Carbon-13 Kinetic Isotope Effects in the Decarbonylation Of Liquid Formic Acid in Water Solution

Abstract

Carbon-13 kinetic isotope effects (¹³C KIEs) in the decarbonylation of formic acid diluted with water 1:1 (V:V) has been studied in the 130–181°C temperature interval in sealed vacuum all glass reactions vessels. The experimental ¹³C KIEs are higher than the ¹³C KIEs values extrapolated from low 50–100°C temperature interval ¹³C KIEs observed in the decarbonylation of water free liquid formic acid but less than ¹³C KIEs expected theoretically assuming the complete carbon—oxygen (¹³C[sbnd]¹⁶O) bond rupture in the transition state. For instance the (k₁₂/k₁₃) KIE found in this study is 1.0375 at 170.2°C while the “full” ¹³C KIE is expected to be 1.0429 at this temperature. The ¹³C KIE extrapolated to 170.2°C from the low temperature data published earlier is 1.0299. - The Arrhenius activation energy for the decarbonylation of formic acid in 1:1 water solution E = 31.3 kcal/mol is by 6 kcal/mol higher than that which was obtained with 99,9% pure formic acid (E = 25,660 kcal/mol). The entropy of activation ΔS ^≠ increased from -21.4 e.u. (pure formic acid) to -15.3 e.u. in the decarbonylation of formic acid diluted with water 1:1. The increases of the enthalpy of activation, of the entropy of activation and partly of the carbon-13 kinetic isotope effect observed in the decarbonylation of formic acid in water solution have been rationalized by suggesting isotopic equilibria interfering the pure kinetic fractionation of ¹³C and intervention of the water molecules into the process of transfer of protons to the formic acid molecules lowering the absolute rate of their decomposition.