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Heat capacity, c p: 118.4 J/(mol K) at 0 °C Liquid properties Std enthalpy change of formation, Δ f H o liquid +48.7 kJ/mol Standard molar entropy, S o liquid: 173.26 J/(mol K) Enthalpy of combustion, Δ c H o –3273 kJ/mol Heat capacity, [2] c p: 134.8 J/(mol K) Gas properties Std enthalpy change of formation, Δ f H o gas +82.93 kJ/mol ...
Heat capacity, c p? J/(mol K) Liquid properties Std enthalpy change of formation, Δ f H o liquid: −118.910 kJ/mol Standard molar entropy, S o liquid: 171.0 J/(mol K) Heat capacity, c p: 98.36 J/(mol K) Gas properties Std enthalpy change of formation, Δ f H o gas: −104.7 kJ/mol Standard molar entropy, S o gas: 269.91 J/(mol K) Enthalpy of ...
The enthalpy of combustion of propane gas where products do not return to standard state, for example where the hot gases including water vapor exit a chimney, (known as lower heating value) is −2043.455 kJ/mol. [29] The lower heat value is the amount of heat available from burning the substance where the combustion products are vented to the ...
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.
J.A. Dean (ed.), Lange's Handbook of Chemistry (15th Edition), McGraw-Hill, 1999; Section 6, Thermodynamic Properties; Table 6.4, Heats of Fusion, Vaporization, and Sublimation and Specific Heat at Various Temperatures of the Elements and Inorganic Compounds
Reid vapor pressure (RVP) is a common measure of the volatility of gasoline and other petroleum products. [1] It is defined as the absolute vapor pressure exerted by the vapor of the liquid and any dissolved gases/moisture at 37.8 °C (100 °F) as determined by the test method ASTM-D-323, which was first developed in 1930 [2] and has been revised several times (the latest version is ASTM D323 ...
Raoult's law (/ ˈ r ɑː uː l z / law) is a relation of physical chemistry, with implications in thermodynamics.Proposed by French chemist François-Marie Raoult in 1887, [1] [2] it states that the partial pressure of each component of an ideal mixture of liquids is equal to the vapor pressure of the pure component (liquid or solid) multiplied by its mole fraction in the mixture.
The vapor pressure of a liquid, which varies with its temperature, is a measure of how much the vapor of the liquid tends to concentrate in the surrounding atmosphere as the liquid evaporates. [30] Vapor pressure is a major determinant of the flash point and flame point, with higher vapor pressures leading to lower flash points and higher ...