilibrium temperature of ice and pure water was 0.4 ˚C. When she added 10.0 g of her sample (CH3OH), it fell to -5.4˚C. The mass of the solution was 101.8 g.What was the freezing point depression?What was the molality of CH3OH?How many moles of CH3OH are in the solution?Find the molar mass of CH3OH from the experimental data. How does it compare the value calculated from the periodic table?

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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 student determines the molar mass of methanol, CH3OH by the same method used in this experiment. She found that the equilibrium temperature of ice and pure water was 0.4 ˚C. When she added 10.0 g of her sample (CH3OH), it fell to -5.4˚C. The mass of the solution was 101.8 g.

What was the freezing point depression?
What was the molality of CH3OH?
How many moles of CH3OH are in the solution?
Find the molar mass of CH3OH from the experimental data. How does it compare the value calculated from the periodic table?

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