Chemical Reactions Lab

This experiment was performed to demonstrate a cycle of chemical reactions involving copper. This lab will start with copper as a reactant in the first reaction through a series of five chemical forms of aqueous phase reactions and ending to calculate the percentage of recovered solid copper as a product in the last reaction of the experiment. The experiment resulted in a percent recovery from the cycle of copper reactions of an increase to 139%.
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Introduction: The purpose of this experiment is to become accustomed with different types of aqueous reaction types. Our task will be to use a variety of chemical forms to transform copper metal back to its solid state. If copper is transformed through five different reactions ending is solid copper
Reaction 1, we start with 0.503 g copper metal that dissolves in 5.0 mL of concentrated nitric acid. This is an example of redox as a transfer of electrons is occurring. The second part of the reaction allows the nitrate ion to oxidize the copper. Reaction two, while stirring 20 mL of 6.0 M NaOH was added to the flask. Hydroxide ion binds to the copper (II). This is an example of metathesis as the cations and anions exchange partners. Reaction Three, Heating the copper hydroxide to a medium boil on the hotplate while occasionally stirring produces copper oxide. Heating allows for decomposition. It also allows the copper to oxidize. 50 mL of hot water was added three times and then decanted the supernatant solution. Reaction 4, Copper oxide is dissolved with 5 mL of 6.0M Sulfuric Acid. This allows the Oxygen to bind with to water and allow the Copper (II) ion to reform. Reaction 5, 1.0 g of 30-mesh Zinc is added. Start with half and add remain half of zinc until solution lacks the blue hue. Followed by adding 10 mL of concentrated HCl. This should eliminate the zinc through gas form decant the liquid and heat until copper is dry. Weigh out the flask + copper. Then determine the percent