Chemical reaction of copper and percent yield

Decantation errors could be avoided by employing filtration techniques instead of decantation techniques. Throughout the entirety of the lab, there were many steps that presented possible sources of error such as adding too much or too little of a compound to the copper solution, or the loss of copper during transport or by being left on the stirring rod.

This is equivalent to 8. This occurs when reactions are not allowed to finish. Personal ramifications include increased laboratory experience and increased understanding of redox and metathesis reactions.

In the final reaction, solid zinc was added to aqueous copper sulfate. Open flames must not be used in the presence of either of these substances. The contents of the beaker were stirred.

Ice water is used as an absorber for the heat released in this reaction. The copper was washed with 5 mL of distilled water. The unwanted precipitate will not participate in subsequent reactions, causing a constant unwanted mass in addition to the desired mass of reaction products.

This is equivalent to 2. Washing that solution removed all other ions or precipitates from the beaker. The acetone was decanted. Clearly these values are not the same as hypothesized, due to a variety of sources of error throughout the lab.

The precipitate in the beaker was allowed to settle. Black Copper Oxide precipitate formed and water formed.

The evaporating dish and copper were weighed and the mass was recorded. During step 5, stirring of the mixture was required, so another source of error was that copper from the beaker may have been left on the stirring rod.

The function of using the ice bath in this step is to control the temperature of the reaction, because the reaction may become too violent if nothing is used to cool it down.

The reaction that occurred in step 9 was a single replacement reaction. Thus, 0 g of O2 remains. A double replacement reaction took place in step 4 between the copper nitrate and sodium hydroxide.Mass of Dish, Watch Glass, and Copper g Mass of Copper Chemically Foundg Percent Yield = Actual/Theoretical X Percent Yield/ X = % Conclusion The objective of this lab was to fully carry out five reactions of copper, and to observe and understand the methods behind each reaction.

Determine a percent yield for the mass of recovered copper. The actual yield is the amount you ended up with, the theoretical yield can be found from the limiting. Chemical Reactions of Copper and Percent Yield 1.

Weight copper initial _____ 2. Weight of copper and evaporating dish _____ 3. Weight of evaporating dish _____ 4. Chemical Reactions of Copper and Percent Yield ny time an acid is added to a metal hydrogen gas is released.

We also checked with a glowing wooden splint that burst into flames when placed in the beaker.5/5(6). Oxidation-reduction (redox) reactions and metathesis (single-replacement) reactions will be used.

The objective of the experiment is to recover as much of the original copper as possible. The quantitative measure of success in this experiment is percent yield, which is the ratio of recovered mass to initial mass.

Percent Yield

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Chemical reaction of copper and percent yield
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