door frames‚ paneling)- Aeroplanes- Motor car parts (cylinder heads‚ radiator cores)- High voltage transmission lines- Domestic pots and pans and wrapping foil- Drink containers- Electric wiring over long distances (long distance power lines) | Copper | - Electrical wiring (household and street cables)- Pipes and plumbing fittings - Electroplating‚ jewellery and household decorations | Zinc | - Galvanizing iron (surface coating)- Protective paints and electroplating- Diecast alloys (car carburetors)
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Have you ever wondered what drove modern humans to abandon bronze for iron? In this paper I will present the reasons for and the techniques used to develop iron into a useable metal that is far superior to bronze. Topics will include‚ when iron was first used‚ the accidental discovery of steel‚ and why bronze was replaced by iron. First though‚ let us look at the origins of iron. The Iron Age began around 1200 BC‚ according to Scarre‚ in southwest Asia (2005:434). It is know however that iron
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project value addition done by financial manager. • Southport Indonesia (SI)‚ a wholly-owned subsidiary of Southport Minerals‚ entrusted with a responsibility of mining the copper ore at Firstburg‚ Indonesia. o Initial experiments established that Firstburg mine contained 33 million tons of copper ore with an average copper content of 2.5%. o Bechtel conducted the cost and feasibility studies and informed that the total development cost would be $120mil and could be operationalized by end of 1972
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Exercise in Extracting Copper from a Synthetic Copper Ore Your Name __Mel Hine______________________ Partner’s Name __Jay Ranson____________________ Date _October 2‚ 2012____________ Introduction This laboratory exercise involves the use of dilute sulfuric acid (H2SO4) to leach copper from a synthetic copper-containing ore
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mass of copper formed when excess aluminum is reacted with a given mass of a copper salt (Copper Chloride dihydrate)‚ and the mole-to-mole ratio between the reactant and the product of a chemical reaction. Apparatus * 150ml beaker * Stirring rod * Ruler * Hotplate * Tweezers * 50ml graduated cylinder Materials * Copper (II) chloride dehydrate * Aluminum foil Procedure 1) Determine the mass of a clean 150ml beaker. 2) Add 2g of copper (II) chloride
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the most amount of copper after it is subjected to a sequence of reactions. The copper is originally in solid form‚ but the reactions will turn it into free Cu+2 ions floating in solution. The ions will then be regrouped to form solid copper once again. During this process‚ however‚ some of the Cu+2 ions may be lost. The copper will subjected to changes in pH and heat. These steps were responsible for the breakdown and reconstruction of the copper. The percent of copper retrieved will reflect
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9/19/06 Lab Report The Empirical Formula of a Copper Oxide Purpose: To convert an unknown copper oxide to copper (Cu) metal using natural gas to provide a reducing environment as shown below: Cu O (s) + CH (g) ¨ Cu (s) + Co (g) + H O (g) From the mass difference between the unknown copper oxide and the Cu metal generated at the completion of the reaction and the molar mass of Cu and oxygen‚ the empirical formula of the original copper oxide can be calculated. Materials: gCopper
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CHEMICAL REACTIONS OF COPPER AND PERCENT YIELD Objective To gain familiarity with basic laboratory procedures‚ some chemistry of a typical transition element‚ and the concept of percent yield. Apparatus and Chemicals |0.5 g piece of no. 16 or no. 18 copper wire |evaporating dish | |250 mL beaker (2) |weighing paper | |concentrated HNO3 (4 – 6 mL)
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Introduction: Copper (II) Chloride is the compound with a chemical formula of CuCl2. This is a light brown solid‚ which slowly absorbs moisture to form a blue green dihydrate. Copper (II) Chloride is highly soluble in water and will produce a blue solution. solutioAluminum is the compound that has a chemical formula of Al. This is a silver solid that can be easily formed‚ machined‚ or cast. In this lab‚ we will be finding the limiting reactant between Copper(II) Chloride and Aluminum. The limiting
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Purpose: To find out the percent yield of copper in the reaction between copper sulfate (CuSO4) and Iron (Fe). Materials: Balance 100-mL beaker 250-mL beaker Bunsen burner Copper sulfate crystals Glass stirring rod 100-mL graduated cylinder Iron filings Ring stand and ring Wire gauze Procedure: 1. Record mass of clean 100-mL beaker. 2. Add 8.0 grams of copper sulfate crystals to beaker. 3. Add 50.0 milliliters of distilled water to the crystals. 4. Put wire gauze on ring on ring
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