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Grade 8 explain chemical reactions
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The experiment we did was Copper Cycle. We reverted the copper to its elemental form after a chain of reactions. We performed a series of reactions, starting with copper metal and nitric acid to form copper (ii) nitrate. Then we reacted copper with sodium hydroxide, sulfuric acid, nitric acid and zinc to form precipitates. In conclusion our percent recovery was 40.38%. Introduction: The purpose of this lab was to to cycle solid copper through a series of chemical forms and return it to its original form. A specific quantity of copper undergo many types of reactions and went through its whole cycle, then returned to its solid copper to be weighted. We observed 5 chemical reactions involving copper which are: Redox reaction (which includes all chemical reactions in which atoms have their oxidation state changed), double displacement reaction, precipitation reaction, decomposition reaction, and single displacement reaction. 4HNO3(aq) + Cu(s) --> Cu (NO3)2(aq) + 2H2O (l) + 2NO2(g) Oxidation reduction reaction Cu (NO3)2(aq) + 2 NaOH (aq) --> Cu (OH)2(s) + 2 NaNO3(aq) Precipitation Reaction Cu (OH)2(s) + heat --> CuO (s) + H2O (l) Decomposition reaction CuO (s) + H2SO4(aq) --> CuSO4(aq) + H2O (l) double displacement reaction CuSO4(aq) + Zn (s) --> ZnSO4(aq) + Cu (s) Redox reaction
The citric acid cycle is an amphibolic pathway. It utilises both anabolic and catabolic reactions; the first reaction of the cycle, in which oxaloacetate (a four carbon compound) condenses with acetate (a two carbon compound) to form citrate (a six carbon compound) is typically anabolic. The production of the isomeric isocitrate is simply intramolecular rearrangement. The subsequent two reactions are typically catabolic, producing succinate (a four carbon compound), which is then oxidised, forming fumarate (a four carbon compound). Water addition produces malate and then oxidised for regeneration of oxaloacetate. Thus the cycle can be seen to exhibit both anabolic and catabolic processes to form its intermediates.
To complete this lab several chemicals must be measured and transferred to test tubes. First 5.0 mL of 0.200 M Fe(NO3)3 must be diluted to a total volume of 50 mL in a flask. Next 0.0020 M SCN–. This solution is then added to 4 test tubes in 1 mm increments. Each test tube is then put in to
...han 10% out from any group of results would be considered inaccurate and would be repeated. The uncertainties in my results after any repeated results were sufficiently small enough to keep my results reliable.
The copper ions are transferred from the water where they are of a high concentr... ... middle of paper ... ... is likely to be placed and a thorough environmental impact assessment carried out to ensure that the processes do not cause undue environmental damageι. Finally governmental permission must be obtained before commercial activity can take placeι. References α - Article 1 from examination pack: Mining with microbes, John Merson. β - How hydrometallurgy and the SX/EW process made copper the "green" metal, William Dresher. γ - Article 2 from examination pack: Extracting copper from leaching solutions.
In the second part of phase 1 which was steps 5-8 4 different pieces of clean zinc were placed in 4 different acids. The acids were Hydrochloric ...
For example, if it is found mixed in an ore of copper, manufacturers must use a technique called smelting to separate the mineral from the element. The smelting oxidizes all the elements present except for silver and gold. Then, the manufacturers use the processes of the Moebius and Thum Balbach electrorefining that result in refining 99.99% silver.6 If found mixed in an ore of lead, the Parkes process is used to separate the silver. People add zinc to the mixture, which reacts and combines with the silver. The silver is then refined through the processes of Moebius or Thum Balbach, as well as the Wohlwill process to refine it from gold.6 When the silver is found in a zinc ore, however, the zinc concentrates are roasted and then put through the process of slag fuming, which makes the silver dissolve. After, it goes through the same lead refining process
An atom, by definition, is the smallest part of any substance. The atom has three main components that make it up: protons, neutrons, and electrons. The protons and neutrons are within the nucleus in the center of the atom. The electrons revolve around the nucleus in many orbitals. These orbitals consist of many different shapes, including circular, spiral, and many others. Protons are positively charged and electrons are negatively charged. Protons and electrons both have charge of equal magnitude (i.e. 1.602x10-19 coulombs). Neutrons have a neutral charge, and they, along with protons, are the majority of mass in an atom. Electron mass, though, is negligible. When an atom has a neutral charge, it is stable.
The purpose of this experiment is to use our knowledge from previous experiments to determine the theoretical, actual, and percent yields of the lead chromate from the reaction of solutions of potassium chromate and lead nitrate (Lab Guide pg. 83).
Copper Oxide + Carbon Dioxide (CuCO3 = CuO + CO2) The reactivity series determines how fast this reaction occurs. The reactivity series is the order of metals in the periodic table. The most reactive metals are placed at the top of the reactivity series.
Chemistry Aim- To determine the enthalpy change for the reaction of copper sulphate and zinc. Materials Required- Calorimeter Glass Thermometer Weighing Machine Digital Stop Watch Measuring Cylinder Cuso4. 5H2o Zinc Metal Powder Distilled Water.
The Electrolysis of Copper Sulphate Aim Analyse and evaluate the quantity of Copper (Cu) metal deposited during the electrolysis of Copper Sulphate solution (CuSo4) using Copper electrodes, when certain variables were changed. Results Voltage across Concentration of solution electrode 0.5M 1.0M 2.0M 2 5.0 10.6 19.5 4 10.5 19.8 40.3 6 14.3 26.0 60.2 8 15.2 40.4 80.3 10 15.0 40.2 99.6 12 15.1 40.0 117.0 Analysing/Conclusion The input variables in this experiment are; concentration of the solution and the voltage across the electrodes. The outcome is the amount of copper gained (measured in grams) at the electrodes. By analyzing the graph, we can see the rapid increase of weight gained for the 2.0 molar concentration as the gradient is steeper.
== == I completed a table to show my results, here is the table: Table 1. Results of different changes of substances Part A Copper (II) Sulfate and Water Reactant description Water (reactant): Color: Colorless Transparency:
Possible sources of error in this experiment include the inaccuracy of measurements, as correct measurements are vital for the experiment.
To investigate the temperature change in a displacement reaction between Copper Sulphate Solution and Zinc Powder
Aluminum is an element in the boron group with a symbol of Al, and an atomic number of 13. Aluminum is a very soft metal when pure but becomes strong and hard when alloyed, a malleable metal with a silvery gray color. Aluminum is a very reactive element so it is found in nature combined with other elements. Aluminum resists corrosion by the formation of a self-protecting oxide coating. Aluminum is the third most abundant element in the Earth’s crust, following oxygen and silicon. It makes up approximately 8% by weight of the Earth’s surface. Although this is evident, it is also apparent that aluminum is never found by itself in nature. All of the earth’s aluminum has combined with other elements to form compounds and in order to create new aluminum products; it has to be taken out of that specific compound. Aluminum does not rust like other elements, therefore it always remains strong and shiny, which means reused aluminum is almost identical to a brand new piece of metal. An electrochemical process creates aluminum. An electrochemical process is “the direct process end use in which electricity is used to cause a chemical transformation” ( E.I.A. Government). Major uses of electrochemical processes occur in the aluminum industry in which alumina is reduced to molten aluminum metal and oxygen, where than the aluminum can be used into making several different materials. Electrochemical processes, although very useful, can have serious environmental consequences. To help reduce the consequences that the production of aluminum creates, the idea of aluminum recycling comes into play.