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Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
Hydrogen Peroxide Manufacturing Process
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Hydrogen Peroxide Manufacturing Process

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Sachin Hadavale, Shital Jagtap and Mayur Zunjarrao

Sachin Hadavale, Shital Jagtap and Mayur Zunjarrao

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  • Hello ! I'm doing a project about hydrogen peroxide and i would like to know where did you find the heat capacity of 2-ethyl-antraquinone? thanks!
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  • 1. SHITAL JAGTAP SACHIN HADAVALE MAYUR ZUNJARRAO GUIDE:- PROF. A K BANDSODE
  • 2. INTRODUCTION
    • Hydrogen peroxide (H 2 O 2 ) is the simplest peroxide
    • Hydrogen peroxide is a clear liquid, slightly more viscous than water.
  • 3. HISTORY
    • Hydrogen peroxide was first manufactured in 1818 by Louis Jacques Thenard by reacting barium peroxide with nitric acid. An improved version of this process used hydrochloric acid, followed by sulfuric acid to precipitate the barium sulfate byproduct. Thenard's process was used from the end of the 19th century until the middle of the 20th century.
  • 4. LITERATURE SURVEY Susana Silva Martínez 15 October 2007 Hydrogen Peroxide production by oxidation of cyanide 4 Yuji Ando, Tadayoshi Tanaka 13 October 2004 Hydrogen Peroxide production by water electrolysis 3 Qunlai Chen May 2008 Anthraquinone process for the production of hydrogen peroxide 2 Tomoya Inoue, Yusuke Tanaka, Koichi Sato 1 Jan 2010 Direct production of hydrogen peroxide from oxygen and hydrogen applying membrane-permeation mechanism 1 Auther Date Process No
  • 5. Yury Voloshin, Adeniyi Lawal 16 January 2010 Hydrogen peroxide formation by direct combination of H 2 and O 2 in a micro reactor 5 Albert F. Carley, Jennifer Edwards 30 May 2006 Direct synthesis of hydrogen peroxide from H 2 and O 2 using zeolite supported Au catalysts 10 Ji Chul Jung, Sunyoung Park, 25 July 2009 Direct synthesis of hydrogen peroxide from hydrogen and oxygen over palladium catalyst 9 David J. Kieber 6 June 2000 Photochemical production of hydrogen peroxide in Antarctic Waters 8 K. Kusakabe, Maehara 4 April 2008 Catalytic synthesis of hydrogen peroxide in micro reactors 7 Mao Mao, Xue-You Duan, 1 January 2011 Hydrogen peroxide synthesis by direct photo reduction of 2-ethylanthraquinone 6
  • 6. PHYSICAL PROPERTIES -4.007 kJ/g Std enthalpy of formation Δ H f 298 k 6.2 pH 2.619 J/g K (liquid) Specific heat capacity 1.245 cP (20 °C ) Viscosity 1.34 Refractive index Soluble in ether Solubility 150 °C, 423 K, 302 °F Boiling point -0.43 °C, 273 K, 31 °F Melting point 1.450 g/cm 3 (20 °C) Density light blue to colourless Appearance 34.0147 g/mol Molar mass H 2 O 2 Molecular formula
  • 7. USES
    • Pulp and paper
    • Mining
    • Textile bleaching
    • Controlling fungus on fish and eggs
    • Waste water treatment
    • Healing wounds
    • Explosive
  • 8. MARKET SURVEY
  • 9.  
  • 10. IMPORT AND EXPORT EXPORT IMPORT 105000 Kenya 600277 Taiwan 259830 Sri Lanka 887374 Turkey 400000 Maldives 1121118 Rep. Of Korea 1156390 Bangladesh 2268897 Indonesia 1167115 Untd. Arab Emts. 5155989 China QUANTITY (Kg) COUNTRY QUANTITY (Kg) COUNTRY
