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Answered 2012-04-02 22:00:22

Because octane has more carbons, and the more carbons you have the higher the melting point. also octane is a gas that is very close to nonane (which is the first liquid) and that would mean it has a larger boiling point that methane (which is a gas that is the first one CH4). that is why octane has a larger boiling point that methane. Also, you can also figure it out the boiling points of each and look at the differences.

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Octane. The boiling point of straight-chain alkanes increases within its homologous series (meaning methane has a lower boiling point than ethane, which is lower than propane, etc). Hexane : Boiling Point 69 o C Octane : Boiling Point 125.5 o C


Octane has a higher boiling point than pentane because octane has a larger number of carbon atoms than propane


Boiling point of ethanol is higher than its isomer methane due to the presence of hydrogen bond in ethanol


Yes, Boiling point of ammonia, NH3: - 33,34 0C Boiling poit of methane, CH4: - 161,6 0C


The boiling point of octane is 125 0C.


Octane has more carbon atoms than pentane.


Metahne does not have a higher boiling point than methane. Fluoromethane, CH3F, has a boiling point of 195K, -78.2C, methane, CH4, has a boiling point of 109K approx -164 C. I make that fluoromethane has a higher temeprature boiling point than methane. This is what you would expect, London dispersion forces will be greater in CH3F as it has more electrons than CH4. CH3F is polar and there will be dipole dipole interactions which will not be present in CH4.


The normal boiling point for n-octane is 398.7 +/- 0.5 Kelvin


The boiling point of Methane is 83F


Octane is a liquid, not a gas. Its boiling point is considerably higher than that of water.


Water has stronger hydrogen bonds than Methane. More energy is required to break them, hence the difference in boiling point


The intermolecular forces in neon are weaker than those in methane


The boiling point of methane is NOT higher, but lower than of propane (about 119 degrees lower), as can be seen from the table below:Methane: Bp. −161 °C, 112 KPropane: Bp. -42.1, 231.1 K


Both compounds are straight chained alkanes. (General formula CnH2n-2) The general rule is the bigger the molecule in a group of similar compounds the higher boiling point it has. Methane is C1, butane is C4 - much bigger.


The boiling point of methane is -161 degrees Celsius or -278.5 degrees Fahrenheit


Methane is gas derived from liquid methane.


This is because methane is more stable or happier than ethane. It has a shorter carbon chain and less branching making it the harder one to boil.


The boiling point is cca. 83 oC.


The dispersion forces in the non polar octane molecules are stronger thand the dispersion forces and hydrogen bonding in water.


The boiling point of water is 100 0C at 760 mm col. Hg. The boiling point of methane is -164 0C.


Indeed it can. At the boiling point liquid methane is in equilbrium with gaseous methane, so both exist simultaneously.


That depends on what kind of octane you are referring to. n-octane has much different melting and boiling points than iso-octane. Octane has 18 structural isomers. Assuming the person asking the question is interested in either n-octane or iso-octane:n-octanemelting point: −57 °C, 216 K, -71 °Fboiling point: 125.52 °C, 399 K, 258 °Fiso-octane (also known as 2,2,4-Trimethylpentaneor isooctane)melting point: -107.38 °C, 166 K, -161 °Fboiling point: 99.3 °C, 372 K, 211 °F


At low pressure the boiling point is lowered and inverse.


Methane has a boiling point of −161 °C at a pressure of one atmosphere. For the source and more detailed information concerning this subject, click on the related links section indicated below.


Ammonia has a higher boiling point then methane because it is a polar molecule, meaning that one part of the molecule has a partial positive charge while the other has a partial negative charge. As a result, ammonia molecules are attracted to each other in a similar manner as magnets are. Methane, dues to its symmetry, is nonpolar.



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