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Copper Recovery Lab Report

471 Words2 Pages

The percent recovery of the copper was calculated using the equation, percent recovery = (the mass of the copper recovered after all the chemical reactions/the initial mass of the copper) x 100. The amount of copper that was recovered was 0.32 grams and the initial mass of the copper was 0.46 grams. Using the equation, (0.32 grams/0.46 grams) x 100 equaled 69.56%. The amount of copper recovered was slightly over two-thirds of the initial amount. Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and …show more content…

There are only two circumstances in which I think the copper could have been lost. The first chance where some of the lost mass of copper may have gone could have been during the first reaction. If distilled water was added to the solution before the chemical reaction finished, some copper may have been lost during that step. While all nitrogen dioxide gas seemed to have dissipated, perhaps, it was not finished yet. By stopping the reaction early, all of the solid, elemental copper may have not had a chance to react with the nitric acid, and some mass may have been lost during the step. The other time where mass could have been lost was during reaction 3, more specifically each time the liquid was decanted. Although a few black sand-coffee grains of the copper (II) oxide lost do not seem like a significant amount, they do have an impact on the final result, and each time a few of the grains were accidentally decanted could have an impact on why our final recovered mass was less than the initial amount that we began

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An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the

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801 Words | 4 Pages

RESULTS AND DISCUSSION Table of Results DDA Concentration (M) Initial Mass(g) Time Interval Recovered Mass (g) Cumulative Mass (g ) Cumulative Recovery (%) 10^(-5) 160 0

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Discussion 1. Zn0 (s)+ Cu2+S6+O42-(aq) →Cu0(s) + Zn2+S6+O42-(aq) Zn0(s) → Zn2+(aq) + 2e- Cu2+(aq) + 2e- → Cu0(s) Zn0(s) + Cu2+(aq) → Zn2+(aq) + Cu0(s) Oxidant (oxidizing agent) is the element which reduces in experiment.

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Deductive reasoning was used by determining the identity of an unknown copper mineral by looking at different possible copper minerals in the database with observations that were taken throughout the entire lab. Through roasting, the percentage of mass could be found through the mass of copper contained in an unknown copper containing mineral sample by gravimetric analysis of the copper (II) oxide produced. Through the idea of smelting and spectroscopy the identity of the unknown copper could be found through careful calculations and analysis of the lab.

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1931 Words | 8 Pages

When it stopped bubbling it indicated that Zn was gone and there wasn't any more to take part of a chemical reaction. It bubbled for a little while longer and I added 7 ½ + or - 1 mL more of sulfuric acid to finish up the chemical reaction. After this had finished I grabbed a new piece of filter paper, a new funnel, and drained out the filtrate and just the copper remained. I then finished the copper in the funnel 3 times with deionized water.

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728 Words | 3 Pages

The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.

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Error Analysis We may have made a few errors along the way. We could have had a blunder because we may not have waited long enough for the penny to stay on the scale. We could have made a human error because we could have had a little more or less sodium hydroxide in our graduated cylinder and eyeballed it wrong. Another error you could have made was an instrumental limitations because read the cylinder wrong on the side by

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1020 Words | 5 Pages

The volume stayed consistent because to decrease, the process needs activation energy. Once the activation energy was stored, the compost started to decrease almost linearly. The decreasing was due to worms eating the compost and disposing some of it as dirt, disposing some into the air (CO2), and using other part of the compost like the H’s as energy. This was due to cellular respiration; the worms used the compost for glucose, and due to homeostasis unused molecules were released through respiration.. The compost stayed constant again at the end of the experiment because worms started to die, and weren’t able reduce any more

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729 Words | 3 Pages

As the water was added to the heated sample, the solid copper chloride began to dissolve into a pretty blue-green solution, as a result of the compound breaking apart into individual Cu2+ and Cl- ions. When the water was first mixed with the copper chloride, it dissolved the solid pretty slowly, turning into a sort of mush at first. However, eventually, the water dissolved all of the solid copper chloride and the solution was homogenous. Since the compound just changed physical form, from solid to liquid, this change was purely physical. Just as in the first part of the experiment, the chemical character of the compound was not altered, so the compound did not experience a chemical change.

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578 Words | 3 Pages

The heating of the solution caused the reaction to start which decomposed Cu(OH)2 and made the solution colorless and darkened the precipitate. The fourth step was the formation of CuSO4. After the solution was decanted from the precipitate and washed with near boiling water, 6 M H2SO4 was added to the beaker containing Copper (II) Oxide and this caused the precipitate to dissolve and the liquid become clear blue. The last step was the formation of Cu(s). This step recovered Solid elemental copper.

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800 Words | 4 Pages

Introduction: The purpose of this experiment is to demonstrate the different types of chemical reactions, those including Copper. There are different types of chemical reactions. A double displacement reaction is a chemical process involving the exchange of bonds between two reacting chemical species. A a decomposition reaction is the separation of a chemical compound into elements or simpler compounds and the single-displacement reaction is a type of

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1237 Words | 5 Pages

If only one reactant is increased, then the chemical reaction will only produce a certain amount of products after the limiting reagent is used up, and in this experiment, the most mass the reaction could produce was 0.4 grams. Although we kept adding calcium chloride, not adding sodium hydroxide in the same proportions will not yield more product, which is the main goal in conducting this lab. We should have seen a plateau at 0.4 grams to show that the limiting reagent inhibited further Ca(OH)2 production, but we made several mistakes in our experiment, which made the data unusable to conclude. Once again, the data is polluted, so these number are not accurate, but it is the data our group has to work with. The theoretical yield should have been more than the actual yield, and the percentages should have been less than 100.

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1161 Words | 5 Pages

But the difference was no bigger than 0.08, and after the values were rounded the same empirical formula was deduced. So the experiment can be concluded as successful. Evaluation: The method used was simple and easy to follow; however, it did not include how much oxygen was needed to react completely. Also it didn 't mention what magnesium oxide looked like after it finished reacting, so it was a guesswork of determining whether the reaction was finished or not.

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851 Words | 4 Pages

This experiment is performed to test how Daphnia react when exposed to differing levels of copper sulfate so that we may understand what effects it has on underwater organisms. One possible hypothesis is, if the levels of copper sulfate in their environment rise, more of the Daphnia will die because copper sulfate is toxic. Daphnia are members of a collection of small crustaceans that are commonly called water fleas that are commonly found in small lakes and ponds. They reproduce through parthenogenesis, only creating male eggs once food becomes scarce. They eat algae, bacteria, and yeast.

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463 Words | 2 Pages

The purpose of this lab was to change pennies from copper to silver to gold, like alchemists have attempted to do in history. Through the data and observations gathered throughout this experiment, it can be concluded that the pennies were not changed into a different element. For example, the density of the penny from 2005; which was the penny that was experimented on to see whether or not it could turn into silver; was 4.62 g/cm3 before the experiment and 4.89 g/cm3 by the end of the experiment. If this copper penny really would have turned into silver, then the density of the penny would be 10.49 g/cm3; which is the density of silver; by the end of the experiment. The penny may have turned silver in color, but this was only because it was plated in the zinc that was added to the beaker of water in the experiment.

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