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- W1968474078 abstract "The gas phase equilibria in the reaction CF3CH2Br+I2=CF3CH2I+IBr have been studied over the temperature range 614–726 K. A third law treatment of the data gave ΔH°itr (298 K)=6.6±0.5 kcal mole−1. This result led to Δ°itf(CF3CH2Br, g, 298)= −166.0± 0.5 kcal mole−1 and DH° (CF3CH2Br)=69.2±1 kcal mole−1. These results were combined with previous data to obtain the enthalpies of reaction for the series. in which X=H, I, and Br. It was found that the enthalpies of reaction became progressively less negative as the electronegativity of the substituent, X, increased. These experimental enthalpy changes are shown to be in excellent agreement with the net change in electrostatic interaction energy which was calculated assuming that the CF3 and CH2X groups in the reactant and product molecules were polarizable dipoles. The good agreement supports the hypothesis that polarity does play an important role in gas phase thermochemistry." @default.
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- W1968474078 date "1980-12-01" @default.
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- W1968474078 title "The thermochemistry of the gas phase reaction: CF3CH2Br+I2=CF3CH2I+IBr. Polarity effects in thermochemistry" @default.
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- W1968474078 doi "https://doi.org/10.1016/0040-6031(80)85096-9" @default.
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