Copper And Silver Nitrate Lab Conclusion Essay

 

Copper and Silver Nitrate- Mike LiuObjective- To determine if the copper reacted was copper (I) or copper (II)Procedure-Weigh a Packet containing silver nitrate and transfer the AgNo3 into a small 50 mL beakercontaining 15 ml of distilled water. Mix until dissolved and weigh the paper. Make a copperwire assembly and weigh it. Transfer AgNO3 to a large test tube. Wash the Beaker twice with 5ml of distilled water, transferring the washings to a test tube. Wait 30 minutes while observingthe reaction. After 30 minutes are up, weigh a piece of filter paper and filter the silver. Discardthe filtrate and wash the filter paper twice with distilled water. Place the silver and filter paperin a small beaker, and put it on a window sill. Place the copper wire on a paper towel and weighboth the silver and copper wire during the next day.Observations-1.

Copper turns a bluish silver color and fuzz begins to form on the copper2.

Flakes start to fall off from the fuzz3.

Solution is now a light blue4.

There is a little bit of vapor condensing on the side of the test tube5.

Edge of copper is darkening after 30 minutes6.

Fuzz is brown in some areas while in others, silver7.

Solution is now a dark blue

Copper Cycle Essay

700 WordsOct 10th, 20103 Pages

Elena Chen
CH 221-227
November 3rd, 2009
Lab Report #3: Copper Cycle
Abstract:
The purpose of the experiment is to cycle solid copper through a series of five reactions. At different stages of the cycle, copper was present in different forms. First reaction involves reaction between the copper and nitric acid, and copper changed from elemental state to an aqueous. The second reaction converted the aqueous Cu2+ into the solid copper (2) hydroxide. In the third reaction Cu(OH)2 decomposed into copper 2 oxide and water when heated. When solid CuO reacted with sulfuric acid, the copper returned to solution as an ion (Cu2+). The cycle of reactions was completed with the reaction where elemental copper was regenerated by Zn and Cu…show more content…

Net ionic reaction: See attachment on the back for the net ionic equations
Reaction 4: CuO (s) + H2SO4 (aq) → CuSO4 (aq) + H2O (l)
Type of the reaction: Displacement/acid-base
Net ionic reaction: See attachment on the back for the net ionic equations
Reaction 5: CuSO4 (aq) + Zn (s) → ZnSO4 (aq) + Cu (s)
Type of the reaction: Redox
Net ionic reaction: See attachment on the back for the net ionic equations

Percent recover of copper=
Discussion:
In this experiment an elemental copper was cycled a series of five reactions where it ended with pure elemental copper as well, but at different stages of the cycle the copper was in different forms. In the first reaction, elemental copper was reacted with concentrated nitric acid where copper changed the form from solid to aqueous. Second reaction then converted the aqueous Cu2+ into the solid copper II hydroxide (Cu(OH)2) through reaction with sodium hydroxide. The third reaction takes advantage of the fact that Cu(OH)2 is thermally unstable. When heated, Cu(OH)2 decomposes (breaks down into smaller substances) into copper II oxide and water. When the solid CuO is reacted with sulfuric acid, the copper is returned to solution as an ion (Cu2+). The cycle of reactions is completed with the

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