PDF Publication Title:
Text from PDF Page: 007
International Journal of Chemical Engineering and Analytical Science Vol. 2, No. 1, 2017, pp. 1-8 7 concentrated chloride medium being lost at the rate of 0.2-0.4 g per ton of chlorine [30]. Additionally, the electrochemical cell has a large gap between the electrodes (1.5 cm). This gap resulted in a significant ionic resistance and then should deeply affect the current efficient. 3.6.2. Current Efficiency for Cathodic Reaction Similarly to chlorine, the hydrogen current efficiency is determined from the ratio of the obtained values by the thermodynamic values calculated from Faraday’s law of electrolysis, equation (11). The obtained current efficiency was around 83%. This current efficiency depended from the current densities. The differences between the obtained hydrogen flow rate and the thermodynamic values should be related to hydrogen crossover through membrane to find side of the anodic compartment, combine with oxygen (from parasite reaction) and can form water [31]. The material of the electrode was also important and can contribute to reduce or increase the current efficiency. At the cathode where hydrogen is evolved, the design must permit rapid bubble release, otherwise the bubbles will contribute to additional IR (ohmic resistant) loss. In addition to the overpotential for the cathode reaction in chlor-alkali cell, is critical to the energy consumption. Similarly to the anode material, the use of the graphite cathode where the hydrogen overpotential was about 400 mV, potentially decreases the current efficiency was observed. Thus, catalytic coating such as nickel alloys or platinum will decrease this overpotential it further to 20 - 50 mV [9, 29]. For example, [32] obtained a hydrogen efficiency of 99% on platinum electrode for 120 mA cm-2 current density. These platinum cathodes were, however, expensive. Similarly, to the anolyte compartment, the electrochemical cell had a large gap between the electrodes and the membrane (0.75 cm). This gap originates a significant ionic resistance and then should deeply affect the current efficient. 4. Conclusion Membrane electrolyzer was performed to study the parameters of electrolysis for chlorine and hydrogen production. The electrodes used in this study were composed of graphite tube with an effective surface of 12.058 cm2. These electrodes were recycled from used batteries. To reduce the energy consumption, the optimum gap between electrode and membrane was 0.75 cm. Also, the cell performance of different number of electrode was evaluated. Results indicate that a larger electrode surface area was better for chlorine and hydrogen production. The operating parameters of electrolysis were optimized and they were: 320 g.L-1 NaCl (pH=2), 24% NaOH, T= 80°C, i= 41.4 A/dm2. Under these conditions, the current efficiency was 81% for chlorine and 83% for hydrogen production. The research described in this paper has enabled a better understanding of chlorine-hydrogen membrane process. Further study will focus on the optimization of the electrode parameters for maximization of chlorine and hydrogen current efficiency. References [1] O’Brien, Th. F.; Bommaraju, T. V.; Hine F., (2005). Handbook of Chlor-Alkali Technology. Springer US, LXXXVI, Hardcover ISBN: 978-0-306-48623-4. [2] Euro Chlor, (2011). Le chlore en perspective. Euro Chlor©: Avenue E Van Nieuwenhuyse 4, box 2 B-1160 Brussels- Belgium. [3] Saksono, N., Abqari, F., Bismo, S., Kartohardjono, S., (2013). Effect of Process Condition in Plasma Electrolysis of Chlor- alkali Production. International Journal of Chemical Engineering and Applications, vol. 4, No. 5, 266-270. [4] Siracusano, S., (2010). Development and characterization of catalysts for electrolytic hydrogen production and chlor-alkali electrolysis cells. Thesis, University of Rome. [5] European Commission, (2001). Integrated Pollution Prevention and Control, Reference Document on Best Available Techniques in the Chlor-Alkali Manufacturing industry. [6] Chen, R., (2010). Electrochemical Chlorine Evolution at Sol- Gel Derived Mixed Oxide Electrocatalyst Coatings. Dissertation, Saarlandes University. [7] Cardarelli, F., (2008). Materials Handbook: A concise Desktop Reference, 2nd Edition. Springer, London, New York, 540-590. [8] Hansen, H. A., Man, I. C., Studt, F., Abild-Pedersen, F., Bligaard, T., Rossmeisl J., (2010). Electrochemical chlorine evolution at rutile oxide (110) surface. Physical Chemistry Chemical physics, 12, 283-290. [9] Karlsson R. K. B., (2015). Theoretical and experimental studies of electrode and electrolyte processes in industrial electrosynthesis. Doctoral Thesis, KTH Royal Institute of Technology, Sweden. [10] Chandler, G. K., Genders, J. D., Pletcher, D., (1997). Electodes Based on Noble Metals. Platinum Metals Rev., 41, 2, 54-63. [11] Malpass, G. R. P., Neves, R. S., Motheo, A. J., (2006). A comparative study of commercial and laboratory-made Ti/Ru0.3Ti0.7O2 DSA@ electrodes: ‘‘In-situ’’ and ‘‘ex-situ’’ surface characterization and organic oxidation activity. Electrochim. Acta, 52, 936. [12] Euro Chlor, (2015). Chlorine Industry Review 2014-2015. Euro Chlor©: Avenue E Van Nieuwenhuyse 4, box 2 B-1160 Brussels-Belgium. [13] Ullberg, Ø., (2003). Modeling of advanced alkaline electrolyzers: a system simulation approach. International journal of hydrogen energy, 28, 21-33.PDF Image | Electrolysis Parameters for Chlorine and Hydrogen Production
PDF Search Title:
Electrolysis Parameters for Chlorine and Hydrogen ProductionOriginal File Name Searched:
70560032.pdfDIY PDF Search: Google It | Yahoo | Bing
Salgenx Redox Flow Battery Technology: Power up your energy storage game with Salgenx Salt Water Battery. With its advanced technology, the flow battery provides reliable, scalable, and sustainable energy storage for utility-scale projects. Upgrade to a Salgenx flow battery today and take control of your energy future.
CONTACT TEL: 608-238-6001 Email: greg@salgenx.com (Standard Web Page)