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Experimental study on kinetic characteristics of oil sludge gasification
Author(s) -
Chu Zhiwei,
Gong Zhiqiang,
Wang Zhenbo,
Zhang Haoteng,
Wu Jinhui,
Wang Ziyi,
Guo Yizhi,
Zhang Jianqiang,
Li Guoen,
Zhang Lei,
Wang Hongpeng
Publication year - 2021
Publication title -
asia‐pacific journal of chemical engineering
Language(s) - English
Resource type - Journals
SCImago Journal Rank - 0.348
H-Index - 35
eISSN - 1932-2143
pISSN - 1932-2135
DOI - 10.1002/apj.2616
Subject(s) - gibbs free energy , volatilisation , activation energy , enthalpy , chemistry , oil sludge , kinetic energy , thermal decomposition , chemical process of decomposition , pyrolysis , decomposition , charring , thermodynamics , analytical chemistry (journal) , environmental chemistry , organic chemistry , physics , quantum mechanics
Abstract Oil sludge (OS) is a typical dangerous waste in petroleum industry, which also contains abundant energy. The purpose of this study was to recover resources from OS gasification. To figure out the gasification process, a thermal analyzer was used to carry out OS gasification experiments under steam/nitrogen atmosphere with different heating rates. Results showed that the OS gasification reaction could be divided into five stages: free water volatilization, the escape of light components, the cracking of heavy components and steam reforming, the charring process and water gas shift (WGS) reactions, and inorganic mineral decomposition. The activation energy ( E ), pre‐exponential factor ( A ), enthalpy change (Δ H ), Gibbs free energy change (Δ G ), and entropy change (Δ S ) of three main reaction stages (Stages 2–4) were analyzed through kinetic and thermodynamic analysis. From Stage 2 to Stage 4, E , Δ H , and Δ S decreased from 118.80 kJ·mol −1 , 113.92 kJ·mol −1 , and −4.09 J·(K mol) −1 to 13.19 kJ·mol −1 , 5.92 kJ·mol −1 , and −234.06 J·(K mol) −1 , respectively. Nevertheless, Δ G increased from 116.01 to 210.04 kJ·mol −1 . From these parameters, it could be found that the decrease of E was beneficial to the reaction. However, the values of Δ G were always positive and the reaction could not happen spontaneously.