Which of the following molecules would be expected to have the lowest boiling point?

Question

1) CH4
2) C12H26
3) C16H34
4) C2H6
5) C8H18

Answer 1

Hear is a simple concept:

Boiling and melting points depend on the strength of the intermolecular forces between the molecules. The stronger the intermolecular forces, the higher the melting and boiling points because more energy is required to break the bonds and cause the phase.

All of the above you listed are called hydrocarbons. Then the question to ask is, what sort of intermolecular forces can be found between hydrocarbons, answer: only the weak london (dispersion) forces cause by temporarily induced dipole moments, which is directly related to the number of electron that can be polarized which increases as the molecular weight increases because the number of electrons also increase. The strength of London forces depends on two facors
1. Molecular Weight: larger compounds, higher molecular weight= more electrons
2. Shape: more linear compounds have a higher melting/boiling point then ones that are more spherically because linearity makes more electron available, the more compact forms have less polarizable elctron available and thus lower melting/boiling points

Answer: 1<4<5<2<3

Well hope that helps

Answer 2

1) CH4 lowest molecular weight

Answer 3

CH4. since they are all just H's and C's, just choose the shortest chain. btw, CH4's a gas.

Answer 4

CH4
To answer at this question we have to look at the molar masses.
CH4 has the lowest molar mass so it has the lowest boiling point

Answer 5

CH4 less H molecules so less forces working on it

Answer 6

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Answer 7

CH4 at -162C???

Answer 8

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