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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
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Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
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Ch.19 - Nuclear Chemistry
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Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Methanol (CH3OH) and ethanol (C2H5OH) are miscible because the major intermolecular force for each is H bonding. In some methanol-ethanol solutions, the mole fraction of methanol is higher, but the ma

Solution: Methanol (CH3OH) and ethanol (C2H5OH) are miscible because the major intermolecular force for each is H bonding. In some methanol-ethanol solutions, the mole fraction of methanol is higher, but the ma

Problem

Methanol (CH3OH) and ethanol (C2H5OH) are miscible because the major intermolecular force for each is H bonding. In some methanol-ethanol solutions, the mole fraction of methanol is higher, but the mass percent of ethanol is higher. What is the range of mole fraction of methanol for these solutions?

Solution

Recall: Mole fraction is calculated by:

The problem states that when the mole fraction of methanol is higher, the mass percent of ethanol is higher. The range of the mole fraction is in between the point where moles of ethanol = moles of methanol and the point where the mass of ethanol > mass of methanol.

This means the mole fraction of ethanol ranges from 0.51 to a higher value, which can be approximated by using a mass percent where the mass of ethanol is just slightly greater than that of methanol.

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