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Toggle the table of contents. Ethylene (data page) ... Vapor pressure of liquid. P in mmHg: 1: 10: 40: 100: 400: 760: ... log 10 of ethylene vapor pressure.
Valid results within the quoted ranges from most equations are included in the table for comparison. A conversion factor is included into the original first coefficients of the equations to provide the pressure in pascals (CR2: 5.006, SMI: -0.875).
This is illustrated in the vapor pressure chart (see right) that shows graphs of the vapor pressures versus temperatures for a variety of liquids. [7] At the normal boiling point of a liquid, the vapor pressure is equal to the standard atmospheric pressure defined as 1 atmosphere, [1] 760 Torr, 101.325 kPa, or 14.69595 psi.
Table data obtained from CRC Handbook of Chemistry and Physics, 44th ed. Temperature dependence of ethylene glycol vapor pressure. Uses formula ...
This causes severe problems for computational techniques which rely on a continuous vapor pressure curve. Two solutions are possible: The first approach uses a single Antoine parameter set over a larger temperature range and accepts the increased deviation between calculated and real vapor pressures.
On a pressure–temperature (P–T) diagram, for any phase change the line separating the two phases is known as the coexistence curve.The Clapeyron relation [6] [7] gives the slope of the tangents to this curve.
A log-lin vapor pressure chart for various liquids. The higher the vapor pressure of a liquid at a given temperature, the lower the normal boiling point (i.e., the boiling point at atmospheric pressure) of the liquid. The vapor pressure chart to the right has graphs of the vapor pressures versus temperatures for a variety of liquids. [10]
The equation of state of Soave is defined as follows: = (+). The original α-function has been replaced by the function of Mathias–Copeman: [2] = [+ + + ()].The parameters of the Mathias–Copeman equation are fitted to experimental vapor-pressure data of pure components and provide a better description of the vapor pressure than the original relation.