The liquid-phase irreversible reaction
A → B + C
is carried out in a CSTR. To learn the rate law, the volumetric flow rate, v0, (hence τ = V/v0) is varied and the effluent concentrations of species A are recorded as a function of the space time t. Pure A enters the reactor at a concentration of 2 mol/dm3. Steady-state conditions exist when the measurements are recorded.
Run | 1 | 2 | 3 | 4 | 5 |
τ (min) | 15 | 38 | 100 | 300 | 1200 |
CA (mol/dm3) | 1.5 | 1.25 | 1.0 | 0.75 | 0.5 |
(a) Determine the reaction order and specific reaction rate constant.
(b) If you were to repeat this experiment to determine the kinetics, what would you do differently? Would you run at a higher, lower, or the same temperature? If you were to take more data, where would you place the measurements (e.g., τ )?
(c) It is believed that the technician may have made a dilution factor-of-10 error in one of the concentration measurements. What do you think? How do your answers compare using regression (Polymath or other software) with those obtained by graphical methods?
Note: All measurements were taken at steady-state conditions.
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