Copper Synthesis Experiment
Essay by review • February 24, 2011 • Lab Report • 1,123 Words (5 Pages) • 4,396 Views
Experiment 1: Synthesis of Copper Compounds
Introduction
This experiment involves the synthesis of compounds originating from pure solid copper. By applying solubility rules and the reactive properties of substances, many compounds which would otherwise be costly to extract from nature are able to be synthesized in the laboratory. Laboratory synthesized may sometimes be more economical than natural extraction, however it poses its own problems with the amount of substance that is actually yielded from the production reactions (Stathopulos, 2007). Almost no reaction has 100% yield, thus 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 refer to "Experiment 1: Synthesis of Copper Compounds" on pages 11-13 in the CHEM 120L lab manual for the procedure outline. All steps were followed without deviation.
Results and Observations
Please refer to the calculations and tables (16) located on the following 2 pages.
INITIAL MASS (copper wire) - 1.120g FINAL MASS (recovered copper - dish mass) - 37.88g
% Recovery = Recovered mass / Initial Mass . 100 = 37.88g / 1.120g . 100 = 3382%
Table 1- Reaction of Cu with Nitric Acid
Reaction Cu + 4HNO3  Cu(NO3)2 + 2NO2 + 2H2O
Description * Nitric acid dissolved copper wire completely
* A brown gas was produced
* Black precipitate formed
Table 2- Formation of Cu(OH)2
Reaction Cu(NO3)2 + 2NaOH  Cu(OH)2 + 2NaNO3
Description * Solution turned from a bright blue colour to a very dark blue
* Solution turned from very light to extremely thick, almost sludge like
Table 3- Conversion of Cu(OH)2 to CuO
Reaction Cu(OH)2 + heat  CuO + H2O
Description * Black precipitate formed while heating
* Lost 1 drop in transition to filter
* Filtrate was clear
* Sediment left on filter paper was black and clay-like
Table 4- Formation of CuSO4 from CuO
Reaction CuO + H2SO4  CuSO4 + 5H2O
Description * Black precipitate dissolved and solution turned blue with the addition of H2SO4
* Not all CuO dissolved
* Heat was required to dissolve additional CuO
Table 5- Formation of Cu metal from CuSO4
Reaction CuSO4 + Zn  Cu + ZnSO4
Description * Solid orange precipitate formed
* Clear/yellowish gas is produced
* Zinc dissolves
Table 6- Removal of excess Zn with acid
Reaction 2ZnSO4 + 2 HCl  2ZnCl + H¬¬2 + 2SO4
Description * No reaction occurred
* All excess zinc was used up
* Small amount of CuO residue
Discussion
What this lab mostly involved was the formation of new substances and combinations of copper using prior knowledge of reactivity and solubility rules. The intent of the experiment was to perform all the reactions only to return to the pure form of copper again. A reasonable percent recovery would be 90% +, however, the percent recovery obtained in our experiment was an outrageous and impossible figure of 3382%. Unless the law of conservation for matter is wrong, only error can explain that abnormal figure. Under the guidance of our TA, we were advised to remove our evaporating dish from the Bunsen burner to prevent overheating and the formation of copper oxide. A very reasonable claim, though in doing so it left much of the water un-evaporated accounting for much of the extra mass measured. The heat that was being applied was not intense heat, it was turned down to a rather low setting so that it would be hot enough to evaporate the water but not cause the copper to "pop" and end up all over the counter top. in addition, the copper was likely bunched up in the dish opposed to spread out which may also contribute to the lack of evaporation. The formation of copper oxide render the copper sample impure as it would have additional oxygen mass. Aside from the obvious mass error,
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