The energies of reaction of XeF 6(c), XeF 4(c), and XeF 2(c) with PF 3(g) were measured in a bomb calorimeter. These results were combined with the enthalpy of fluorination of PF 3(g), which was redetermined to be −(151.98 ± 0.07) kcal th mol −1, to derive (at 298.15 K) ΔH f o(XeF 6, c, I) = −(80.82 ± 0.53) kcal th mol −1, ΔH f o(XeF 4, c) = −(63.84 ± 0.21) kcal th mol −1, and ΔH f o(XeF 2, c) = −(38.90 ± 0.21) kcal th mol −1. The enthalpies of formation of the solid xenon fluorides were combined with reported enthalpies of sublimation to derive (at 298.15 K) ΔH f o(XeF 6, g) = −(66.69 ± 0.61) kcal th mol −1, ΔH f o(XeF 4, g) = −(49.28 ± 0.22) kcal th mol −1, and ΔH f o(XeF 2, g) = −(25.58 ± 0.21) kcal th mol −1. The average bond dissociation enthalpies,〈 D o〉(XeF, 298.15 K), are (29.94 ± 0.16), (31.15 ± 0.13), and (31.62 ± 0.16) kcal th mol −1 in XeF 6(g), XeF 4(g), and XeF 2(g), respectively. The enthalpy of formation of PF 3(g) was determined to be −(228.8 ± 0.3) kcal th mol −1.