CHEMICAL REACTION (SYNTHESIS REACTION‚ DECOMPOSITION AND SINGLE REAPLACEMENT REACTION) Purpose : 1. To identify the chemical changes 2. To observe the effect of temperature of a chemical reaction. Theoritical basic : A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Classically‚ chemical reactions encompass changes that strictly involve the motion of electrons in the forming and breaking of chemical bonds between
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scientists inadvertently produce undesired products that must be filtered or decanted out of solution (Petrucci et al‚ 2007). Beginning with pure copper wire‚ this experiment will exhibit its transformation to substances including Cu(NO3)2‚ Cu(OH)2‚ CuO‚ CuSO4 . 5H2O and finally returning to pure copper (Cu). The experiment objective is to successfully complete these conversions and then calculate the percentage of recovered copper using the initial and final mass data obtained. Procedure Please
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questions about chemical reactions dealing with “how much” and “how many.” In the first part of this experiment you will investigate the reaction of copper metal with oxygen in the air. Using stoichiometry‚ you can predict the amount of copper oxide (CuO) that could be produced if all the copper would react. However‚ when you perform the reaction yourself‚ you will discover that only some of the copper reacts to form black copper oxide. A stoichiometric calculation will allow you to determine the
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TITLE : The copper cycle IN TRODUCTION The purpose of the experiment is to recognize that change of state‚ change in colour‚ formation of a precipitate‚ or the evolution of heat are associated with a chemical change; to study reactions of copper. Copper is an element that can be found in nature in a variety of different compounds. The most common natural ore is the sulphide‚ known as chalcocite‚ Cu2S. This mineral is an important source of copper metal because it is about 80% copper by
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Equations: 1) Cu + 4H+(aq) + 2NO3-(aq) Cu2+ + 2NO2 + 2H2O 2) Cu2+(aq) + 2-OH(aq) Cu(OH)2 3) Cu(OH)2 + heat CuO + H2O 4) CuO + H2SO4 Cu2+(aq) + SO42-(aq) + H2O 5) Cu2+(aq) + Zn Cu + Zn2+(aq) Stage 1- Dissolution of Copper Mass of vial & copper = 3.537g Mass of vial = 2.505g Mass of Copper = 1.032g Moles of copper = mass (g) ÷ (63.5g/mol) = 0.0162 mol (3s.f) Copper description: Initially‚ the copper was a solid that was
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Part C Observations Solution becomes darker Part D Observations Mixture goes back to its natural state Part E Observations Bubbling Heat is generated Liquid is clear In-Lab Discussion 1) A. Cu (NO2)2 Cu (OH)2 B. Cu (OH)2 CuO C. CuO CuSO4 D. CuSO4 Cu0 Post Lab Discussion 2) 1.95/0.91*100= 214%; we were not able to verify the Law of Conservation of Mass within 5% of the
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temperature of a Bunsen burner flame‚ whereas the carbonates of silver and copper are easily decomposed. In this experiment copper (ii) carbonate will be decomposed at a high temperature‚ forming copper (ii) oxide and carbon dioxide: CuCO3(s) arrow CuO(s) + CO2(g) You will test for the formation of copper (ii) oxide and carbon dioxide. Limewater is a sensitive test for CO2‚ forming a distinctive milky precipitate: CO2(g) + Ca(OH)2(aq) arrow CaCO3(s) + H2O(l) APPARUTUS: * fat Pyrex test tubes x
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Objectives n To observe a sequence of chemical reactions starting and finishing in elemental copper metal‚ and to practice quantitative laboratory techniques. Cu → Cu(NO3)2 → Cu(OH)2 → CuO → CuSO4 → Cu Cu(NO3)2 = copper nitrate Cu(OH)2 = copper hydroxide CuSO4 = copper sulfate CuO = copper oxide Experiment 1(a) Cu + 4HNO3 → Cu(NO3)2 + 2NO2↑ + 2H2O NO2 given off as a coloured gas* H(NO)3 Transfer contents to beaker containing 100 mL of water Cu 100mls H2O Wash
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the residue is found to weigh 18g‚ what is the mass of CO2 released in the reaction? 3. In an experiment‚ 1.375g of CuO was reduced by heating in a current of hydrogen and the weight of copper that remained was 1.098g. In another experiment‚ 1.179g of CuO was dissolved in nitric acid and the resulting Copper(I) nitrate converted into CuO by ignition. The weight of CuO that was formed was 1.476g. Show that these results illustrate the law of constant proportions. 4. Carbon and oxygen are
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Need to Know Know the reaction equations‚ which reactions occur (ex. by heating‚ etc.) and physical descriptions/color of tings Ex. CuO (s) (black solid) + H2SO4 (aq) + H2O --> Cu(SO)4 (aq) (blue solution) + H2O Know how to calculate percent yield (i.e. CuSO4 was obtained from the reaction of CuO with sulfuric acid. If 2.5 g of CuSO4 was obtained from 5.0 g of CuO‚ what is the percent yield?) Purpose To observe the chemical properties of copper through a series of reactions To recover the
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