(BAT) Reference Document for the Production of Chlor-alkali ...
(BAT) Reference Document for the Production of Chlor-alkali ... (BAT) Reference Document for the Production of Chlor-alkali ...
Chapter 2 The electrolyser is operated at a temperature of approximately 70 – 80 ºC. The brine normally enters the electrolysis cell at 60 – 70 °C. At this temperature, the conductivity of the brine solution and the fluidity of the mercury are higher compared to operation at ambient temperature. The temperature can be achieved by preheating the saturated brine with steam and is increased in the cell electrolyser by the Joule heating heat of resistance to approximately about 75 – 85 °C. The heat produced during electrolysis and amalgam decomposition requires the air of the cell room to be changed 10 – 25 times per hour, depending on the type of building [ 1, Ullmann's 2006 ], [ 17, Dutch Ministry 1998 ]. 2.2.3 Decomposition of the amalgam The amalgam is decomposed in horizontal decomposers, alongside or beneath the cell (Figure 2.4) or more often, since ca. 1960, in vertical decomposers (or denuders), at one end of the cell (Figure 2.5). Industrial decomposers are essentially short-circuited electrochemical primary cells in which the graphite catalyst is the cathode and sodium amalgam the anode. The most common catalyst is graphite, usually activated by oxides of iron, nickel or cobalt or by carbides of molybdenum or tungsten. The decomposer operates at a temperature of approximately 90 – 130 ºC, which is caused by the chemical reactions in the decomposer and the input of warm amalgam from the cell electrolyser. Higher temperatures lead to a lower overpotential of hydrogen on graphite and therefore to a quicker reaction [ 1, Ullmann's 2006 ], [ 17, Dutch Ministry 1998 ]. Figure 2.4: Mercury cells with horizontal decomposer [Le Chlore, 1996] {The original black-and-white figure was replaced by Figure 2.4.} The mercury cell technique has the advantage over diaphragm and membrane cells that it produces a chlorine gas with nearly no oxygen, and a 50 wt-% caustic soda solution. However, mercury cells operate at a higher voltage than diaphragm and membrane cells and, therefore, use more energy (caustic soda concentration excluded). The technique also requires a pure brine solution with little or no metal contaminants to avoid the risk of explosion through hydrogen generation in the cell. The mercury cell technique inherently gives rise to environmental releases of mercury. {This text was moved to Section 2.2.1.} Figure 2.5: Mercury cells with vertical decomposer [Le Chlore, 1996] {The original black-and-white figure was replaced by Figure 2.4.} WORKING DRAFT IN PROGRESS 26 December 2011 TB/EIPPCB/CAK_Draft_1
2.3 The diaphragm cell technique process Chapter 2 {The paragraphs under this section have been rearranged to follow the same logic as the mercury cell technique. Section 2.3.1 description of electrolysis, products and qualities, extent of brine depletion, operating conditions, advantages/disadvantages; Section 2.3.2: description of cells with cathodes, anodes and diaphragms, monopolar/bipolar cells.} 2.3.1 General description The diaphragm cell technique process was developed in the 1880s in the US and was the first commercial technique process used to produce chlorine and caustic soda from brine. In North America, diaphragm cells are still the primary technique, accounting for roughly 70 % of all US production. The technique process differs from the mercury cell technique process in that all reactions take place within one cell and the cell effluent contains both dissolved salt and caustic soda. A diaphragm is employed to separate the chlorine liberated at the anode, and the hydrogen and caustic soda produced directly at the cathode (Figure 2.2). Without the diaphragm to isolate them, the hydrogen and chlorine