The enthalpies of formation of XeF6(c), XeF4(c), XeF2(c), and PF3(g) |
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Authors: | Gerald K. JohnsonJohn G. Malm Ward N. Hubbard |
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Affiliation: | Chemical Engineering and Chemistry Divisions, Argonne National Laboratory, Argonne, Illinois 60439, USA |
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Abstract: | The energies of reaction of XeF6(c), XeF4(c), and XeF2(c) with PF3(g) were measured in a bomb calorimeter. These results were combined with the enthalpy of fluorination of PF3(g), which was redetermined to be −(151.98 ± 0.07) kcalth mol−1, to derive (at 298.15 K) ΔHfo(XeF6, c, I) = −(80.82 ± 0.53) kcalth mol−1, ΔHfo(XeF4, c) = −(63.84 ± 0.21) kcalth mol−1, and ΔHfo(XeF2, c) = −(38.90 ± 0.21) kcalth mol−1. The enthalpies of formation of the solid xenon fluorides were combined with reported enthalpies of sublimation to derive (at 298.15 K) ΔHfo(XeF6, g) = −(66.69 ± 0.61) kcalth mol−1, ΔHfo(XeF4, g) = −(49.28 ± 0.22) kcalth mol−1, and ΔHfo(XeF2, g) = −(25.58 ± 0.21) kcalth mol−1. The average bond dissociation enthalpies,〈Do〉(XeF, 298.15 K), are (29.94 ± 0.16), (31.15 ± 0.13), and (31.62 ± 0.16) kcalth mol−1 in XeF6(g), XeF4(g), and XeF2(g), respectively. The enthalpy of formation of PF3(g) was determined to be −(228.8 ± 0.3) kcalth mol−1. |
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