Cufee Industry Analysis

In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution which was 1M, the same clean equipment was used to make up the standard solution as used to make sodium carbonate. However there was one difference and that was that the hot distilled water was used to dissolve the copper sulphate crystals. There had to be enough hot water in order to dissolve the crystals into the beaker and then add cold distilled water to cool the solution.

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

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.

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

During the heating period, a noticeable change took place in the sugar test tube – it began to caramelize, melting into a golden brown color, then finally a dark brownish/black hue; it remained constant at that color. The copper sulfate began losing color when applied to the heat, turning from a bright blue to white and remained white after heating. Once cooled, 2-3 drops of water were added to each tube; the sugar remained the same, while the copper sulfate immediately bubbled and transformed from white back to its original blue hue. Next 1-3 grams of the hydrated copper sulfate were added to a crucible, which was weighed prior to adding the sample, then heated gently with a Bunsen burner. Once the salt stopped changing color, it was heated for an additional 5 minutes, then the total mass was measured. Finally, a pea-sized amount of Epsom Salt was added to a test tube and heated for 1 minute without the tube becoming red

The first reaction involves pyrite rock reacting with oxygen (air) and water to produce dissolved ferrous iron, sulfate, and acidity. The second reaction oxidizes the dissolved ferrous iron in acidic conditions and produces ferric iron and water. The third reaction involves the hydrolysis of the ferric iron to form ferric hydroxide and more acid. The ferric hydroxide is the orangey-red colored solid you see in the water (Juniata College).

I started with elemental copper metal and then reactions occur step by step as follows:

Purpose: The purpose of this experiment was to observe the many physical and chemical properties of copper as it undergoes a series of chemical reactions. Throughout this process, one would also need to acknowledge that even though the law of conservation of matter/mass suggests that one should expect to recover the same amount of copper as one started with, inevitable sources of error alter the results and produce different outcomes. The possible sources of error that led to a gain or loss in copper are demonstrated in the calculation of percent yield (percent yield= (actual yield/theoretical yield) x 100.

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:-

Copper is usually extracted from sulphide ores such as Chalcopyrite. Since these ores contain low amounts of copper, they have to be concentrated through froth flotation before refining. The sulphate ore is first mined underground, and then bought to the surface to be crushed. Pine oil is then applied to the crushed copper ores, binding copper compounds together, but not the rocky material remaining. The ore is then put in a tub of water through the feed consisting of a foaming agent. Air is then released bit by bit in the agitator, causing bubbles to form. The water repellent copper compounds are picked up with the bubbles, making them float, letting the excess froth flow over the sides, creating concentrated copper in the concentrate launder.

These chemicals include sulfuric acid, water, zinc, and polysiloxane. The chemicals break down he scrap copper into a liquid mixture known as copper sulfate (CuSO4). The copper sulfate is then poured over a drum, and electrified, this adheres the foil to the drum, which is then peeled off as foil. Because of the chemical intense process, entry is very hard. The process requires very precise and technical equipment that is very costly. Oak-Mitsui, the leading company in the market, has a $200 million production plant to produce the foil in a 20 million pounds or about $105 million market size. Another barrier to entry is the transportation cost, which tends to be a major cost for the companies. Owning or outsourcing transportation is an expensive cost that most companies across all markets face, and copper foil is certainly a market where transportation is a factor. Because there are few sites of production or importation, the foil needs to be shipped to the consumers, which are located across all of North America. This leads to transportation being a costly factor in the production of copper foil. Copper foil has constant returns to scale. When all of the inputs are increased, the output is increased proportionally. This is due to the fact that there is no loss or setbacks on the inputs during production. This also means that the production function is linear, like Q= 2K+5L (however with many more variables).

When the zinc was added to the copper (II) sulfate solution, the solution started to bubble. As the solution was stirred, it turned a cloudy blue. Small flecks of a brown solid were visible. As the solution became colorless, the brown solid settled to the bottom of the beaker. The solid formed was copper in its elemental state. The color faded from the solution as the copper ions slowly formed into solid copper. The copper was poured into a funnel with filter paper and washed three times with 25 mL

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.

Iron disulfide (FeS2) is the chemical formula for the mineral pyrite. This mineral has long been described and prevalent in modern and ancient history. Pyrite’s name originates from the Greek for fire, which is “pyr”. The Roman author Pliny the Elder described a stone which is thought to be pyrite. He described a stone used for grindstone, which would readily fire sparks or sulfur. He also commented on the heft, its resemblance to brass or copper, and its porosity. A Greek physician called pyrite an ore of copper, due to the brassy look, but also commented on the sparks the mineral gave. Many of the early descriptions of pyrite included similar easily confused minerals such as chalcopyrite, marcasite, and pyrrhotite. (Dana, 1982)