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Butane (/ ˈ b juː t eɪ n /) is an alkane with the formula C 4 H 10. Butane exists as two isomers, n-butane with connectivity CH 3 CH 2 CH 2 CH 3 and iso-butane with the formula (CH 3) 3 CH. Both isomers are highly flammable, colorless, easily liquefied gases that quickly vaporize at room temperature and pressure.
The attractive force draws molecules closer together and gives a real gas a tendency to occupy a smaller volume than an ideal gas. Which interaction is more important depends on temperature and pressure (see compressibility factor). In a gas, the distances between molecules are generally large, so intermolecular forces have only a small effect.
Butane, or n-butane; Isobutane, also known as methylpropane or 2-methylpropane This page was last edited on 22 December 2022, at 18:58 ...
Alkanes experience intermolecular van der Waals forces. The cumulative effects of these intermolecular forces give rise to greater boiling points of alkanes. [18] Two factors influence the strength of the van der Waals forces: the number of electrons surrounding the molecule, which increases with the alkane's molecular weight
n-Butane: Table data obtained from CRC Handbook of Chemistry and Physics 44th ed. Vapor pressure of n-butane. From formula: ...
The ideal gas model tends to fail at lower temperatures or higher pressures, when intermolecular forces and molecular size becomes important. It also fails for most heavy gases, such as many refrigerants, [2] and for gases with strong intermolecular forces, notably water vapor. At high pressures, the volume of a real gas is often considerably ...
The example below is looking down the C2 and C3 bond. Below is the sawhorse and Newman representation of butane in an eclipsed conformation with the two CH 3 groups (C1 and C4) at a 0-degree angle from one another (left). If the front is rotated 60° clockwise, the butane molecule is now in a staggered conformation (right).
Deviations of the compressibility factor, Z, from unity are due to attractive and repulsive intermolecular forces. At a given temperature and pressure, repulsive forces tend to make the volume larger than for an ideal gas; when these forces dominate Z is greater than unity. When attractive forces dominate, Z is less than unity.