Rank from highest to lowest vapor pressure.CH3CH2CH2CH2OH,CH4,CH3CHCH2CH3CH3,CH3CH2CH2CH2CH3

4.5 liters of a solution that is 5.0% NaCl by mass (the density of the solution is 1.08g/ml)

stupid question

To rank the substances from highest to lowest vapor pressure, we need to consider their molecular structure and intermolecular forces. The vapor pressure is primarily determined by the strength of intermolecular forces between molecules. Higher vapor pressure indicates weaker intermolecular forces.

1. CH4 (Methane):
Methane has the lowest boiling point and the weakest intermolecular forces among the compounds listed. It consists of only carbon and hydrogen atoms, which are nonpolar. Since methane molecules do not have polar bonds, the only intermolecular force acting on them is van der Waals forces, specifically London dispersion forces. Hence, methane has the highest vapor pressure.

2. CH3CH2CH2CH2CH3 (Pentane):
Pentane is a hydrocarbon with five carbon atoms, and it is a linear chain molecule. It has slightly stronger intermolecular forces compared to methane due to its larger size. Pentane molecules also experience London dispersion forces, but the increased number of electrons and surface area in pentane compared to methane molecules leads to stronger forces. Therefore, pentane has the second highest vapor pressure.

3. CH3CHCH2CH3CH3 (2-Methylbutane):
2-Methylbutane, also known as isopentane, is an isomer of pentane. The presence of the methyl group gives it a branched structure. The branching reduces the surface area available for intermolecular interactions, resulting in weaker intermolecular forces. Thus, isopentane has a lower vapor pressure than pentane but higher vapor pressure than 1-butanol.

4. CH3CH2CH2CH2OH (1-Butanol):
1-Butanol is an alcohol with a linear chain of four carbon atoms and a hydroxyl group (-OH). The presence of the hydroxyl group introduces stronger intermolecular forces, including hydrogen bonding. Hydrogen bonding is stronger than London dispersion forces and is responsible for the higher boiling point and lower vapor pressure compared to hydrocarbons. Therefore, 1-butanol has the lowest vapor pressure among the listed compounds.

In summary, the ranking from the highest to lowest vapor pressure is:
CH4 > CH3CH2CH2CH2CH3 > CH3CHCH2CH3CH3 > CH3CH2CH2CH2OH