Lab report 4 - Lab 04: Get Charged Dr.O PDF

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Lab 04: Get Charged Dr.O...

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Chancey Turner CHEM 1315-038

Lab 04: Get Charged Observations: In this lab, my partner and I watched the chemical reactions involved with changes in hydration. We were able to notice most chemical reactions by seeing a change in color. For part one of this experiment, we heated 1.511g of the originally blue copper (II) sulfate pentahydrate until it lost all color. Once it turned a greyish white, we let it cool and weighed it again. It weighed 0.977g after being heated to remove all water from the copper. It took approximately 5 minutes of constant heat to get the color change we were looking for. During part two, we measured the temperature of 15mL of D.I. water in a test tube which was 21.5 degrees Celsius. Once the temperature stabilized, we began recording the temperature at 2 second intervals as seen in figure 1 while we added in the copper. For part three, we obtained 1.001g of copper chloride hydrate. We then heated the compound by moving the Bunsen burner back and forth underneath it slowly. It turned brown and we then allowed it to cool before we created a solution of the copper chloride. Once we did that, we generated elemental copper, cleaned the copper using a Büchner funnel, and dried it in the oven. After the copper was dried, we weighed it, it weighed 0.099g, we put it back in the oven for ten minutes then weighed it again and it weighed 0.102g.

Run 1 Temperature °C 45 40 35

Temperature

30 25 20 15 10 5 0 5 5. 11.5 17.5 23.5 29.5 35.5 41.5 47.5 53.5 59.5 65.5 71.5 77.5 83.5 89.5 95.5 01.5 07.5 1 1

Figure 1 represents part 2 of the experiment where the temperature was measured while we added the copper to the water in the test tube. Chemical name Amount 6M HCl 20 mL Copper (II) sulfate 1.511g pentahydrate Figure 1.1 Chemicals utilized table

Waste Type Aqueous Aqueous (dissolved)

Data Analysis: 1. The moles of copper was 0.002 moles. 2. The mass of chlorine was 1.001g, which makes the moles of chlorine 0.028 mol Cl. 3. The experimental molar ratio of Cu:Cl is 4. Aluminum wire, HCl, copper, and water were used for the reaction. The evidence was the formation of bubbles and heat production. The reaction occurred between the HCl and the aluminum wire to form copper 5. The increase of mass in the aluminum wire would indicate more copper production. A decrease would indicate less copper being produced. Discussion: 1. With as many steps as there is in this experiment, many of them could be error prone. If the steps weren’t properly completed, then it could cause the formula mass to be to heavy or to light because the substance could be used up too much or not enough. This could cause an incorrect reaction or it to not be completed. 2. The copper used in this experiment is the most common than the others we have worked with in my opinion. Copper is mostly used in electric wiring.1 The copper created in this experiment is made of something as common as aluminum wire which supports my idea of it being the most common. 3. Copper ions have two charges because they are an exception to the Aufbau principle. Because it takes more energy to remove the second electron from copper than it does to remove the first, it can have more than one common charge. Reference: 1. John Emsley, Nature’s Building Blocks: An A-Z Guide to the Elements, Oxford University Press, New York, 2nd Edition, 2011...