Please simulate the reactors given in the figure below. The reversible reaction, which takes place at 70Ā°C and 1 atm, is given as:
Ethanol + Acetic Acid $\rightleftharpoons$ Ethyl Acetate + Water
The reaction is first order with respect to each of the reactants (overall second order). The reaction rate is expressed by Arrhenius Equation ($k = k_0 e^{-E/RT}$). For the forward reaction, the preexponential factor is $1.9 \times 10^8$ m$^3$/kmol-s and the activation energy is $5.95 \times 10^7$ J/kmol. For the backward reaction, the preexponential factor is $5.0 \times 10^7$ m$^3$/kmol-s and the activation energy is $5.95 \times 10^7$ J/kmol. The reaction takes place in the liquid phase, and the components are in mole basis. Please consider mixed phase as the valid phase for each reactor. Simulate your process by using NRTL as the thermodynamic K value model and Latent Heat as the enthalpy model.
a. What is the flow rate of ethyl acetate exiting each reactor in kmol/h?
b. What is the conversion of ethanol for each reactor?
c. In the PFR reactor, for each component, draw the composition profile (chose "moles" as the composition option) as a function of reactor volume.
Feed:
Temperature: 70Ā°C, Pressure: 1 atm
Water: 8.892 kmol/h
Ethanol: 186.59 kmol/h
Acetic Acid: 192.6 kmol/h
Stoichiometric Reactor
Ethanol: 70% conversion
Gibbs Reactor
PFR; L = 2 m, D = 0.3 m
CSTR; V = 0.14 m$^3$
Equilibrium Reactor
Ethanol: 70% conversion
For PFR and CSTR, in "More Specifications" section, select the following:
- Activation Energy: J
- Molar flow: K-moles
- Volume: Cubic meters
- Time: Seconds