would spontaneously ignite and the caustic soda and chlorine would react to form sodium hypochlorite (NaClO), with a further reaction to produce producing sodium chlorate (NaClO3) [ 17, Dutch Ministry 1998 ] [Kirk-Othm,er 1991]. The diaphragm is usually made of asbestos and separates the feed brine (anolyte) from the caustic-containing catholyte. Purified brine enters the anode compartment and percolates through the diaphragm into the cathode chamber. The percolation rate is controlled by maintaining a higher liquid level in the anode compartment to establish a positive and carefully controlled hydrostatic head. The percolation rate is determined as a compromise to maintain a balance between a low rate that would produce a desirably high concentration of caustic soda in the catholyte (which provides the cell effluent) and a high rate to limit back-migration of hydroxyl ions from catholyte to anolyte, which decreases cathode current efficiency [ 17, Dutch Ministry 1998 ] [Kirk-Othm,er 1991]. All diaphragm cells produce cell liquor that contains ca. 11% 10 – 12 wt-% caustic soda and 18% 15 – 17 wt-% sodium chloride. Generally, this solution is evaporated to 50 wt-% NaOH by weight at which point all of the salt, except a residual of approximately 1.0 wt-% 1.0-1.5% by weight, precipitates out. The salt generated is very pure and is typically used to make more brine [ 10, Kirk-Othmer 2002 ]. This high quality sodium chloride is sometimes used as a raw material for a mercury or membrane cell technique an amalgam or membrane process. A flow diagram of a possible integrated plant site is shown in Figure 2.5 on page 17. Brine Purification H 2 Cl 2 Mercury or membrane cells WORKING DRAFT IN PROGRESS Saturation H 2 Reclaimed salt TB/EIPPCB/CAK_Draft_1 December 2011 27 Cl 2 Diaphragm cells Concentration (only for 50 wt-% NaOH membrane technique) Depleted brine Concentration 50 wt-% NaOH 1 wt-% NaCl Figure 2.5: Flow diagram of the integration of the membrane or mercury and the diaphragm cell techniques {This figure was updated.}
- Page 1 and 2: EUROPEAN COMMISSION JOINT RESEARCH
- Page 3 and 4: PREFACE 1. Status of this document
- Page 5 and 6: Reference Document on Best Availabl
- Page 7 and 8: 3.4.7 Emissions of noise ..........
- Page 9 and 10: 4.3.6.3.3 Chemical reduction ......
- Page 11 and 12: List of Tables Table 2.1: Main char
- Page 13 and 14: List of Figures Figure 1.1: Share p
- Page 15 and 16: SCOPE WORKING DRAFT IN PROGRESS Sco
- Page 17 and 18: 1 GENERAL INFORMATION 1.1 Industria
- Page 19 and 20: Chlorine production in Mt/yr 12 11
- Page 21 and 22: Chapter 1 Figure 1.4 shows the annu
- Page 23 and 24: Share of total capacity in % 70 70%
- Page 25 and 26: 1.4 Chlor-alkali products and their
- Page 27 and 28: Total consumption: 9 801 kt Miscell
- Page 29 and 30: 1.4.5 Consumption of hydrogen Chapt
- Page 31 and 32: Chapter 1 and hazardous waste incin
- Page 33 and 34: 2 APPLIED PROCESSES AND TECHNIQUES
- Page 35 and 36: Chapter 2 WORKING DRAFT IN PROGRESS
- Page 37 and 38: Chapter 2 The main characteristics
- Page 39 and 40: 2.2 The mercury cell technique proc
- Page 41: Chapter 2 Characteristics of the ca
- Page 45 and 46: Source: [ 2, Le Chlore 2002 ] [USEP
- Page 47 and 48: 2.4 The membrane cell technique pro
- Page 49 and 50: Chapter 2 (carcinogenic) [ 76, Regu
- Page 51 and 52: Chapter 2 The membranes used in the
- Page 53 and 54: Table 2.2: Typical configurations o
- Page 55 and 56: 2.5 Brine supply 2.5.1 Sources, qua
- Page 57 and 58: Chapter 2 centrifuges before dispos
- Page 59 and 60: Source: [ 29, Asahi Glass 1998 ] (p
- Page 61 and 62: Impurity Source Upper limit of brin
- Page 63 and 64: Chapter 2 No such dechlorination tr
- Page 65 and 66: Chapter 2 The cooling water is gene
- Page 67 and 68: Chapter 2 composition of the chlori
- Page 69 and 70: 2.6.11 Dealing with impurities 2.6.
