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Chloride process

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<div id="mw-content-text" class="mw-body-content mw-content-ltr" lang="en" dir="ltr"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr">The chloride process is used to separate <a href="Titanium" title="Titanium">titanium</a> from its ores. The goal of the process is to win high purity <a href="Titanium_dioxide" title="Titanium dioxide">titanium dioxide</a> from ores such as <a href="Ilmenite" title="Ilmenite">ilmenite</a> (FeTiO3) and <a href="Rutile" title="Rutile">rutile</a> (TiO2). The strategy exploits the volatility of TiCl4, which is readily purified and converted to the dioxide. Millions of tons of TiO2 are produced annually by this process, mainly for use as white pigments. As of 2017, the chloride process is used alongside the older sulfate process, which relies on hot <a href="Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> to extract iron and other impurities from ores.<a href="#cite_note-Ullmann-1">[1]</a>: 15

<div class="mw-heading mw-heading2"><h2 id="Process_chemistry">Process chemistry</h2></div>

In this process, the feedstock is treated at 1000 °C with <a href="Carbon" title="Carbon">carbon</a> and <a href="Chlorine" title="Chlorine">chlorine</a> gas, giving <a href="Titanium_tetrachloride" title="Titanium tetrachloride">titanium tetrachloride</a>. Typical is the conversion starting from the ore <a href="Ilmenite" title="Ilmenite">ilmenite</a>:<a href="#cite_note-2">[2]</a>

<dl><dd>2 FeTiO3 + 7 Cl2 + 6 C → 2 TiCl4 + 2 FeCl3 + 6 CO</dd></dl>

The process is a variant of a <a href="Carbothermic_reaction" title="Carbothermic reaction">carbothermic reaction</a>, which exploits the reducing power of carbon.

The titanium tetrachloride is purified by <a href="Distillation" title="Distillation">distillation</a>. Other impurities are converted to the respective chlorides as well, but most are less volatile than TiCl4. <a href="Vanadium_tetrachloride" title="Vanadium tetrachloride">Vanadium tetrachloride</a> and <a href="Vanadium_oxytrichloride" title="Vanadium oxytrichloride">vanadium oxytrichloride</a> codistill with TiCl4, but these impurities can be removed by chemical reduction.<a href="#cite_note-Ullmann-1">[1]</a>: 13

It can be subsequently oxidized in an <a href="Oxygen" title="Oxygen">oxygen</a> flame or plasma to give the pure titanium dioxide.<a href="#cite_note-Ullmann-1">[1]</a>: 13 <a href="#cite_note-3">[3]</a><a href="#cite_note-Kirk-Othmer-4">[4]</a>

In this way, chlorine is recovered for recycling.

<div class="mw-heading mw-heading2"><h2 id="Process_engineering">Process engineering</h2></div>

The standard chloride process for titanium dioxide base material consists of the following main production units:<a href="#cite_note-5">[5]</a>

<ul><li>Oxidation</li>

<li>Chlorination</li>

<li>Condensation</li>

<li>Purification</li></ul>

The following auxiliary production units are necessary:

<ul><li>Ore/coke storage</li>

<li>Off-Gas Treatment</li>

<li>Dust treatment</li></ul>

Under steady state conditions the chloride process is a continuous cycle in which chlorine changes from the oxidized state to the reduced state and reverse. The oxidized form of the chlorine is molecular chlorine Cl2, the reduced form is titanium tetrachloride (TiCl4). The oxidizing agent is molecular oxygen (O2), the reducing agent is coke. Both must be fed into the process. The titanium is fed into the process in form of ore together with the coke. Titanium ore is a mixture of oxides. The added O2 leaves the process with the product TiO2, the added coke leaves the process together with the added oxygen from the titanium ore in form of CO and CO2. The other fed metals leave the process in form of metal chlorides.<a href="#cite_note-6">[6]</a>

