This is a Reaction/Chemical Reactor Engineering question. Please provide full, clear working for the answer with legible handwriting and explanation, if needed.

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It is desired to carry out the gaseous reaction AB in an existing tubular reactor consisting of 50 parallel tubes 12m long with a 25cm inside diameter. Lab scale experiments have given the reaction rate constant for the first-order reaction as 0.00152s1 at 400K and 0.0740s1 at 550K. The system is operating at 100kPa with pure A being fed into the reactor at 200kg/h. A has a molecular weight of 33g/mol. You may assume ideal gas behavior. Apply Arrhenius equation to calculate the activation energy of the specified reaction. Then determine the conversion when the reactor operates isothermally at T=450K. Select one: a. E=47.4kJ/mol,X=97% b. E=94.8kJ/mol,X=99% c. E=47.4kJ/mol,X=90% d. E=38.6kJ/mol,X=92% e. E=94.8kJ/mol,X=97% f.E=52.1kJ/mol,X=92%