How can we complete part 2 using vaporization? **General Chemistry 1****Part II. Enthalpy of vaporization, bp, and vapor pressure from IMFs.**In part II of today’s workshop, you will practice identifying IMFs and predicting their effect on boiling point, vapor pressure, and enthalpy of vaporization (\( \Delta H_{\text{vap}} \)).The \( \Delta H_{\text{vap}} \) for a given molecule is the energy required to transform a given quantity of a substance from the liquid phase to the gaseous phase. \( \Delta H_{\text{vap}} \) values are usually measured in units of kJ/mol just like the \( \Delta H_{\text{rxn}} \) that we looked at in Topic 6.For each of the following pairs, list IMFs and predict which liquid would have the higher boiling point, vapor pressure, and \( \Delta H_{\text{vap}} \). In each case, you MUST explain your answer using IMFs.**HINT:** Think about the structures of the molecules.a) \( \text{CH}_3\text{COCH}_2 \text{CH}_2 \) (butanone) vs. \( \text{CH}_3\text{CHOHCH}_2\text{CH}_3 \) (2-butanol)b) \( \text{C(CH}_3\text{)}_4 \) (2,2-dimethylpropane) vs. \( \text{CH}_3\text{CH}_2\text{CH}_2\text{CH}_2\text{CH}_3 \) (pentane)c) \( \text{ICl} \) vs. \( \text{Br}_2 \)e) \( \text{CH}_3\text{CH}_2\text{CH}_2\text{NH}_2 \) vs. \( \text{N(CH}_3\text{)}_3 \)---Page number: 5

Boiling point is the temperature required to transform liquid to gas . Where vapor pressure is the pressure that exerted by vapors on liquid surface when liquid and vapor is in equilibrium with eachother. Thus with increasing in strength of intermolecular interaction force of interaction, more energy is required to break the bond among the molecules, thus higher temperature is required, thus both boiling point and dHvap will increases . But amount of vapor decreases, thus vapor pressure will also decreases. Note: As per our company guideline we can answer only three subparts. Kindly repost the question mentioning the parts of question to be answered.