KINETICS STUDY OF FISCHER-TROPSCH SYNTHESIS WITH COBALT BASED CATALYST
<p align="justify">Until now, the need for gas oil is still fulfilled mostly by crude oil. Crude oil has been known that only left with limited deposits and not renewable, sooner or later crude oil reserves will be depleted. The fact that Indonesia has massive coal reserve, has an ab...
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| Format: | Final Project |
| Language: | Indonesia |
| Online Access: | https://digilib.itb.ac.id/gdl/view/30893 |
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| Institution: | Institut Teknologi Bandung |
| Language: | Indonesia |
| Summary: | <p align="justify">Until now, the need for gas oil is still fulfilled mostly by crude oil. Crude oil has been known that only left with limited deposits and not renewable, sooner or later crude oil reserves will be depleted. The fact that Indonesia has massive coal reserve, has an abundant natural gas resource, and a lot of biomass waste, these are the alternative energy sources should be developed in Indonesia. The development of coal conversion technology, natural gas, and biomass into liquid fuels is a major concern for energy saving programs. This alternative energy source can be regulated into synthesis gas, which is a mixture of hydrogen gas (H2) and carbon monoxide (CO) gas. With Fischer-Tropsch synthesis, this synthesis gas can transform into liquid phase hydrocarbon. <br />
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This study aims to determine the Fischer Tropsch kinetics model with Co/γ-Al2O3/K catalyst (developed at Chemical Reaction Engineering Laboratory and Catalysis ITB). This research consisted of kinetics data collection and determination of kinetics equation of Fischer-Tropsch reaction. The reaction takes place in a fixed bed continuous reactor with an operating pressure of 20 bar. The temperature variation is around 230-250℃ and GHSV variation is around 25-40 ml/minute. The product of the reaction is then analyzed by gas chromatographic analysis. The results are used to determine reaction conversion and selectivity. The kinetics equation for 230240℃ uses Power Law model and can be determined by the ode or Runge-Kutta function in the MATLAB®. The kinetics equation of the reaction obtained follows the -1,54 towards CO order and 0,79 towards H2 order. Based on the experiment, it is found that the has an activation energy of 19306 J/mol and Arrhenius value of 10898 Bar1,75.h-1. However, for the temperature 250℃ resulting a different equation. <p align="justify"> <br />
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