<div class="mw-heading mw-heading2"><h2 id="References">References</h2></div>

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</style><cite id="CITEREFAuerWoditschWesterhausKischkewitz2017" class="citation encyclopaedia cs1">Auer, Gerhard; Woditsch, Peter; Westerhaus, Axel; Kischkewitz, Jürgen; Griebler, Wolf-Dieter; Rohe, Markus; Liedekerke, Marcel (2017). "Pigments, Inorganic, 2. White Pigments". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. pp. 1–36. <a href="Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1002%2F14356007.n20_n01.pub2">10.1002/14356007.n20_n01.pub2</a>. <a href="ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <bdi>978-3-527-30673-2</bdi>.</cite>

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<li id="cite_note-2"><a href="#cite_ref-2">^</a> <cite id="CITEREFGreenwoodEarnshaw1997" class="citation book cs1"><a href="Norman_Greenwood" title="Norman Greenwood">Greenwood, Norman N.</a>; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). <a href="Butterworth-Heinemann" title="Butterworth-Heinemann">Butterworth-Heinemann</a>. <a href="Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1016%2FC2009-0-30414-6">10.1016/C2009-0-30414-6</a>. <a href="ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <bdi>978-0-08-037941-8</bdi>.</cite>

</li>

<li id="cite_note-3"><a href="#cite_ref-3">^</a> <cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://ti-cons.com/technology/">"The TiO2 Process"</a>. Ti-Cons. Retrieved 2016-12-17.</cite>

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<li id="cite_note-Kirk-Othmer-4"><a href="#cite_ref-Kirk-Othmer_4-0">^</a> <cite id="CITEREFJonesEgerton2000" class="citation book cs1">Jones, Tony; Egerton, Terry A. (2000). "8.3 Titanium Dioxide. Chloride Process". Kirk-Othmer Encyclopedia of Chemical Technology. John Wiley & Sons, Inc. pp. 22–23. <a href="Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1002%2F0471238961.0914151805070518.a01.pub3">10.1002/0471238961.0914151805070518.a01.pub3</a>. <a href="ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <bdi>9780471238966</bdi>.</cite>

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<li id="cite_note-5"><a href="#cite_ref-5">^</a> <cite class="citation web cs1"><a rel="nofollow" class="external text" href="http://arquivo.pt/wayback/20110124235702/http://www.huntsman.com/pigments/Media/Manufacture_and_Generals_Properties.pdf">"Manufacture and General Properties of Titanium Dioxide Pigments"</a> (PDF). Ti-Cons. Archived from <a rel="nofollow" class="external text" href="http://www.huntsman.com/pigments/Media/Manufacture_and_Generals_Properties.pdf">the original</a> (PDF) on 2011-01-24. Retrieved 2012-04-11.</cite>

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<li id="cite_note-6"><a href="#cite_ref-6">^</a> <cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://ti-cons.com/wp-content/uploads/2023/03/ti-cons_pt_en.pdf">"The Details of the TiO2 Process"</a> (PDF). Ti-Cons. Retrieved 2012-04-11.</cite>

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<div class="mw-heading mw-heading2"><h2 id="External_links">External links</h2></div>

<ul><li><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://web.archive.org/web/20190620201100/https://kronostio2.com/en/about-tio2/chloride-process">"Chloride Process"</a>. KRONOS Worldwide, Inc. Archived from <a rel="nofollow" class="external text" href="https://kronostio2.com/en/about-tio2/chloride-process">the original</a> on 2019-06-20. Retrieved 2020-05-11.</cite></li>

<li><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://ti-cons.com/technology/">"The Chloride Process from Ti-Cons"</a>. Ti-Cons Jendro, Weiland und Partner. Retrieved 2010-06-16.</cite></li></ul></div><div><div class="zim-footer">

This article is issued from <a class="external text" title="Last edited on 2025-03-15" href="https://en.wikipedia.org/wiki/?title=Chloride_process&oldid=1280533795">Wikipedia</a>. The text is available under <a class="external text" href="https://creativecommons.org/licenses/by-sa/4.0/deed.en">Creative Commons Attribution-Share Alike 4.0</a> unless otherwise noted. Additional terms may apply for the media files.

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