  • 11. MANUFACTURING PROCESSES
    • Wet Chemical Process
    • Electrochemical Process
    • Autoxidation Process
  • 12. The Wet Chemical Process
    • Disadvantages
    • High capital cost
    • Low hydrogen peroxide content
    • Unsatisfactory stability
  • 13. Electrochemical process
    • Advantages
    • More conc. H 2 o 2
    • High purity H 2 o 2
    • Disadvantages
    • High capital investment
    • High electricity consumption
  • 14. AUTOXIDATION PROCESS
    • Hydrogen peroxide is manufactured almost exclusively by the autoxidation (AO) process. The process is based on a reduction of anthraquinone, followed by oxidation resulting in the formation of H2O2.
    • Hydrogen peroxide is separated from water with extraction and is concentrated to produce grades at standard commercial strengths of 35 - 65%.
  • 15.
    • Reactions Of Autoxidation Process
    • Hydrogenation
    • Oxidation
  • 16.  
  • 17. Process Selection
    • Higher industrial applicability
    • Greater purity of H 2 O 2
    • Ease of operation
    • Easy availability of raw material
    • Lesser cost of raw material
    • Recycle of raw material
    • Lesser power requirement
  • 18. THERMODYNAMIC FEASIBILITY 26.1 0 Oxygen O 2 28.65 0 Hydrogen H 2 70.79 -45.16 Hydrogen Peroxide H 2 O 2 489.4 -132.46 2-Ethyl Hydroquinone C 16 H 14 O 2 453.4 -111.021 2-Ethyl Anthraquinone C 16 H 12 O 2 Heat Capacity (KJ/ Kmol °C) Heat Of Formation (KJ/mol) Components
  • 19. For Hydrogenation Reaction that is C 16 H 12 O 2 + H 2 ->C 16 H 14 O 2 Heat of Formation of above reaction at 298 K is Δ H f 298K = ΣΔ H f Products - ΣΔ H f Reactant = - 132.46 - ( - 111.021) = - 21.439 KJ/mol The specific heat is givaen as follows Δ C P = ΣΔ C P Products - ΣΔ C P Reactant = 489.4 - (453.4 + 28.65) =7.35 KJ/ Kmol °C The heat of reaction at working temp. Δ H R 313 K = Δ H f 298K = -21439 + (7.35) (40 - 25) = -21328 KJ/Kmol The entropy of Hydrogenation Reaction Δ S R 313 K = Δ S R ° + At const temp Δ S R °= 0 Δ S R 313 K = 7.35 ln (40/25) = 3.454 KJ/Kmol °C
  • 20. The Gibbs free energy Δ G 313 k = Δ H R 313 K - T Δ S R 313 K = -21328.75 - 40 X 3.54 =- 21446.93 KJ/Kmol (Less than zero) Consider second reaction taking place in oxidizer C 16 H 14 O 2 + O 2 ->C 16 H 12 O 2 + H 2 O 2 Δ H f 298K = ΣΔ H f Products - ΣΔ H f Reactant = ( - 111.021 - 45.16) - ( - 132.46 ) = -23.721 KJ/mol Δ C P = ΣΔ C P Products - ΣΔ C P Reactant = 453.4 + 70.79 - 489.4 - 26.1 = 8.69 KJ/ Kmol °C Δ H R 323 K = Δ H f 298K = -23721 + 8.69 ( 50 - 25 ) =-23503.75 KJ/Kmol Δ S R 323 K = Δ S R ° + = 0 + 8.69 ln ( 50/25 ) = 6.023 KJ/ Kmol °C
  • 21.
    • The Gibbs free energy
    • Δ G 323 k = Δ H R 323 K - T Δ S R 323 K
    • = - 23503.75 - 50 X 6.023
    • = -23804.922 KJ/Kmol (Less than zero)
    • From the above values it can be seen that the values of Gibbs Free energy at respective working temp. is less than zero, which is the ideal case scenario. Thus both the reactions are feasible and thereby the selected process is also feasible.
  • 22. Bibliography
    • Perry's handbook of chemical engineering 8th edition
    • Ullmans Encyclopedia
    • Wikipedia
    • Sciencedirect.com
    • www.cheresources.com
  • 23. THANK YOU

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