- Page 71 and 72: Chapter 2 amount of chlorine, and t
- Page 73 and 74: 2.6.12.2 Chemical reactions Chapter
- Page 75 and 76: 2.7 Caustic processing production,
- Page 77 and 78: Chapter 2 2.8 Hydrogen processing p
- Page 79 and 80: 3 CURRENT PRESENT EMISSION AND CONS
- Page 81 and 82: Chapter 3 Table 3.1: Overview of em
- Page 83 and 84: 3.3 Consumption levels of all cell
- Page 85 and 86: 3.3.3 Ancillary materials Ancillary
- Page 87 and 88: Further materials and/or further us
- Page 89 and 90: Chapter 3 current) and the efficien
- Page 91 and 92: Chapter 3 distance means a higher f
Chapter 2<br />
The electrolyser is operated at a temperature <strong>of</strong> approximately 70 – 80 ºC. The brine normally<br />
enters <strong>the</strong> electrolysis cell at 60 – 70 °C. At this temperature, <strong>the</strong> conductivity <strong>of</strong> <strong>the</strong> brine<br />
solution and <strong>the</strong> fluidity <strong>of</strong> <strong>the</strong> mercury are higher compared to operation at ambient<br />
temperature. The temperature can be achieved by preheating <strong>the</strong> saturated brine with steam and<br />
is increased in <strong>the</strong> cell electrolyser by <strong>the</strong> Joule heating heat <strong>of</strong> resistance to approximately<br />
about 75 – 85 °C. The heat produced during electrolysis and amalgam decomposition requires<br />
<strong>the</strong> air <strong>of</strong> <strong>the</strong> cell room to be changed 10 – 25 times per hour, depending on <strong>the</strong> type <strong>of</strong> building<br />
[ 1, Ullmann's 2006 ], [ 17, Dutch Ministry 1998 ].<br />
2.2.3 Decomposition <strong>of</strong> <strong>the</strong> amalgam<br />
The amalgam is decomposed in horizontal decomposers, alongside or beneath <strong>the</strong> cell (Figure<br />
2.4) or more <strong>of</strong>ten, since ca. 1960, in vertical decomposers (or denuders), at one end <strong>of</strong> <strong>the</strong> cell<br />
(Figure 2.5). Industrial decomposers are essentially short-circuited electrochemical primary<br />
cells in which <strong>the</strong> graphite catalyst is <strong>the</strong> cathode and sodium amalgam <strong>the</strong> anode. The most<br />
common catalyst is graphite, usually activated by oxides <strong>of</strong> iron, nickel or cobalt or by carbides<br />
<strong>of</strong> molybdenum or tungsten. The decomposer operates at a temperature <strong>of</strong> approximately<br />
90 – 130 ºC, which is caused by <strong>the</strong> chemical reactions in <strong>the</strong> decomposer and <strong>the</strong> input <strong>of</strong><br />
warm amalgam from <strong>the</strong> cell electrolyser. Higher temperatures lead to a lower overpotential <strong>of</strong><br />
hydrogen on graphite and <strong>the</strong>re<strong>for</strong>e to a quicker reaction [ 1, Ullmann's 2006 ], [ 17, Dutch<br />
Ministry 1998 ].<br />
Figure 2.4: Mercury cells with horizontal decomposer<br />
[Le <strong>Chlor</strong>e, 1996] {The original black-and-white figure was replaced by Figure 2.4.}<br />
The mercury cell technique has <strong>the</strong> advantage over diaphragm and membrane cells that it<br />
produces a chlorine gas with nearly no oxygen, and a 50 wt-% caustic soda solution. However,<br />
mercury cells operate at a higher voltage than diaphragm and membrane cells and, <strong>the</strong>re<strong>for</strong>e, use<br />
more energy (caustic soda concentration excluded). The technique also requires a pure brine<br />
solution with little or no metal contaminants to avoid <strong>the</strong> risk <strong>of</strong> explosion through hydrogen<br />
generation in <strong>the</strong> cell. The mercury cell technique inherently gives rise to environmental<br />
releases <strong>of</strong> mercury. {This text was moved to Section 2.2.1.}<br />
Figure 2.5: Mercury cells with vertical decomposer<br />
[Le <strong>Chlor</strong>e, 1996] {The original black-and-white figure was replaced by Figure 2.4.}<br />
WORKING DRAFT IN PROGRESS<br />
26 December 2011 TB/EIPPCB/CAK_Draft_1