Hydrometallurgy to Analyze a Chromite Sample 10/8/09 Introduction: Chromium is very important for industries in the present day. Chromium is essential in hardening steel, manufacturing stainless steel, and forming many useful alloys. Chromium is used to plate metals, pigments, leather processing, catalysts, surface treatments, and refractories. Chromium is used to prevent corrosion. The only ore that contains chromium is the mineral chromite, which is iron magnesium chromium oxide.
Hydrometallurgy to Analyze a Chromite Sample : Chromium can be used in the production of stainless steel and other nonferrous alloys in order to enhance their harden ability and to make the alloys more resistant to corrosion and oxidation. It can also be used to plate metals, make pigments, process leather, catalyze, and treat surfaces. Chromite is the only ore of chromium. Chromite is iron magnesium chromium oxide. Metallurgy can be used in order to recover the chromium from the chromite ore.
Also, the chromium in chromite may sometimes be replaced by aluminum and ferrous ions. Hydrometallurgy is a way to separate the different elements making up ores and isolate the metals from each other. In order for this to occur, the ore must be melted down into a solution. After the metals of the ore have been dissolved, they may be separated from each other by many different processes, some of the most popular are leaching and precipitating the metal from the solution via electrolysis or chemical means. In this experiment the team of students must determine exactly what is in chromite sample, and also confirm the existence of all such metals that should be in the sample of chromite.
Chromite is iron magnesium chromium oxide. In some rare cases, magnesium is substituted for iron. Also aluminum and ferric ions can substitute chromium in a reaction. Hydrometallurgy is a form of extractive metallurgy that utilizes aqueous solution chemistry for the recovery of metals from salts, minerals, or ores. Extraction is a process in which metal is removed from an ore by dissolving the metal in a solvent, then recovering the metal from the solution (This is done by dissolving the metal into an acid or water).
These impurities include vanadium, arsenic, zirconium, iron, silicon, and magnesium. Therefore, impure titanium tetrachloride is then cleaned of all these impurities for the purpose of gaining a pure titanium tetrachloride. The cleaning process is initiated by allowing the former mixture to settle, where the undissolved particles are removed as dirt or mud. Afterwards, the liquid that contains several chlorides is passed through a distillation column and is chemically treated with hydrogen sulfide or mineral oil to eliminate vanadium oxychloride, which is a chloride that boils at the same temperature as titanium tetrachloride. Finally, it is redistilled again to further purify the titanium tetrachloride produced.
The copper is then fed to electrolysis for refining. In an aqueous solution copper is dissolved at the anode, the ion moves across the electrolyte to the cathode and plates out. Cu → Cu2+ + 2 e- (anode) Cu2+ + 2 e → Cu (cathode) Aluminum are commercially extracted mainly from bauxite, which is mostly gibbsite (Al(OH)3). The Bayer process is used to refine the bauxite into alumina or aluminum oxide, which
A circumstance without any of the evidences present concludes that a chemical reaction has not occurred and thus a displacement reaction has not taken place. Figure 1 Figure 1 chlorine + sodium iodide iodine + sodium chloride (non-metal) (compound) (non-metal) (compound) Cl2 + 2 NaI I2 + 2 NaCl Figure 2 Figure 3 Figure 3 (Source of Figure 3: http://vinstan.wikispaces.com/Chapter+3+++++Chemical+Reactions) Purpose: The main objective of Activity Series of Metals is to determine the reactivity of common metals. For this lab we should be able to find out and predict the products that come from a
Extended Practical Investigation The catalysis of the reaction between zinc and sulphuric acid The activation energy of the reaction will be estimated using experimental data, a catalyst will be added and the activation energies will be compared to see if the catalyst has had an effect on this. Contents Aims and objectives 3 Background 3 Preliminary experiments 4 Equipment 4 Method 4 References 5 Risk Assessment 6 Aims and objectives The effect of adding a copper catalyst to the reaction between zinc and sulphuric acid on the activation energy will be investigated. The effect of copper as a catalyst on the rate of the reaction will be observed and the Arrhenius equation will be used to calculate the activation energy. Background Acids react with some metals to produce a metal salt and hydrogen gas. Zinc reacts with sulphuric acid, producing hydrogen gas.
Main – group metals usually for one cation (positive ion). In a binary ionic compound the metal (cation) is named first. Then the nonmetal (anion) is named, and the suffix -ide is added. To create the formula, you switch the charges, and that tells you how many of each element you will need. For example: Cation Anion Formula Name of Compound Ba2+ I- Ba2+ I- Barium Ion Iodide Ion BaI2 Barium Iodide Type 2: Binary Ionic Type 2 Binary Ionic compounds consist of a metal and a nonmetal.
Alkali Metals- Group 1 (IA) The alkali metals make up Group 1 of the periodic table. This family consists of the elements lithium, sodium, potassium, rubidium, cesium, and francium (Li, Na, K, Rb, Cs, and Fr, respectively). Group one elements share common characteristics. They are all soft, silver metals. Due to their low ionization energy, these metals have low melting points and are highly reactive.