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File Size 746 KB
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Qualitative and Quantitative Data Copper Quantitative Data Initial Mass of Copper Mass of Evaporating Dish Mass of Evaporating Dish and Copper Mass of Recovered Copper 2.004 g 50.165 g 57.01 g 6.845
g Qualitative Data from Reactions Reaction Cu + HNO 3 Cu(NO3) 2 + NaOH Cu(OH)2 copper cycle lab report answers CuO + H2SO4 CuSO4 + Zn Zn + H2SO4 Observations Exothermic and produced nitrogen dioxide gas Exothermic, precipitate formed, solution became thicker,
and gas was produced. Black Copper Oxide precipitate formed and water formed. Black precipitate is denser than water and sinks to the bottom of the beaker. Copper Sulfate and water formed. Copper Sulfate is a blue precipitate, copper cycle lab equations but since it is soluble in water, it dissolves and the mixture is turned a bright blue color. Zinc sulfate is formed and is aqueous. Hydrogen gas is also formed and released. Solid copper is found on the bottom of the beaker. Net Ionic Equations 1. Cu (s) + HNO3 (aq) NIE: Cu(s) + 4H+(aq) + 2NO3-(aq)---> Cu2+(aq) +2NO2(g) + 2H2O(l) 2. Cu(NO3)2 (aq) + NaOH (aq) NIE: Cu2+(s) + 2OH-(s) ---> Cu(OH)2O(s) 3. copper cycle lab balanced equations Cu(OH)2 (s) decomposes NIE: Cu(OH)2(s)---> CuO(s) + H2O(l) 4. CuO (s) + H2SO4 (aq) NIE: CuO(s) + 2H+(aq)---> Cu2+(aq) + H2O(l) 5. CuSO4 (aq) + Zn(s) NIE: Cu2+(aq) + Zn(s)---> Cu(s) + Zn2+(aq) Calculations: Final Mass of Copper Mass of evaporating dish and copper - mass of evaporating dish = mass of copper57.01 g - 50.165 g = 6.845 g Final Moles of Copper Final mass of copper X (moles of copper)/(molar mass of copper) = Final moles of copper6.845 g Cu X ( 1 mole Cu) / ( 63.564 g Cu) = 0.1077 moles Cu Initial Moles of Copper Initial mass of copper X (moles of copper) / (molar mass of copper) = Initial moles of copper2.004g Cu X ( 1 mole Cu)/ (63.564g Cu)= 0.0315 moles Cu Percent Yield Percent Yield = (moles of copper recovered) / (initial moles of copper) X 100Percent Yield = 0.1077 moles Cu / 0.0315 moles Cu X 100 = 341.9 % Conclusions The initial mass of copper used in the experiment was 2.004 grams, and the initial moles of copper was 0.0315. Due to the Law of Conservation of Mass, one would predict that after any number of chemical reactions and phase changes, the final mass and number of moles of copper would remain the same as the initial amounts. After th
a discussion of the data with a conclusion. This particular lab report shows my ability to work with quantitative data, and analyze the calculations and measurements from the lab. It also shows my ability to recognize error
and discuss how the error affects the outcome of the lab. Conservation Of copper cycle lab materials Mass: A Cycle of Copper Reactions November 4, 2014 Purpose The purpose of this experiment is to test the Law of Conversation
of Mass. Copper will undergo many types of reactions and go through its whole cycle, then return to solid copper to be weighed. The percent recovery of copper in this experiment was 90.8%. Introduction The scientific http://alexgoldapchemlabs.weebly.com/copper-lab law that was tested in this experiment is called the Law of Conservation of Mass. The Law of Conservation on Mass states that all matter is conserved; no matter can be created or destroyed. Rather, matter is shifted and converted into different states. To test this law, copper can be put through a cycle to test if the same mass of copper is present at the end of the cycle. This copper cycle consists https://sarahjacksonumd.wordpress.com/chemistry-lab-reports/ of six different reactions and four different types of reactions. The four types of reactions are oxidation/reduction, precipitation, decomposition, and acid/base neutralization. Oxidation/reduction reactions involve a change in oxidation number and a transfer of electrons. Precipitation reactions yield a solid product that is insoluble. Decomposition reactions yield a product that is a broken down form of the reactant, such as AB à A + B. Acid/base neutralization reactions involve the creation of water and a salt. Solid copper is the first reactant in this experiment. After the six steps of the experiment, the same mass of solid copper should be recovered, based on the Law of Conservation of Mass. Data & Results Copper was put through a series of several reactions, until solid copper was the last remaining product. The initial mass of copper was recorded, and then compared with the mass of recovered copper at the end of the experiment. Table 1: Measurements and calculations of mass, and calculation of percent recovery of copper after the experiment was completed. Initial mass of copper 0.500 g Mass of evaporating dish 60.614 g Mass of evaporating dish and copper 61.068 g Mass of recovered copper 0.454 g Percent recovery 90.8% Calculations: mass of recovered copper equals dish and copper minus dish. 61.068 g - 60.614 g = 0.454 g Percent
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copper cycle experiment sources of error
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Compatible with Windows XP, Vista, Windows 7 (32 and 64 bit), Windows 8 & 8.1 (32 and 64 bit), Windows 10 (32/64 bit).