The greater the potential of a liquid's molecules to interact with each other through intermolecular forces, the lower the vapour pressure is going to be above the liquid (because molecules will preferentially stay liquid and interact with other molecules rather than fly away as a gas), and the lower the boiling point of the liquid. Therefore the relationship is an inverse one.
The liquid with the highest heat of vaporization (400 J) will have the strongest intermolecular forces of attraction. This is because a higher heat of vaporization indicates that more energy is required to overcome the intermolecular forces holding the liquid molecules together, resulting in stronger attractions between the molecules.
The correct answers are: Capillary attraction; Melting point; and Heat of vaporization. Stronger intermolecular forces increase capillary attraction, melting point, and the heat of vaporization. They have no bearing on conductivity and hardness.A.HardnessB.ConductivityC.Capillary attractionD.Melting pointE.Heat of vaporization
Smallest intermolecular forces of attraction
The enthalpy of vaporization is positive because energy is required to break the intermolecular forces holding liquid molecules together and convert them into vapor. This energy input is needed to overcome the attractive forces between the molecules in the liquid phase.
Chloroform's low heat of vaporization is likely due to its relatively weak intermolecular forces compared to other liquids. These weak forces make it easier for chloroform molecules to escape the liquid phase and enter the vapor phase at lower temperatures.
The liquid with the highest heat of vaporization (400 J) will have the strongest intermolecular forces of attraction. This is because a higher heat of vaporization indicates that more energy is required to overcome the intermolecular forces holding the liquid molecules together, resulting in stronger attractions between the molecules.
The correct answers are: Capillary attraction; Melting point; and Heat of vaporization. Stronger intermolecular forces increase capillary attraction, melting point, and the heat of vaporization. They have no bearing on conductivity and hardness.A.HardnessB.ConductivityC.Capillary attractionD.Melting pointE.Heat of vaporization
Yes, the process of vaporization does require an input of energy. The energy is required to break the intermolecular forces of a given substance. The intermolecular forces is usually very strong.
Smallest intermolecular forces of attraction
The enthalpy of vaporization is positive because energy is required to break the intermolecular forces holding liquid molecules together and convert them into vapor. This energy input is needed to overcome the attractive forces between the molecules in the liquid phase.
A volatile liquid is easy to vaporize because there are weak intermolecular attractions between its molecules. A nonvolatile liquid is difficult to vaporize because there are strong intermolecular attractions between its molecules.
Chloroform's low heat of vaporization is likely due to its relatively weak intermolecular forces compared to other liquids. These weak forces make it easier for chloroform molecules to escape the liquid phase and enter the vapor phase at lower temperatures.
Evaporation occur when intermolecular forces weakened.
A low boiling point, high vapor pressure, and low viscosity are indicators of weak intermolecular forces in a liquid. These properties suggest that the molecules in the liquid are easily separated and can escape into the gas phase more readily.
The strength of intermolecular forces is directly related to the boiling point of a substance. Substances with stronger intermolecular forces require more energy to break those forces, leading to a higher boiling point. Conversely, substances with weaker intermolecular forces have lower boiling points.
Vaporization reactions typically require energy input to break intermolecular forces and change a substance from liquid to gas state, making them endothermic (positive ΔH or enthalpy). The process absorbs heat from the surroundings to overcome forces of attraction between molecules, resulting in a cooling effect.
The movement of particles increases during vaporization as they gain more energy to overcome intermolecular forces and transition from a condensed phase to a gaseous phase.