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Heptane, octane, and nonane are alkanes that only contain London-dispersion forces. And of these three alkanes, nonane has the strongest intermolecular forces. When dealing with London dispersion forces, the strongest intermolecular forces are found with the substance that has the highest molecular mass. This is because the stronger the intermolecular forces are, the fewer molecules that have enough kinetic energy to evaporate. This can be seen for nonane in the graph: the temperature decrease for nonane was the steepest out of the three because it lost the least amount of energy from evaporation (See Figure 1).

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For Fraction 1, below 110 degree Celsius (approximately 63 degree Celsius) because that is the boiling point for 1-hexene. For Fraction 2, around 143 degree Celsius because that is the boiling temperature for 2-bromohexane.

As a student, it can sometimes be arduous to navigate the multitude of available publications and properly format each reference. While the in-text citation guidelines for APA

Butanoic Acid, however, has a much higher boiling point than all three ketones. Butanoic acid does not have the highest molecular mass. This phenomenon can be attributed to hydrogen bonding. Due to the way the carboxylic molecule is arranged,

The basis of this project is to measure the time it takes for isopropyl alcohol, 100% acetone, and water to evaporate. Also calculating which liquid evaporated more quickly, when apply to heat. In addition, to examine the structure of each liquid to understand the reason each liquid evaporate at the rate it does.

Figure 1 shows 2-hexanone. This is a straight-chain ketone with the functional group oxygen attached to the second carbon (as highlighted). This is has the highest boiling point due to the absence of branching to decrease bonding strength and has a six carbon backbone. Similarly to Figure 2, both 2-hexanol has a similar structure, however 2-pentanone has a five carbon backbone. Its lower boiling point is attributed to the shorter chain length.

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1-Propanol is in the middle with a boiling point of 97oC. The molecule is like propionic acid because the molecule also has a hydrogen bond (O-H) but, it differs because the second carbon on 1-propanol contains a non-polar covalent bond (Van der Waals forces) instead of dipole interactions. 1-propanol also contains a strand of hydrocarbons which increases Van der Waals forces so to larger surface area. Lastly propionaldehyde has a boiling point of 48oC because it does not contain any hydrogen bonding. The only intermolecular interactions in propionaldehyde are dipole forces and Van der Waals

There is a very large difference between methanol and ethane in their boiling points despite their similarity in molar mass. Boiling points do not depend on the molar mass, instead it depends on the hydrogen bond. Methanol is an alcohol therefore it has hydrogen bonds, meaning that it will also obtain a high boiling point. Ethane is a gas therefore does not obtain hydrogen bonds which results in having a low boiling point.

I am going to investigate the enthalpy change of combustion for the alcohol homologous series. I will investigate how alcohols with increasing number of carbons affect the enthalpy change when an alcohol goes under combustion.

D. What are some practical applications of freezing point depression, boiling point elevation, and vapor pressure lowering?

The melting point usually increases when you go from the element sodium to silicon however then starts to decrease when it gets to argon. The boiling point will usually increase when going from sodium to aluminium but will then decrease to argon.

Alkenes are an unsaturated chemical compound containing at least one carbon-to-carbon double bond. The simple alkenes have only one double bond and no other functional groups. For example, (C=C). The boiling points of each alkene are very similar to that of the alkane with the same number of carbon atoms. In this case, the alkenes have a boiling point which is a small number of degrees lower than the alkane. Each alkene has 2 fewer electrons than the alkane with the same number of carbons. (Clark, J. 2003).

where a and b are both constants depending on the properties of oil and gas sample as well as the operation condition (pressure and temperature). Hayduk and and Das−Butler proposed different correlations for normal paraffin solute/solvent system and propane/heavy oil system, respectively.