In Reaction 1‚ the mass of the pre-cut copper wire was measured with watch glass on the analytical balance‚ the mass was recorded using as many significant figures as possible on Table 2. The copper wire was bended into a circle and laid flat on the bottom of the 250 mL beaker. Inside the fume hood‚ 4mL 16M of HNO3 was added into the 250mL beaker that contained the copper wire. The copper wire was completely dissolved by swirling the beaker. The observation was recorded in Table 3. For Reaction 2
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Introduction: Copper has played a vital role in past civilizations and continues to do so today due to its many properties as a metal. Although advantageous in today’s economy and also in human bodies‚ high concentrations of copper can prove toxic to our health and even pollutant to the environment. By altering the element through a number of chemical reactions including redox‚ metathesis‚ decomposition‚ and single replacement reactions‚ the cycle will be complete once solid copper is recovered.
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Determining the enthalpy change for the thermal decomposition of potassium hydrogen carbonate into potassium carbonate. Controlled Variables: 1. Volume of HCl ± 0.5 cm3 (± 2%) 2. Concentration of HCl‚ 3. Same mass of K2CO3 and KHCO3 within specified ranges of 2.5 – 3.0g and 3.25 – 3.75g respectively 4. Same calorimeter used i.e. polystyrene cup is used in this experiment 5. Same thermometer will be used ± 0.10K 6. Same source of K2CO3‚ KHCO3 and HCl Raw Data Results: The raw
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Measuring the Enthalpy change of combustion Abstract This simple experiment is carried out to show the difference in the enthalpy change of combustion between two fuels‚ hexane and methanol. These fuels are individually weighed before and after used as heat source to heat water in a calorimeter. The result is used to find out amount of heat transferred by the fuel‚ amount of fuel used and the enthalpy change of combustion. Introduction Enthalpy change of combustion is the enthalpy change when a substance
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Oxidation and Reduction Reactions: The Reactions of Copper Data: Part I: Preparing a solution of copper (II) nitrate Initial mass of copper wire: .520g Mass of copper wire after vigorously scouring: .518g Observations of Copper (II) ribbon mixed with HNO3: Solution turned green. Thick brown gas formed. Copper (II) bubbled vigorously. Cu (II) dissolved‚ solution appeared green/blue. After the addition of H2O a blue crusty precipitate formed. Part II: Synthesis of solid copper (II) hydroxide
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time limit of 600 seconds for a reaction between copper (II) sulfate (CuSO_4) and zinc(Zn) using a temperature probe. Time/ s (± 1 s) Temperature / °C (± 0.05 °C) 0 27.9 30 25.9 60 25.9 90 25.8 120 25.8 150 48.7 180 57.6 210 61.1 240 62.7 270 63.5 300 62.8 330 61.3 360 59.3 390 58.9 420 57.7 450 56.5 480 55.2 510 54.2 540 52.6 570 51.9 600 51.1 Qualitative observations:- Table 2: table depicting the qualitative observations observed during the reaction between Copper (II) sulfate solutions (CuSO_4)
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primary objective of this lab is to be able to determine the specific heat of a reaction by using a calorimeter. A calorimeter is a device used to determine the specific heat of chemical reaction or a physical change. The specific heat a reactions is used to refer to the amount of heat that is lost or gained when one gram of a particular substance increases or decreases by one degree Celsius. When a chemical reaction occurs in an open container most of the energy gained or lost is in the form of
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Enhtalpy change - Hess’ law Experiment #7 Date performed: March 4‚ 2014 Presented by: Sam Tabah(I.D.#1402433) & Giuliano Amato(I.D.#1328425) General Chemistry 202 Nya-05 (00006) Vanier college Part A. Objective: The objective of this lab was to determine the standard heat formation (∆H°F) of MgO‚ using a calorimeter and determining the enthalpy of two reactions. Applying Hess’ law we were able to determine the standard heat formation of MgO. Introduction
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DETERMINATION OF ENTHALPY CHANGE OF NEUTRALIZATION IA Criteria Assessed: DCP CE MS Introduction When an alkali neutralizes an acid‚ a salt and water are formed. Aqueous hydrogen ions (H+(aq)) from the acid react with the hydroxide ions (OH- (aq)) from alkali‚ forming water. The identity of salt will depend on the nature of the acid and alkali used. H+(aq) + OH- (aq) → H2O(L) The combination of H+ and OH- ions in this way releases energy. In this practical‚ the enthalpy changes accompanying
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Thermochemistry: An Ice Calorimeter Determination of Reaction Enthalpy D. F. Nachman 6/23/2010 Abstract: An ice calorimeter was used to study the reaction of magnesium metal and 1.00M sulfuric acid solution: Mg(s) + H2SO4(aq) →MgSO4(aq) + H2(g). We found the experimental molar enthalpy of reaction to be ΔH = –355 ± 17 kJ/mol at 0°C‚ 24% lower than the textbook value of ΔH° = –466.9 kJ/mol‚ reported at 25°C. Introduction Whether a chemical reaction occurs spontaneously or is driven by an outside force
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