carry electrons as there are more ions in the water‚ therefore the iron will rust faster. There are also many factors that will inhibit the rusting of iron. Examples of this are painting the iron‚ greasing the iron and electroplating the iron with copper and galvanizing the iron with zinc. Paint and grease are impermeable so oxygen and water cannot come into contact with the iron as the paint and grease would be in the way. Plating the iron (galvanizing) with zinc can inhibit the rusting process.
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The cost to buy a metal will be affected by how abundant the metal is. The more abundant a metal is‚ the less it will cost. This is because less time and money will be needed to find economically viable deposits of the metal. Example: The cost of Copper has increased due to a decline in availability. b The cost of production of a metal‚ which includes mining the ore and then refining it to obtain the final product‚ will affect the price of the metal‚ because the more costly it is to turn the ore
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(l) Water is added to make a pumpable slurry. Flotation (separation of valuable content) Cu2S(s) + H20 (l) CaCO3(s) (added to give a basic PH level) pine oil or C2H5OH (liquid called a frother) C3H5KOS2 (potassium amyl xanthate to make the copper particles cling to the bubbles as they rise to the surface) O2 (pumped into bottom of tank‚ agitates soloution and starts to froth‚ bringing bubbles to the surface) Cu2S particles adhere to the bubbles‚ which is separated from the liquid‚ tailings
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modern amalgam alloy • 67% silver‚ 27% tin‚ 5% copper‚ 1% zinc – overcame expansion problems History • 1960’s – conventional low-copper lathe-cut alloys • smaller particles – first generation high-copper alloys • Dispersalloy (Caulk) – admixture of spherical Ag-Cu eutectic particles with conventional lathe-cut – eliminated gamma-2 phase Classification According to content – Silver amalgam: Silver more than 65% – Copper amalgam: 70% Hg and 30% Cu According to presence
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Metal Q is added to salt solution of P. Q being more reactive ; displaces metal P from its salt solution. Chemical equation : Metal Q + Salt solution of P → Salt solution of Q + Metal P. Example : Zn Zinc + CuSO4 → ZnSO4 + Cu 1 Copper sulphate Zinc sulphate Copper 1 6. 1 volt is the potential difference between two points in a current carrying conductor when 1 joule of work is done to move a charge of 1 coulomb from one point to another. 1 Potential difference = = Work done (W) Charg e
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not easy. Batteries consist of two different metals suspended in an acidic solution. Copper and Zinc work well as the metals and the citric acid content of a lemon will provide the acidic solution. Batteries like this will not be able to run a motor or energize most light bulbs. It is possible to produce a dim glow from an LED. The picture at the top of this page shows a basic lemon battery‚ a lemon‚ copper penny and zinc coated nail. The lemon: A large‚ fresh‚ "juicy" lemon works best. The
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still it go back to its natural form. It became a big crystal. Naphthalene ball dissolve by means of air. It evaporates. Copper wire with Nitric Acid Objective: In this experiment‚ we’re going to find what will happen if we put the piece of copper wire in the Nitric Acid. And what type of reaction will occur. Materials: Test tube Graduated Cylinder Test tube rack Copper wire Beaker Nitric Acid Test tube holder Observation: 1. The color of the Nitric Acid is similar in the color
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platedmetals include nickel‚copper‚ and gold. While the electroplating is in progress‚ additionalsalts of the metal to be plated must continually be added to the platingsolution‚ or else the anode must be renewed‚ if it consists of the platingmetal. If the coating metal does not form a strong alloy with the metal to be plated‚ it may be necessary to first coat with an intermediate metal; for example‚ when plating silver on steel‚ it is customary to first place a coating of copper over the steel. When
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Qualitative Cation Tests Name Test Tube 1: HClNH3 Test Tube 2: NaOHExcess Aluminum 3+ No precipitate Slightly milky Dissolves Ammonium + No Precipitate No precipitate Calcium 2+ No Precipitate Milky white precipitate Precipitate does not dissolve Copper 2+ No precipitate Became much darker blue and milky Iron 3+ Brighter yellow Orange precipitate that then dissolves Lead 2+ Milky white precipitate Precipitate gets more milky Silver + Milky white precipitate Precipitate gets more milky with ammonium
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The lab was to include a purpose‚ procedure‚ data/observations‚ all reactions and side reactions written out with qualitative data beneath each product and reactant except H20‚ and a summary. The purpose of this experiment is to observe the qualitative aspects of a series of reactions involving copper. Procedure 1.Measure about 1g of solid copper. 2.Place Cu in Erlenmeyer flask and place flask under fume hood. 3.Add dropwise 15M HNO3 until solid copper is completely reacted. 4.Place flask
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