to carry out an extensive series of reactions based on the element copper. These reactions include; synthesis‚ decomposition‚ single and double replacement. In this experiment‚ recycling will also be introduced. Procedure: See attached Story board. Data and Observations and Data Analysis: Step Word Equation 1 Balanced Chemical Equation Type of Reaction Observations Copper + nitric Cu + 4HNO3 acid à copper(II) à Cu(NO3)2 + nitrate + nitrogen 2NO2 + 2H2O dioxide + water
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we will study is called copper chloride hydrate. We first drive out the water‚ which is called hydration. This occurs if we gently heat the sample to a little over 100*C. The compound formed is anhydrous (no water) copper chloride. If we subtract its mass from that hydrate‚ we can determine the mass of the water that was driven off‚ and using the molar mass of water‚ find the number of moles of H2O that were in the sample. Next‚ we need to the find either the mass of copper of chlorine in the anhydrous
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using cutters. 7 If not‚ skip the above step and continue by soldering 2 cables onto the two capacitor terminals. Wire one of these to a high current switch. 8 Form a load coil by wrapping 5-10 of turns of thick‚ insulated‚ stranded copper wire around a former approximately 1-2 inches (25-50mm) in diameter. With care‚ slide the windings off the former and bind together with adhesive tape. 9 Connect one of the leads of the load coil to the other unused terminal on the switch
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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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hydrated copper (II) sulphate compound? Controlled Variable: The mass of hydrated copper (II) sulphate. Responding Variable: The mass of dehydrated copper (II) sulphate‚ mass of H2O Materials: Ones on the handout + Hot plate. Procedure: 1. Mass 3.00g of hydrated copper (II) sulphate using electronic balance 2. Measure the mass of a thin‚ crucible dish using electronic balance 3. Gently pour hydrated copper (II) sulphate into the crucible dish 4. Heat the hydrated copper (II)
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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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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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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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I. Title: Iron-Copper (II) Chloride Reaction II. Purpose: The purpose of this lab is to see how iron reacts with a copper (II) chloride solution. III. Equipment and Reagents Scoop copper (II) chloride (CuCl2) Beaker Iron (Fe) Wash Bottle water (H2O) Scale Hydrogen chloride (M HCl) Filter Paper IV. Procedure: 1. Obtain a clean‚ dry 250 mL beaker. 2. See teacher to obtain a scoop of CuCl2 in the beaker. 3. Add approximately 50 mL of tap water to
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