Question

C3H8 has a boiling point than C2H6

Answer 1

Propane (C3H8) has a higher boiling point than ethane (C2H6) because as the size and mass of the alkane molecules increase, so do the London dispersion forces, which are the only intermolecular forces in these nonpolar molecules.

Step-by-step explanation:

The boiling point of hydrocarbons such as alkanes increases with the molecular size and mass. This is because London dispersion forces, which are the only intermolecular forces present in nonpolar molecules like C3H8 (propane) and C2H6 (ethane), become stronger as the size of the molecule increases. Therefore, the statement C3H8 has a higher boiling point than C2H6 is accurate, as propane (C3H8) is a larger molecule than ethane (C2H6). This trend continues with even larger alkanes, such as C4H10 (butane), which have an even higher boiling point due to larger London dispersion forces.

For comparison, polar molecules with a permanent dipole moment experience stronger dipole-dipole interactions than London dispersion forces, leading to a higher boiling point. Aldehydes and alcohols also have higher boiling points due to their functional groups that allow for dipole-dipole interactions and, in the case of alcohols, hydrogen bonding.

Answer 2

C₃H₈ has a higher boiling point than C₂H₆

Step-by-step explanation:

The boiling point is the temperature at which the intermolecular bonds holding molecules in liquid form are overcome and change the state into a gas. C₃H₈ experiences stronger intermolecular bonds then C₂H₆ because it has more carbons. While the strength of each bond is the same between the two molecules, C₃H₈ has more opportunities to create these bonds due to the higher carbon count. The more bountiful the intermolecular bonds, the more energy is needed to overcome them all. Thus, C₃H₈ has a higher boiling point.