your observations in your notebook. 3. After the sample has cooled‚ add a few drops of deionized water. What happens and what can be concluded? Part II: Formula of a Hydrate You and your partner will perform two trials of dehydration of a copper (II) sulfate hydrate. During the course of the experiment‚ handle the crucible and lid only with crucible tongs as shown here or as demonstrated by your instructor. Clean two crucibles with soap and water. Rinse the crucibles with distilled water and
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© UCLES 2012 9701/36/O/N/12 3 1 You are to determine the concentration of aqueous copper(II) sulfate by titration. The concentration of Cu2+ ions in a solution can be found by reaction with an excess of aqueous iodide ions to produce iodine. The amount of iodine formed can be found by titration with thiosulfate ions‚ S2O32–. For Examiner’s Use FB 1 is aqueous copper(II) sulfate‚ CuSO4. FB 2 is 0.100 mol dm–3 sodium thiosulfate‚ Na2S2O3. FB 3 is aqueous potassium iodide‚
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Calculations Mass percent of water in CuSO4·5H2O using experimental data: (mass of water lost / mass of hydrated salt) x 100 (0.658 / 2.009) x 100 = 32.75 % Mass percent of water in CuSO4·5H2O using theoretical data: (90 / 249) x 100 = 36.14 % Percent error using experimental and theoretical mass percentages: (experimental value – theoretical value / theoretical value) x 100 (32.75 – 36.14 / 36.14) x 100 = 9.38 % Average percent water in CuSO4·5H2O using experimental values: (trial 1 % water +
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collection and processing Qualitative observation Before * Blue solution of copper sulfate * Grey zinc powder During * Blue color solution changes to greyish black * Heat is given out‚ so the surroundings become hotter. After * Grey powder remains on the sides of the cup * Precipitate formed at the bottom of the cup List of chemicals and apparatus used Chemicals used Copper sulfate solution‚ 1 mol dm-3 25g of zinc powder Apparatus needed Pipette‚ 25ml
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FINAL PROJECT 1 Final Project Assignment Shawn Ovington XACC/280 Sheila Sullivan FINAL PROJECT 2 Keeping good records is a key in any good business and it helps companies find key areas where they feel they can improve. Coke and Pepsi are two large named soda distributers that have
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in thermochemistry. Explain each one of them by giving an appropriate example: (a) Standard enthalpy change (b) Exothermic process (c) Endothermic process Define and write an example of thermochemical equation for each of the following terms: (a) Enthalpy of formation (b) Enthalpy of combustion (c) Enthalpy of atomisation (d) Enthalpy of neutralisation (e) Enthalpy of hydration (f) Enthalpy of solution (dissolution) (g) Lattice energy Consider the following reaction: H2(g) + ½ O2(g)
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sources Project more suitable for students with a mathematical background 14 The amount of copper in brass Compare different methods for finding the concentration of copper(II) ions in solution. Could include redox titration‚ colorimetry‚ ion exchange followed by acid/base titration‚ gravimetric‚ use of an electrochemical cell. Starter page Chemistry Review Project page ‘The concentration of copper
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2014 Purpose: To determine the identity of an unknown hydrated salt calculating the percent water loss after heating and also to determine the empirical formula of magnesium oxide. Results: Table 1: Determination of the mass of waters of hydration of an unknown hydrated compound. Hydrated Compound code: C-14 Mass (g) Crucible + Lid 30.581g Crucible + Lid + Hydrated compound 31.590g Hydrated Compound 1.004g Crucible + Lid + contents (after 1st heating) 31.122g Crucible + Lid + contents
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(anion)[pic] X + Y (anion); where Y > X on activity series or Eo table. • Alkene/alkane reactions: – Cracking of pentane: ▪ pentane [pic] ethylene + propane ▪ C5H12 (g) [pic] C2H4 (g) + C3H8 (g) – Hydration of ethylene (the reverse can also happen known as de-hydration‚ where concentrated acid is used): ▪ ethylene + water [pic] ethanol ▪ C2H4 (g) + H2O (l) [pic] C2H5OH (l) – Hydrogenation of ethylene: ▪ ethylene + hydrogen [pic] ethane ▪ C2H4 (g) + H2
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the formula Ccal = -(ΔHwater * nLR) / ΔT (eq 1) where ΔHwater is the enthalpy change of water. This is equal to -55.81 kJ/mol. nLR is the number of moles of the limiting reactant‚ and ΔT is the change in temperature associated with the reaction. The Ccal obtained was later used to determine the experimental values of the enthalpy change of the reactions (ΔHrxn). Six other reactions were also used to determine its enthalpy change. The reactions are: Neutralization: a. Ammonia and hydrochloric
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