1. F LORIDA S OLAR E NERGY C ENTER A Research Institute of the University of Central Florida Hydrogen Production via Photolytic Oxidation of Aqueous Sodium Sulfite Solutions Cunping Huang, Clovis A. Linkous, Olawale Adebiyi & Ali T-Raissi Hydrogen 2008 – Materials Innovations in an Emerging Hydrogen Economy Cocoa Beach, Florida, USA February 27, 2008

2. Background  SO 2 is a criteria air pollutant that can cause respiratory & other problems as an acid gas  SO 2 emissions occur both naturally (20%) & anthropogenically (80%)  Natural sources include: geothermal (e.g. volcanic), oceanic, vegetative & land emissions.

3. Anthropogenic Sources of SO 2 Emissions  Combustion of high-sulfur- containing fossil fuels  Sulfuric acid & ammonium sulfate plants  Power plants using coal, crude oil & crude oil-based fuel oil.

4. Major Global Anthropogenic Sources of SO 2 Emissions Emission SourceEmission (%) Electric utility69.7 Industrial fuel combustion13.6 Metal processing3.8 Transportation3.5 Others9.4 Source: Schnelle, K.B., and Brown, C.A., Control of So x, In Air Pollution Control Technology Handbook, ed. Kreith, F., CRC Press, Boca Raton, FL, 257, 2002

5. Generation of SO 2 in 500 MW coal fired power plants can produce huge amounts of SO 2 that can be used for the production of H 2 as well as fertilizers. Source: Pandey, R. A., et al, “Flue gas Desulfurization: Physicochemical and Biotechnological Approaches” Env. Sci. & Tech. 35:571-622., 2005. SO 2 is both a Pollutant & a Resource

6. Objectives  Develop an innovative process for utilizing SO 2 in flue gas for the production of hydrogen  Explore chemistry & chemical engineering aspects of SO 2 utilization  Investigate effects of reaction conditions on the hydrogen production rate.

7. Flue Gas Treatment and H 2 Production Conventional process: Absorption: SO 2 + NaOH = Na 2 SO 3 Oxidation: Na 2 SO 3 + O 2 = Na 2 SO 4 + H 2 O FSEC Approach: Absorption: SO 2 + NaOH = Na 2 SO 3 SO 2 + (NH 4 OH) = (NH 4 ) 2 SO 3 Photooxidation: Na 2 SO 3 + H 2 O + UV light ( or  E)= Na 2 SO 4 + H 2 (NH 4 ) 2 SO 3 + H 2 O + UV light (or  E) = (NH 4 ) 2 SO 4 +H 2

8. Experimental Setup for SO 2 Treatment

9. Exp. Setup for H 2 Production from Aqueous Na 2 SO 3 Solution

10. Hydrogen Production

11. I: HSO 3 - to SO 4 2- II: SO 3 2- to SO 4 2- III: S 2 O 6 2- to SO 4 2- Kinetics of H 2 Production via Photo-oxidation of Na 2 SO 3

12. Material Balance Ionic Species Initial (mmol) Final (mmol) Diff. (mmol) SO 3 2- 63.410.0063.41 SO 4 2- 2.4063.5961.19 Gas Produced Theoretical (mL) Exp. (mL) Diff. (mL) H2H2 15501390160

13. Effect of Solution pH on H 2 Production

14. Effect of Solution pH on H 2 Production (cont’d)

15. Concentration Effect on H 2 Production Rate (at pH = 9.70)

16. Concentration Effect on H 2 Production Rate (at pH = 7.55)

17. Summary At pH = 9.95, H 2 production rate increases with an increase in the concentration of the sulfite. At pH = 7.55, H 2 production rate is independent of the sulfite concentration.

18. Conclusions  A novel approach for utilizing SO 2 in flue gas for hydrogen production has been developed  Photolytic H 2 production from aqueous Na 2 SO 3 solutions is a clean and efficient process  Experimental data indicate that SO 3 2- can be fully converted into SO 4 2-  FSEC process requires no catalysts, reducing the process capital & operating costs.

19. Future Work  Investigate effects of other flue gases (e.g. NO x, CO 2 ) on the photolytic production of hydrogen  Investigate effects of metal catalysts in enhancing the photolytic hydrogen production from SO 2  Photoreactor design considerations  Process design & optimization.

20. Acknowledgment  National Aeronautics and Space Administration (NASA) - Glenn Research Center (GRC) under contract No. NAG3-2751.