Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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 I g/ml. Previous

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 I g/ml. Previous

Chemistry
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
icon
Related questions
Question
100%
ite arses/2015/assignments/7920 Week 5: Freezing Point Depression of Non-Electrolytes Methanol in Water 10.00 1.00 Data and Calculations: Pure Water 10.00 Volume of Water (ml) Mass of Methanol (g) Freezing Point ('C) Freezing point depression AT Calculate the molality m (K, = 1.86 °C/m for water) Calculate number of moles Tsotution = -4.5 Tsolzent = 1 AT, = Tsotvent – Tsotution = AT = Kf.m→ m = AT;/Kf = m = moles methanol/ Kg solvent → moles methanol = m x Kg solvent = moles methanol = mass methanol /molar mass methanol → molar mass methanol = mass methanol / moles methanol → molar mass methanol = 1.00 g/ moles methanol Calculate the molar mass of methanol e 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. Previous 144 01
Transcribed Image Text:ite arses/2015/assignments/7920 Week 5: Freezing Point Depression of Non-Electrolytes Methanol in Water 10.00 1.00 Data and Calculations: Pure Water 10.00 Volume of Water (ml) Mass of Methanol (g) Freezing Point ('C) Freezing point depression AT Calculate the molality m (K, = 1.86 °C/m for water) Calculate number of moles Tsotution = -4.5 Tsolzent = 1 AT, = Tsotvent – Tsotution = AT = Kf.m→ m = AT;/Kf = m = moles methanol/ Kg solvent → moles methanol = m x Kg solvent = moles methanol = mass methanol /molar mass methanol → molar mass methanol = mass methanol / moles methanol → molar mass methanol = 1.00 g/ moles methanol Calculate the molar mass of methanol e 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. Previous 144 01
Expert Solution
steps

Step by step

Solved in 2 steps with 1 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Solutions
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS