Date of Award
Master of Science in Chemical Engineering - (M.S.)
Saul I. Kreps
William H. Snyder
The esterification of oleic acid with oleyl alcohol was studied. A literature search showed that the chemical kinetics for this reaction had not been studied previously.
In the temperature range of 150 to 200°C. and up to a conversion of about 85 per cent, the esterification was found to be a second order reaction when the water of reaction was removed from the system by simple distillation.
Para-toluenesulfonic acid is an effective catalyst for this system, and the observed specific rate constant is a linear function of the catalyst concentration.
The effect of temperature on the specific rate constant for the uncatalyzed reaction is given by the equation
In k1 = 6.88 x 103/T + 10.5
where k1 is in units of l./(g.-mole) (min.) and T is in degrees Kelvin. For the catalyzed reaction, the equation is
ln k2 = -4.90 x 103/T + 14.7
Energies of activation for the uncatalyzed and catalyzed reactions were graphically evaluated to be 13,650 calories per gram-mole and 9730 calories per gram-mole, respectively.
An empirical rate equation was derived for this system. Using the values of the frequency factors and energies of activation determined from the experimental data, the rate equation becomes
r = (2.35e-6.88x10^3/T +2.69e-4.90x10^3/T CC) CA,CB
where r = reaction rate, (g.-moles)/(l.) (min.)
CA,CB,CC = concentrations of oleic acid, oleyl alcohol, and catalyst, respectively, m./l.
T = absolute temperature, °K.
Persurance, Robert, "Esterification of oleic acid with oleyl alcohol" (1964). Theses. 2136.