Identifying reaction types and calculating percent yield after multiple chemical reactions of copper metal *Ashlyn Langner and Katherine Rumfield Chemistry 111 Section 524 Introduction A topic of interest in science is the evaluation of the law of conservation of matter through different types of chemical reactions and determining the percent yield resulting from these reactions. This law states that after a chemical reaction, matter should neither be created nor destroyed. This experiment allows for this law to be tested and for the determination of different errors that may occur during chemical reactions similar to this one. The magnitude of these errors can be found through the percent yield calculated by using the original mass of …show more content…
This is because the copper in the reactants is bonded to nitrate and the sodium is bonded to the hydroxide, then in the products the copper is bonded to the hydroxide and the sodium is bonded to the nitrate. This can also be classified as a precipitation reaction because there was a solid formed from two aqueous solutions. During this step in the cycle, adding NaOH to the copper nitrate caused the formation of small, flaky pieces which quickly disappeared. These pieces can be assumed to be the copper hydroxide in the products as it is the only solid in solution. After adding 100 drops of NaOH to the solution the mixture changed color from a transparent blue to a creamy, thick blue. At 120 drops of NaOH the mixture turned very bright blue and the drop of the solution on the red litmus paper turned the paper blue as well, indicating the reaction was …show more content…
After adding 0.300 g of zinc to the copper sulfate, the zinc immediately fell to the bottom of the beaker and turned black. The mixture became cloudy, bubbly, and dark as a small amount of smoke from the reaction became evident. The solution continued to become darker and never became colorless, as expected in the directions. Once stirring stopped and solution was able to settle, there was a clear separation between the solid and the liquid left in this solution. Anther identification of the single-replacement reaction, as copper in the solid form was
The purpose of the lab is to acquire the percent composition of zinc and copper. The procedure included obtaining a post 1983 penny and washing it with soap and water. Using a triangular file, we made an X on the penny. Then, we cleaned the top and bottom of the penny with steel wool until it was shiny. We rinsed the penny in acetone and dried it with paper towel.
A spectroscopy curve was produced of the acid and the absorbance of the unknown mineral could be obtained in order to find what that unknown copper is. Through these methods there is not preferred method when it comes to finding the percentage of an unknown substance, but which is more effective in accurately depicting what that unknown substance is. Standard deviation plays a major part in this experiment to help balance out and find the mean of the unknown substance to help constitute what it is. Through this the difference between smelting and roasting is that one produces a metal from its ore and the other drices off the carbon to obtain an
Evidence of such loss of material was displayed as a white film on the end of the tongs which held the metal. If the reaction was conducted in a more controlled environment, then maybe the theoretical results would be
The possibilities for the identity of the metal include copper and iron (1). The possible charges for copper are 1+ and 2+ (2). The possible charged of iron are 2+ and 3+ (2). By using stoichiometry, it can be concluded that there are only four possible equations: CuNO3 (aq) + NaOH (aq) > NaNO3 (aq) + CuOH
Copper/ Red Stuff/ Chemical Reaction The purpose of this experiment was to determine what the red stuff that was produced was. We put aluminum foil in a test tube filled with 100 milliliters of copper chloride. During the experiment, I observed that the aluminum foil was breaking away, the aluminum foil that was breaking away was turning into red stuff. After a while, the once light blue copper chloride was turning into a dull gray, almost clear.
The products were aluminum chloride and copper. A change in properties demonstrates that a chemical reaction occurred. One property that changed was the colors. Initially the aluminum foil was a shiny silver, and the copper chloride was a green-blue liquid. After we placed the aluminum into the copper chloride solution, the liquid clouded up a lot and turned to a light grayish hue.
To better understand this law, Cu(s) was transformed with different reactions only to return back to Cu s). The initial and final mass of Cu(s) was recorded to give the percent recovery of copper product at
When the substance reacted with the solution it turned from its initial color yellow/brown to its final color lilac/violet. The experiment went by easily flowing nicely, although one or two things went wrong, none had any effect on the experiment. It is very important to know what foods are composed of because, knowing what is inside our food is essential for our health. We need to be aware of what things we are consuming and what we should be consuming for our bodies to function properly.
The purpose of this lab is to identify the seven numbered solutions through chemical reactions. It was done by mixing the numbered solutions of known names but unknown number of distribution with each other and analyzing the chemical reactions. Research shows that NiCl2 is the green liquid. NiCl2 will not react with anything except with AgNO3 and Na2CO3, so the first step will be mixing all solutions with NiCl2 until those two chemicals are found. Na2CO3 will create bubbles (CO2) while AgNO3 does not when mixed with the other chemicals.
In beaker with the formed CuSO4 from Reaction 4, a piece of aluminum wire, which was bent into a circular shape, was placed in the beaker, and completely submerged in the solution. To this beaker a small stir bar was added along with 5 drops of 6 M HCl to start the reaction. This beaker was place onto the hot plate, covered with a watch glass, and the stir setting on the hot plate was turned on so that the stir bar moved the piece of aluminum wire around and hit it repeatedly. The wire began to have copper form on it and the stir bar hitting the wire would knock off the formed copper. Before the beginning of the next step the reaction had to be completed.
These color changes indicate a chemical change, which show that a reaction had occurred. In the first step when o-vanillin and p-toludine, imine was formed. The color change from green to orange suggests that imine appears as orange colored. In the second step, the addition of sodium borohydride reduced the imine into another derivative, which was yellowish lime color. The solution turned clear when acids and anhydrides was added, which indicated the precipitate were dissolved.
The most important aspect of determining the results is the timing. The timing will be used with a stopwatch, and will be timed from the moment that all the solution have been combined, and will end at the point that the solution has completely finished changing colors. In order to add the solution, and start the timer at the same time, I will need a second person to time while I combine the solutions together. In order to maintain similar results, I will also need to keep the same person keeping track as they will start and end the timer at the same time when they see fit in all the reactions. Procedure Reaction 1 Solution A (in a 100 mL graduated cylinder) 10 mL of 2.0M of sulphuric acid 10 mL of 3% hydrogen peroxide 80 mL water Solution B (in a 100mL graduated cylinder)
+ H2O (g) Reaction 4: when a sulphuric acid is added to the solution that contains copper (II) oxide, a double displacement reaction will occur. the copper (II) oxide will react with the sulphuric acid producing copper (II) sulfate and water. The copper and hydrogen gas replace each other. Balanced Chemical Equation: CuO (s) + H2SO4 (aq) —> CuSO4 (aq) + H2O (l) Reaction 5: when zinc is added to the copper (II) sulfate solution, a single displacement reaction will occur.
The objectives of this experiment were to use knowledge of chemical formulas and chemical nomenclature to experimentally determine the empirical formula of copper chloride. Common laboratory techniques were used to conduct a reaction between copper chloride and solid aluminum in order to get rid of the water of hydration. The amount of water of hydration in the sample of copper chloride hydrate was calculated by measuring the mass before and after heating the sample. Afterwards, an oxidation-reduction reaction was conducted, resulting in elemental copper.
Data Table 2: Table showing the average temperature (oC) (±0.5oC)per increment for the five metals reactions with Copper II Sulphate: Time (s) (±0.01s) Temperature (oC) (±0.5oC) Copper II (Cu) Manganese (Mn) Iron (Fe) Zinc (Zn)