Ethanol and dimethyl ether has same molecular formula, C 2 H 6 O. The reason behind the fact that dimethyl ether has a boiling point that is lower than the boiling point of ethanol is to be explained. Concept Introduction: The various kinds of interactions that bind a molecule together are known as intermolecular forces. These forces can be dispersion, dipole-dipole, ion-dipole, and hydrogen bonding. The boiling point of a substance depends upon the intermolecular forces present in a molecule. When hydrogen is covalently bonded to a very small, highly electronegative atom (usually fluorine, oxygen, or nitrogen), the result is a molecule with a large dipole moment. This leads to a particularly strong type of dipole–dipole attraction traditionally called hydrogen bonding
Ethanol and dimethyl ether has same molecular formula, C 2 H 6 O. The reason behind the fact that dimethyl ether has a boiling point that is lower than the boiling point of ethanol is to be explained. Concept Introduction: The various kinds of interactions that bind a molecule together are known as intermolecular forces. These forces can be dispersion, dipole-dipole, ion-dipole, and hydrogen bonding. The boiling point of a substance depends upon the intermolecular forces present in a molecule. When hydrogen is covalently bonded to a very small, highly electronegative atom (usually fluorine, oxygen, or nitrogen), the result is a molecule with a large dipole moment. This leads to a particularly strong type of dipole–dipole attraction traditionally called hydrogen bonding
Solution Summary: The author explains that dimethyl ether has a lower boiling point than ethanol because of hydrogen bonding.
Ethanol and dimethyl ether has same molecular formula, C2H6O. The reason behind the fact that dimethyl ether has a boiling point that is lower than the boiling point of ethanol is to be explained.
Concept Introduction:
The various kinds of interactions that bind a molecule together are known as intermolecular forces. These forces can be dispersion, dipole-dipole, ion-dipole, and hydrogen bonding.
The boiling point of a substance depends upon the intermolecular forces present in a molecule.
When hydrogen is covalently bonded to a very small, highly electronegative atom (usually fluorine, oxygen, or nitrogen), the result is a molecule with a large dipole moment. This leads to a particularly strong type of dipole–dipole attraction traditionally called hydrogen bonding
32. Consider a two-state system in which the low energy level is 300 J mol 1 and the higher energy
level is 800 J mol 1, and the temperature is 300 K. Find the population of each level. Hint: Pay attention
to your units.
A. What is the partition function for this system?
B. What are the populations of each level?
Now instead, consider a system with energy levels of 0 J mol
C. Now what is the partition function?
D. And what are the populations of the two levels?
E. Finally, repeat the second calculation at 500 K.
and 500 J mol 1 at 300 K.
F. What do you notice about the populations as you increase the temperature? At what temperature
would you expect the states to have equal populations?
30. We will derive the forms of the molecular partition functions for atoms and molecules shortly in
class, but the partition function that describes the translational and rotational motion of a homonuclear
diatomic molecule is given by
Itrans (V,T) =
=
2πmkBT
h²
V
grot (T)
4π²IKBT
h²
Where h is Planck's constant and I is molecular moment of inertia.
The overall partition function is qmolec Qtrans qrot.
Find the energy, enthalpy, entropy, and Helmholtz free energy for the translational and rotational
modes of 1 mole of oxygen molecules and 1 mole of iodine molecules at 50 K and at 300 K and with a
volume of 1 m³. Here is some useful data:
Moment of inertia:
I2 I 7.46 x 10-
45
kg m²
2
O2 I 1.91 x 101
-46
kg m²
K
for each reaction step.
Be sure to account for all bond-breaking and bond-making
steps.
HI
HaC
Drawing Arrows!
H3C
OCH3
H
4 59°F
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H
CH3
HO
O
CH3
'C'
CH3
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CH3 1
L
H&C.
OCH3
H H H
H
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Problem 30 of 20
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H3C
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H
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CH3
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H2C
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