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2 CHAPTER1. INTRODUCTION Table 1.1: Some important uses for chlorine gas[4]. Product Polyvinyl chloride (PVC) and several other plastics TiO2 Highly pure Si for solar cells and electronics Highly pure HCl Pharmaceuticals Chlorine use Raw material In precursor TiClx In precursor SiCl4 As reactant Final product, reactants or intermediates oxidized to form chlorine gas according to 2Cl− → Cl2 + 2e− (1.1) and the cathode, where hydrogen gas is evolved according to 2H2O + 2e− → H2 + 2OH−. (1.2) The anode used in both processes is the so-called Dimensionally Stable Anode (DSA), with is Ti coated with a mixed rutile oxide of ca 30% RuO2 (possibly together with other dopants) and 70% TiO2. If a divider is used, the pH at the anode side is kept low and chlorine gas is liberated. Without a divider the pH in the electrolyte can reach close to neutral values, allowing sodium chlorate to form in the following reactions, starting with hydrolysis of formed chlorine Cl2 +H2O H+ +HOCl+Cl−, HOCl + H2O OCl− + H3O+, followed by chemical formation of chlorate, 2HOCl + OCl− → ClO−3 + 2H+ + 2Cl− . (1.3) (1.4) (1.5) The detailed mechanism of reaction 1.5 has still not been determined[1]. To maxi- mize the chemical formation of sodium chlorate, chlorate plants have low-volume electrolysis cells connected to larger reactors where the chemical conversion can be maximized. In the divided cell, highly concentrated sodium hydroxide (alkali) can be extracted from the cathode side, explaining why this process is known as the chlor-alkali process. The overall reaction occurring in the divided (chlor-alkali) cell is 2NaCl + 2H2O → Cl2 + H2 + 2NaOH, (1.6)PDF Image | Studies of Electrode Processes in Industrial Electrosynthesis
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