Should We Mine This Ore Lab Report

This labs objective was to determine how much copper is in a penny. Concepts that were used for this lab were calibration curves, and oxidatoin of metal.

Due to this fact, the concentration of copper in the solution is able to be calculated by using light absorbance. Since zinc doesn’t absorb any light, we are able to deduce that the greater the absorbance, the greater the concentration of copper.

After this, the solution was poured into a volumetric flask just about to the 1dm3 line and then it was left there to cool to the same temperature as the room before filling precisely to the 1dm3 line with distilled water. The molar mass of CuSO4.5H20 was 249.5 so that means 249.5g of copper sulphate was needed to dissolve, in order to make a standard solution, into 1dm3of distilled water. Following this, a linear dilution of the CuSO4.5H2O was made in order to be used to make a calibration curve after using the colorimeter to write down the absorbance of each sample. A linear dilution is diluted with distilled water in order for it to make the concentration weaker and weaker. For this investigation, the dilutions made ranged from 0.01 to 0.1 M/l . It was essential to only make up 10cm3

Washing of the copper is necessary in this experiment to separate the iron from the copper and make sure the iron is not counted in the mass of the copper.

Obtain a 50 mL beaker for the experiment. In the first part of the experiment, you dissolve the zinc core of a penny and leave the copper covering intact by putting four notches in

The Cu Later lab experiment is designed to allow you to practice lab skills in implementing and performing a series of reactions. Specifically, four types of chemical reactions will occur: oxidation/reduction; double replacement; single replacement; and decomposition. You will begin with a known amount of copper metal, which, after progressing through several steps, is reproduced. In this experiment you will observe and record the various changes such as heat, color changes, and production that occur. This procedure is used to observe some chemical reactions of copper and its compounds while also performing the lab appropriately as to retain the copper as much as

Then 8.0g of copper sulfate crystals were placed inside the beaker and the mass was recorded for the actual crystals. 50 mL of water was added to the beaker with the crystals. The ring stand was set up with the wire mesh on it and one partner should place the mixture in the beaker on it should be heated without letting the mixture boil. Stir the mixture and heat until the crystals are dissolved. While one partner does this, the other should obtain 1.5g of iron filings in a measuring cup and records the mass. Then the iron filings should be added small amounts at a time to the heated solution. Stir continuously until all the mixture is added to the beaker. Then it sat for 10 minutes and observations were recorded. Record the mass of a filter paper and set up a filtration apparatus with the filter paper in a funnel over an Erlenmeyer flask. Decant the liquid through the paper slowly trying not to allow any solid to get on the filter paper. Then with de-ionized water, rinse your solid in the beaker and let the solid settle then decant the liquid. Repeat the washing twice more and in the last time guide all the solid into the filter paper. Then place the filter paper on a watch glass and then into a warm oven to dry. After it is cool, record the mass of the watch glass, filter paper and solid. If there is not enough time to cool, you may have to do it the next

If you see a deep blue color add more zinc powder until there is no change in color of the solution in the test tube.

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

Weigh out the necessary grams of Copper Sulfate Pentahydrate. The 40-degree group weighed out 40 grams. (See Figure 1)

The concentration of Pb varies across the site, with the pattern observed noticeably similar to that seen with Sb. The highest concentrations of Pb are at sites close to the mine building, with a value of 57729 ppm at site 7. There is also a peak at site 11 of 38773 ppm in an area uncovered by vegetation. Uphill of the mine, Pb is present but in lower amounts.

In contrast, this lab report is an A-level lab report. It was well written with plenty of details and every section included. The abstract was descriptive it includes all the parts of a lab. The only thing that needs to be improved in the results section is the graph. The graph does not have its own key for the room temperature. Also, the caption for the graph was an incomplete sentence and was missing a quick summary of the major findings. Overall, this lab report was a high-level lab report with every part such as the biological significance in the discussion section, work cited, acknowledgment present. Unlike the other one if one was to repeat this lab they would have done it

N= 2.5x10^11/65.37 = 3824384274 moles of Zinc to get the moles of re required to create 250,000 tons of zinc metal, we times 3824384274 x 1.85 =707511097 moles of Zinc ore which then can calculate as m=nM 707511097 x (65.37+32.06) =6.89x10^11grams / 1x10^6= 689328.056 tons of ore =689,328 tons of Zinc ore required for 250,000 tons of Zinc metal, therefore the waste is calculated by 689,328 – 250,000=439328 tons wasted (439,328 tons) which are copper, lead and iron. This is 689,328/250,000= 2.757 tons of zinc ore per ton of zinc metal, 1000/2757 = 36.3% of zinc ore becomes zinc metal

0.5% of copper sulphate solution was added by drop at a time and and the test tube was shaked continuously.

At the end of the experiment when the lid was removed, it was found out that the blue colour of the copper (II) sulphate solution has faded away. It was turned to pale grey and there were some precipitates present. It was the zinc powder that was in excess to ensure that the copper (II) sulphate solution could react fully with the zinc powder.