Heats, equilibrium constants, and free energies of formation of the monoolefin hydrocarbons

Abstract

For ethylene, propylene, each of the four butenes, six pentenes, and 17 hexenes, and for the higher normal l-alkenes, values are presented for the following thermodynamic properties to 1,000° or 1,500 0 K: The heat of formation from the elements, D.Hr ; the free energy of formation from the elements, D.Fr; and the logarithm of the equilibrium constant of formation from the elements, 10gIO J(j. For each of the 6 pentenes and 17 hexenes, values are a lso given to 1,000° or 1,500 0 K, for the following properties: The heat-content function, (HO -Ho O)/T; the free-energy function, (FO -HoO)/T; the entropy, S o; the heat content, HO -Hoo; and the heat capacity, eva.Equilibrium constants and concentrations are given in tabular and graphical form for the isomerization of the 4 butenes, 6 pentencs, a nd 17 hexenes, as a function of the temperature to 1,000 0 or 1,500 0 K. Equilibrium constants a re also given in tabula r ancl graphical form for some reactions of hydrogenation, dimerization, ancl alkylation.

Heat content, free-energy function, entropy, and heat capacity of ethylene, propylene, and the four butenes to 1,500 degrees-K

“…This comparison is presented in reference [17]. This value is reasonable in magnitude on pbysical grounds and in addition gives good agreement with the abovementioned experimental equilibrium data over a wide temperature range.…”

Heats, equilibrium constants, and free energies of formation of the alkylbenzenes

“…This plot may be compared with corresponding plots for the normal paraffins [13], the normall-alkynes [15], and thenormall-alkenes [24]. bt;.I-ifo re presents the increment in heat content for the reaction of forming the given compound in the gaseous state from the elements carbon (solid, graphite) and hydrogen (gaseous), with all the reactants and products in their appropriate standard reference states at the temperature indicated.…”

“…In figures 2 and 3 are plotted, as a function of the temperature, the values of IlFo/T given in tables 25 and 26 for the isomerization of the C8HlO and the C9H12 alkybenzenes, These plots may be compared with corresponding plots for the paraffins [21,22], the ace~ylenes [15], and the monoolefins [24]. From these charts, one may see at a glance, for any temperature in the given range, and within the limits of uncertainty of the calculations, which of the isomers is thermodynamically most stable (lowest value of IlFO / T) and which is the least stable (highest vuIue of IlFo/T).…”

The effect of flow maldistribution on conversion in a catalytic packed‐bed reactor. Part II. Experimental studies

“…(1) At 200°C, the temperature used for the present study, the equilibrium constant for this simplified scheme is about 8 (Kilpatrick et al, 1946). An apparent first-order rate constant was computed on the basis that the isomerization of 1-butene can be treated as an irreversible, firstorder reaction.…”