Comparing the boiling points of:

A) C3H8
B) C5H12
C) C2H5OH

and identify the folowing statements as either True or False:

Dispersion forces only for (A)
Boiling point (C) > Boiling point (A)
(B) exhibits hydrogen bonding
Boiling point (C) < Boiling point (A)
(A) exhibits hydrogen bonding
Boiling point (A) < Boiling point (B)
Boiling point (B) < Boiling point (C)
Dispersion forces only for (C)
Boiling point (B) > Boiling point (C)
Dispersion forces only for (B)
(C) exhibits hydrogen bonding
Boiling point (A) > Boiling point (B)

This should get you started since both A and B are hydrocarbons. C is an alcohol and will exhibit hydrogen bonding; therefore, it will boil higher than either A or C.

http://www.elmhurst.edu/~chm/vchembook/501hcboilingpts.html

To determine the boiling points and whether or not hydrogen bonding and dispersion forces are present, we need to consider the molecular structure and intermolecular forces of each compound.

A) C3H8 (propane):
- Propane is a nonpolar molecule, so it only exhibits dispersion forces. Dispersion forces are the weakest intermolecular forces.
- Boiling point: Since propane only experiences dispersion forces, which are relatively weak, it will have the lowest boiling point among the given compounds.

B) C5H12 (pentane):
- Pentane is also a nonpolar molecule, so it only exhibits dispersion forces. Again, dispersion forces are the weakest intermolecular forces.
- Boiling point: Similar to propane, pentane is larger in size and has more electrons, so it will have a higher boiling point than propane but lower than the compound with hydrogen bonding.

C) C2H5OH (ethanol):
- Ethanol is a polar molecule due to the presence of the hydroxyl (-OH) group, and it exhibits hydrogen bonding. Hydrogen bonding is a stronger intermolecular force compared to dispersion forces.
- Boiling point: Hydrogen bonding leads to stronger intermolecular attractions, so ethanol has the highest boiling point among the given compounds.

Now let's go through each statement:

1) Dispersion forces only for (A) - TRUE
2) Boiling point (C) > Boiling point (A) - TRUE
3) (B) exhibits hydrogen bonding - FALSE (Pentane does not have a hydrogen bonding group like -OH or -NH)
4) Boiling point (C) < Boiling point (A) - FALSE (Ethanol has a higher boiling point than propane)
5) (A) exhibits hydrogen bonding - FALSE (Propane does not have a hydrogen bonding group like -OH or -NH)
6) Boiling point (A) < Boiling point (B) - TRUE
7) Boiling point (B) < Boiling point (C) - TRUE
8) Dispersion forces only for (C) - FALSE (Ethanol exhibits hydrogen bonding in addition to dispersion forces)
9) Boiling point (B) > Boiling point (C) - FALSE (Ethanol has a higher boiling point than pentane)
10) Dispersion forces only for (B) - TRUE
11) (C) exhibits hydrogen bonding - TRUE
12) Boiling point (A) > Boiling point (B) - FALSE (Propane has a lower boiling point than pentane)

So the correct statements are:
1) TRUE
2) TRUE
3) FALSE
4) FALSE
5) FALSE
6) TRUE
7) TRUE
8) FALSE
9) FALSE
10) TRUE
11) TRUE
12) FALSE

To compare the boiling points of these compounds, we need to consider their molecular structures, intermolecular forces, and molecular weights.

A) C3H8 (Propane):
- It is a simple alkane with no polar functional groups.
- The only intermolecular force present is dispersion force.
- Boiling point is relatively low due to weaker intermolecular forces.
- Dispersion forces only for (A) - True.

B) C5H12 (Pentane):
- It is also an alkane with no polar groups.
- Similar to propane, it exhibits dispersion forces.
- Boiling point is higher compared to propane due to the larger size and greater surface area.
- Dispersion forces only for (B) - True.

C) C2H5OH (Ethanol):
- It contains an -OH group, making it a polar molecule.
- In addition to dispersion forces, it can also form hydrogen bonds.
- Boiling point is higher due to stronger intermolecular forces.
- Boiling point (C) > Boiling point (A) - True.
- (B) exhibits hydrogen bonding - False.
- Boiling point (C) < Boiling point (A) - False.
- (A) exhibits hydrogen bonding - False.
- Boiling point (A) < Boiling point (B) - False.
- Boiling point (B) < Boiling point (C) - False.
- Dispersion forces only for (C) - False.
- Boiling point (B) > Boiling point (C) - False.
- Dispersion forces only for (B) - False.
- (C) exhibits hydrogen bonding - True.
- Boiling point (A) > Boiling point (B) - False.

To summarize:
- Dispersion forces only for (A) - True.
- Boiling point (C) > Boiling point (A) - True.
- (B) exhibits hydrogen bonding - False.
- Boiling point (C) < Boiling point (A) - False.
- (A) exhibits hydrogen bonding - False.
- Boiling point (A) < Boiling point (B) - False.
- Boiling point (B) < Boiling point (C) - False.
- Dispersion forces only for (C) - False.
- Boiling point (B) > Boiling point (C) - False.
- Dispersion forces only for (B) - False.
- (C) exhibits hydrogen bonding - True.
- Boiling point (A) > Boiling point (B) - False.