The kinetics of the chlorination equilibrium of methanol, Ch2OH + HCl ⇔ CH3OH + Cl (1, -1), have been studied using the fast flow technique with Laser Magnetic Resonance and Electron Paramagnetic Resonance detection. The rate constants of the forward and reverse reactions were found to be k1 = (2.3±0.9) · 1011 exp [-(20.9 ± 2.9) kJ · mol-1/RT] cm3/mol · s in the temperature range 500 K ≤ T ≤ 812 K and k-1 = (3.7 ± 0.4) · 1013 cm3/mol · s at room temperature. These kinetic results were utilized in third law and second law procedures to obtain the value of the heat of formation of the hydroxymethyl radical. The entropy of CH2OH, SF,2980(CH2OH) = (254 ± 4) J/mol · K, and the activation energy of reaction (-1), E-1 = (0 + 4) kJ/mol, which are required for the calculations, were selected by critical assessment of the available literature data. The average of the third law and second law determinations provided ΔfH2980(CH2OH) = - (9 ± 6) kJ/mol. This value is higher by 17 kJ/mol than the heat of formation value in common use and implies a stronger C-H bond energy in methanol, D298(H-CH2OH) = 410 kJ/mol. These new thermochemical quantities are in excellent agreement with the very recent recommendations of Sectula and Gutman [J. Phys. Chem. 96, 5401 (1992)] and have important implications for modeling studies of complex chemical systems such as the combustion of methanol.
|Number of pages||7|
|Journal||Berichte der Bunsengesellschaft/Physical Chemistry Chemical Physics|
|Publication status||Published - 1993|
ASJC Scopus subject areas
- Chemical Engineering(all)