Consider the two molecules CH4 and C6H12. At room temperature and 1 atm pressure, CH4 is a gas and C6H12 is a liquid. Why is C6H12 a liquid instead of a gas like CH4? A C6H12 has hydrogen bonding B C6H12 has greater dispersion forces C CH4 has ion - ion forces D C6H12 has ion - ion forces E CH4 has dipole - dipole forces
Consider the two molecules CH4 and C6H12. At room temperature and 1 atm pressure, CH4 is a gas and C6H12 is a liquid. Why is C6H12 a liquid instead of a gas like CH4? A C6H12 has hydrogen bonding B C6H12 has greater dispersion forces C CH4 has ion - ion forces D C6H12 has ion - ion forces E CH4 has dipole - dipole forces
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter14: Liquids And Solids
Section: Chapter Questions
Problem 1STP
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Question
Consider the two molecules CH4 and C6H12. At room temperature and 1 atm pressure, CH4 is a gas and C6H12 is a liquid. Why is C6H12 a liquid instead of a gas like CH4?
A |
C6H12 has hydrogen bonding |
|
B |
C6H12 has greater dispersion forces |
|
C |
CH4 has ion - ion forces |
|
D |
C6H12 has ion - ion forces |
|
E |
CH4 has dipole - dipole forces |
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