Ethanol molecules have the ability to form Hydrogen bonds with each other ( H from one molecule with O of another).
Propane cannot form hydrogen bonds.
Thus one needs more energy to break these bonds in order to evaporate.
Wiki User
∙ 13y agoEthanol has a higher boiling point than propane because it has stronger intermolecular forces due to hydrogen bonding between its molecules. Propane, on the other hand, is a small nonpolar molecule with weaker London dispersion forces between its molecules. This leads to lower energy required to break the intermolecular forces in propane compared to ethanol, resulting in a lower boiling point.
Wiki User
∙ 13y agoHydrogen Bonding in ethanol but not in propane
Water has a higher boiling point than alcohol. The boiling point of water is 100°C, while the boiling point of alcohol (such as ethanol) is lower, around 78°C.
The higher boiling point of ethanol compared to ether is due to stronger intermolecular forces in ethanol. Ethanol molecules have hydrogen bonding and dipole-dipole interactions, which require more energy to overcome, leading to a higher boiling point. Ether has weaker van der Waals forces between molecules, resulting in a lower boiling point.
C3H8 (propane) has a higher boiling point than C2H6 (ethane) because propane has a larger molecular size and stronger van der Waals forces between its molecules, which require more energy to break and transition to the gas phase.
Ethanol (C2H5OH) has a higher boiling point than methane (CH4) because it has stronger intermolecular forces, specifically hydrogen bonding, which requires more energy to overcome and boil. This results in a higher boiling point for ethanol compared to methane.
Ethanol has a higher boiling point than dimethyl ether because ethanol molecules have stronger intermolecular forces due to hydrogen bonding, while dimethyl ether only has weaker dipole-dipole forces. These stronger hydrogen bonds in ethanol require more energy to break, resulting in a higher boiling point compared to dimethyl ether.
Ethanol (C2H5OH) has a higher boiling point compared to methyl ether (CH3OCH3) due to hydrogen bonding in ethanol. Hydrogen bonding results in stronger intermolecular forces in ethanol, requiring more energy to overcome, hence a higher boiling point.
Oxygen.
I think propane is higher??
Water has a higher boiling point than alcohol. The boiling point of water is 100°C, while the boiling point of alcohol (such as ethanol) is lower, around 78°C.
Ethanol is a better solvent for boiling point elevation compared to water. This is because ethanol has a higher boiling point than water. When a solute is added to ethanol, it will raise the boiling point of the solution more significantly than if the same solute were added to water.
The higher boiling point of ethanol compared to ether is due to stronger intermolecular forces in ethanol. Ethanol molecules have hydrogen bonding and dipole-dipole interactions, which require more energy to overcome, leading to a higher boiling point. Ether has weaker van der Waals forces between molecules, resulting in a lower boiling point.
C3H8 (propane) has a higher boiling point than C2H6 (ethane) because propane has a larger molecular size and stronger van der Waals forces between its molecules, which require more energy to break and transition to the gas phase.
Ethanol (C2H5OH) has a higher boiling point than methane (CH4) because it has stronger intermolecular forces, specifically hydrogen bonding, which requires more energy to overcome and boil. This results in a higher boiling point for ethanol compared to methane.
Ethanol has a higher boiling point than dimethyl ether because ethanol molecules have stronger intermolecular forces due to hydrogen bonding, while dimethyl ether only has weaker dipole-dipole forces. These stronger hydrogen bonds in ethanol require more energy to break, resulting in a higher boiling point compared to dimethyl ether.
Ethanol has a higher boiling point than diethyl ether because ethanol has stronger intermolecular forces due to hydrogen bonding. Hydrogen bonding creates attractions between ethanol molecules, requiring more energy to separate them compared to the weaker London dispersion forces present in diethyl ether. This results in a higher boiling point for ethanol.
It depends what chemical or compound you are comparing the boiling point to. Ethanol has an atmospheric pressure boiling point of 78.1 °C (172.6 °F). This is slightly lower than the boiling point of water at the same pressure, much lower than the boiling point of iron, much higher than the boiling point of bromine.
The boiling point of ethanol is 78.37 degrees Celsius (173.07 degrees Fahrenheit).