Introduction/Purpose: This report discusses an experiment done with copper metal. Several reactions were ran with it, which produced different copper compounds to in the end finally recover the original amount of copper. This experiment is important because it proved the Law of Conservation of Mass. The Law of Conservation of Mass states that mass is neither created nor destroyed. So after the last reaction is done there should be the same amount of copper as there was before you began. Material: Beaker Evaporation Dish Pipette Metal Copper Nitric Acid Litmus paper Sodium hydroxide Stirring rod Pure water Hot plate Beaker tongs Hydrochloric acid Aluminum wire Procedure: To begin the first procedure weigh your piece of copper …show more content…
The “Yields of Copper” chart show the different amounts of that were produced during the original experiment. The initial amount shows the amount that was used in procedure one . The final theoretical amount shows the amount of copper that the reaction for the fifth procedure should give you when using stoichiometry to find the amount of copper in that reaction. Conclusion: In conclusion, The results indicate that there was a yield greater than the initial amount. This could be caused by the rounding done when doing stoichiometry. Misinterpretations in the final experimental amount could be because of leftover aluminum wire. However, regardless of the yield being the greater amount, this experiment proves the Law of Conservation of mass. Appendix: This report discusses an experiment done with copper metal. Several reactions were run with it, which produced different copper compounds to in the end finally recover the original amount of copper. So after the last reaction is done there should be the same amount of copper as there was before you began. The results indicate that there was a yield greater than the initial amount. However, regardless of the yield being the greater amount, this experiment proves the Law of Conservation of
To calculate the percentage of Cu, we divided the final mass of the penny 0.09 and the initial mass of 2.47 and multiplied by 100. To calculate the percentage of Zn, we divided the final mass of the penny 2.38 and the initial mass of 2.47 and multiplied by 100. During the experiment the hydrochloric acid donated its hydrogen ions in the reaction and then the chloride ions reacted with the zinc ions in the solution. Thus, the zinc dissolved in the highly acidic solution which was caused by the high concentration of H2 ions. Hydrogen gas was generated during the reaction which was seen when bubbles were formed as the penny was dissolved into the beaker.
Then the mass of the copper metal and the percentage of Cu were obtained and compared throughout different groups and a mean and standard deviation was calculated for the
Conclusion: Compare Trial 1 and Trial 2. The Trial 1 change in mass are 12.5g, however Trial 2 changes in mass is 1.2g. The Trial 1 change in mass is more than Trial 2. And I think the Low of Conservation of Mass violated in the Trial 1 is can be exist. Because the Trial 1 actually the soda with vinegar have Chemical reactions occur and chemical
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
In this experiment, the evolution of the copper cycle was observed through a series of reactions. Four different copper compounds are formed through different reactions to inevitably lead to the recovery of Cu(s). This primary goal of this experiment was to study the Law of Conservation of Mass and perform 5 reactions on copper compounds. As Jenna Winterberg states in her book “Conservation of Mass,” the first part of this law is that mass or matter cannot be created. The second part of the law is that mass or matter cannot be destroyed .
The density of the penny was 4.68 g/cm3 before the experiment and 4.43 g/cm3 at the end of the experiment. The density of gold, though, is 19.3 g/cm3. Since the densities of the penny and the gold are different, the penny clearly did not change into another element. The gold color of the penny was a result of the flame that it was held above melting the zinc that it was coated in with the original bronze colored coating of the penny, creating an alloy with a shiny yellow color. Since neither of the pennies, silver colored or gold, changed densities throughout the experiment and each retained their own properties; the properties of copper; no new elements were
The volume stayed consistent because to decrease, the process needs activation energy. Once the activation energy was stored, the compost started to decrease almost linearly. The decreasing was due to worms eating the compost and disposing some of it as dirt, disposing some into the air (CO2), and using other part of the compost like the H’s as energy. This was due to cellular respiration; the worms used the compost for glucose, and due to homeostasis unused molecules were released through respiration.. The compost stayed constant again at the end of the experiment because worms started to die, and weren’t able reduce any more
To determine the rate of reaction there are many method to be used for example, measuring the mass after the product has been added and measuring the difference in mass on the duration of a digital scale. Another method, which will be used in this experiment is using a gas syringe to measure the volume of the gas which has been produced. The cylinder inside, will be pushed out to show a quantitative presentation of the volume produced by the reaction. Hypothesis
Copper Cycle Lab Report Ameerah Alajmi Abstract: A specific amount of Copper will undergo several chemical reactions and then recovered as a solid copper. A and percent recovery will be calculated and sources of loss or gain will be determined. The percent recovery for this experiment was 20.46%.
3. In this experiment, the percent yield was 90%. This number implies that there was little error in this experiment. However, this result could have been caused by certain external factors.
Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and
Lab Report Experiment 6 Rates of Chemical Reactions By Nikhola Mirashirova Lab Partner: Dina Abetova Section 3, Saturday October 31, 2015 Introduction Rate reaction is the measure of the change in concentration of the reactants or the change in concentration of the products per unit time.1,2 Rate law for this experiment: Rate = k(I-)m(BrO3-)n(H+)p There are several factors which affect the rate of reaction: catalyst, reactant concentration, and temperature.1,2 A catalyst is a substance that changes, increases or decreases, the rate of a chemical reaction but is not being used up during the reaction.3 It provides an alternative way, so that the rate of reaction changes.4 Catalyst, which is used in this experiment, is (NH4)2MoO (0.5 M).
As soon as the wire was submerged into the solution, the aluminum atoms and the copper (II) ions underwent a reduction-oxidation (redox) reaction, meaning aluminum was oxidized and donated its electrons to the copper ions, which were reduced. As a result, solid copper began to form on the surface of the aluminum wire, giving the wire a brown-orange color that resembled rust. The wire had to be regularly shaken in order to remove the solid copper particles and thereby expose more of the aluminum wire to react with the surrounding solution. As the reaction progressed, the liquid copper chloride solution slowly began to lose its color and turn clear. This was a chemical reaction, as seen by the bubbles formed with the wire was added, meaning gas was released when aluminum was oxidized and copper was reduced, but it also gave rise to physical changes, such as the change in color of the solution from blue-green to rusty orange to clear.
The final product weight for percent yield was only the solid E product, which missed one half of the final product produce. If both products were weight, the percent yield would have been larger that it was. Instead of 22.33%, it could have been 44.66%. To prove that both products were obtained, but only one of the two products was analyze, a TLC plate of the DCM layer, that contains both products, and of the final product, was obtain.
If only one reactant is increased, then the chemical reaction will only produce a certain amount of products after the limiting reagent is used up, and in this experiment, the most mass the reaction could produce was 0.4 grams. Although we kept adding calcium chloride, not adding sodium hydroxide in the same proportions will not yield more product, which is the main goal in conducting this lab. We should have seen a plateau at 0.4 grams to show that the limiting reagent inhibited further Ca(OH)2 production, but we made several mistakes in our experiment, which made the data unusable to conclude. Once again, the data is polluted, so these number are not accurate, but it is the data our group has to work with. The theoretical yield should have been more than the actual yield, and the percentages should have been less than 100.