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?

FREE Expert 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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Problem Details

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?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Mole Fraction concept. You can view video lessons to learn Mole Fraction. Or if you need more Mole Fraction practice, you can also practice Mole Fraction practice problems.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.