Freezing point depression AT, AT, Calculate the molality m (K, = 1.86 °C/m for water) Tsolvent = Tsotution = AT, = Kf.m → m = AT;/Kf = %3! m = moles methanol/ Kg solvent → moles methanol = m x Kg solvent = Calculate number of moles Calculate the molar mass of methanol moles methanol = mass methanol / molar mass methanol → molar mass methanol = mass methanol / moles methanol → molar mass methanol = 1.00 g / moles methanol error (actual molar mass of methanol = %error =[ |actual – experimental| / actual ] x 100% 32.04 g/mol) Question: 1. What is the freezing point of a solution prepared by dissolving 20 g of ethanol (Molar mass = 46 g/mol) in 120 mL of water? The freezing point depression constant K, for water is 1.86 °C/m. Assume density of water is 1 g/ml.

Freezing point depression AT, AT, Calculate the molality m (K, = 1.86 °C/m for water) Tsolvent = Tsotution = AT, = Kf.m → m = AT;/Kf = %3! m = moles methanol/ Kg solvent → moles methanol = m x Kg solvent = Calculate number of moles Calculate the molar mass of methanol moles methanol = mass methanol / molar mass methanol → molar mass methanol = mass methanol / moles methanol → molar mass methanol = 1.00 g / moles methanol error (actual molar mass of methanol = %error =[ |actual – experimental| / actual ] x 100% 32.04 g/mol) Question: 1. What is the freezing point of a solution prepared by dissolving 20 g of ethanol (Molar mass = 46 g/mol) in 120 mL of water? The freezing point depression constant K, for water is 1.86 °C/m. Assume density of water is 1 g/ml.

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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The formula for freezing point depression is AT = а. Кm O b. K/ws/mol O c. w/Ws m с. Od. MW/kw Previous page Type here to search DOLL
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