Lab 3a

The white color implies that chlorine is within the mineral oil, thus did not react. Since chlorine did not react, it means that bromide isn’t a possible anion, leaving chlorine as the anion. In procedure 5, the unknown compound produced water on the watch glass indicating it could be a hydrate. The hydrate test was inconclusive because the number of waters of hydration shown in Table 5 was half way between being lithium chloride monohydrate and lithium chloride 2. The percent error, shown in Table 5, between the expected percent of water in lithium monohydrate and the accepted value, was high at 40% which meant that the unknown could not be properly identified as a hydrate. Repeating the hydrate test produced a similar percent which is shown in Table 7. The reason for these high percent errors is because lithium chloride and lithium monohydrate are both hygroscopic. In addition, Table 6 shows an increase in mass when unknown #42 was left outside, which suggest that the unknown compound is

The main purpose of the lab “Determination of the Formula of a Copper Oxide” was to determine the formula of a copper oxide. Specifically, this is a compound of copper combined with oxygen. This was to be done by heating the copper oxide thoroughly until all of the oxygen had been driven off. To accomplish this experiment, we first had to take and measure the mass of a specified color of copper oxide, ours being red. Then, we used a fischer burner to provide the heat needed for the split of copper oxide, in which our amount resided in a test tube. But, in order for the copper to not recombine with oxygen that could be found in the surrounding atmosphere of our lab, we also had to have a flow of methane gas into the test tube that fed into

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.

The purpose of this lab is to figure out the mass percentage of copper in a penny. Furthermore, by doing this lab we will practice using a spectrophotometer and review the names of equipment such as volumetric glassware, pipets, and volumetric flasks.

“What happens when you put acid on different minerals?” (Formoso, Acid Test: How to tell Minerals Apart , 2013)

Put approximately 9-10(g) copper ore into beaker. Use spatula to break up any large pieces. Next add 17ml H2SO4 (aq) (hydro sulfuric acid) to the beaker. Began mixing until all or most traces of blue dissipate; or the copper ore will no longer dissolve (should appear as a milky liquid). Next use pipette to and remove solution and divide solution into 2 individual test tubes then Place test tubes into centrifuge and run centrifuge for 1 minute. Remove from centrifuge machine Fill a cuvette with the clear solution from the test tube making sure not to disturb the sediment at the bottom. Note the solution should bluish in tint Final place the cuvette in the colorimeter. Then record data and calculate in results section.

3. Examine the luster of the minerals in Figure 1.2 (p. 4 lab book). Place the letter A, B, C, D, or E in

12) Find and extract the remaining copper wire out of the mixture using forceps and rinse the copper wire with distilled water so that the water goes into the plastic container.

Evidence and Analysis: When we heated the red copper powder for three two minute intervals, the product was black. The weight of the evaporating dish was weighed,

Refer to the reaction of iron nails with a copper solution assignment in Module 3, Section assignment 3.4 Part F of the Chemistry 11 course.

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:-

XIV. Record your observations of the dried, cooled copper metal and weigh the recovered copper.

The purpose of the experiment is to cycle solid copper through a series of five reactions. At different stages of the cycle, copper was present in different forms. First reaction involves reaction between the copper and nitric acid, and copper changed from elemental state to an aqueous. The second reaction converted the aqueous Cu2+ into the solid copper (2) hydroxide. In the third reaction Cu(OH)2 decomposed into copper 2 oxide and water when heated. When solid CuO reacted with sulfuric acid, the copper returned to solution as an ion (Cu2+). The cycle of reactions was completed with the reaction where elemental copper was regenerated by Zn and Cu

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.

In the known solution trial, the test tube’s solution turned white confirming the presence of lead while in the unknown solution trial the liquid stayed clear. Additionally, silver was confirmed present because when adding HCl to the solution in step 3 the solution smoked, created a white precipitate, and was acidic. These reactions all occurred during the trial with the known solution as well. Next, copper or iron were proved absent from the solution because in step four, no brown precipitate was formed and the solution maintained its clear form. This proved that there was no copper or iron because copper and iron were the only ions with a physical state of solid, and with the appearance of no precipitate it proves they were not in the solution.