in chemical reactions are described‚ and exothermic reactions and endothermic reactions are discussed in terms of bond energies - including calculations of energy transfers for GCSE/IGCSE/O Level and basic stuff for GCE Advanced Level AS students. Methods of obtained vales for energy changes in chemical reactions are described and how to do the calculations based on calorimeter experiment results. Also discussed are activation energies‚ reaction profiles‚ catalysts. If you are an A Level student
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........................................................................ 15 Project C • Properties of a Liquid Substance.......................................................................................... 23 Project D • Inorganic Forms of Copper ................................................................................................... 29 Project E • Analysis of Lead in Soil......................................................................................................... 35
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particular metal ion. A very common hydrate often encountered in the general chemistry laboratory is copper (II) sulfate pentahydrate‚ CuSO4.5H20. The word “pentahydrate” in the name of this substance indicates that five water molecules are bound in this substance per copper sulfate formula unit. Hydrated water molecules are generally indicated in formulas as shown above for the case of the copper sulfate‚ using a dot to separate the water molecules from the formula of the salt itself. Although not usually
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crucible 29.9g Mass (g) of crucible with hydrate 32.35g Mass (g) of crucible and anhydrous salt 31.39g Questions and Calculations 1. What was the mass of the original hydrate? 2.45g of hydrate Calculations: Mass of crucible with hydrate (32.35g) - Mass of crucible (29.9g) = 2.45g 2. Calculate the mass of water lost from the hydrate. .96g of water lost from hydrate Calculations: Mass of crucible with hydrate (32.35g) - Mass of crucible and anhydrous salt (31.39g) = .96g 3. How many moles of water
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Reaction co-ordinate ?H is the heat content‚ which is the enthalpy‚ which is negative in exothermic reactions as the diagram shows that energy is ’lost’ as heat. Enthalpy is defined as the energy of reaction‚ or the heat energy associated with a chemical change. Chemical Principles By Master & Slowinski says that "For any reaction carried out directly at a constant pressure‚ the heat flow is exactly equal to the difference between enthalpy of products and that of the reactants"‚ or: Qp = Hp - Hr =
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4/13/12-4/14/12 Class Action Lab Report Purpose: To determine‚ through observations‚ the identity of substances produced in a chemical reaction. Materials: Safety Goggles Stirring rod Magnesium ribbon Solid CuSO4•H2O Matches Test tubes Copper metal 3M HCl Red and blue litmus strips 0.1M AgNO3 Zinc metal 0.1M Pb(NO3)2 Test tube holder 0.1M KI Bunsen burner 0.1M Na2NO3 Crucible tongs 1.0M NaOH Water (H2O) 0.1M Ca(NO3)2 50mL beaker 1.0 CuSO4 Procedure: Using
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Bag Oxidation-Reduction Activity Series 1 Copper (II) Sulfate‚ 1 M - 3 mL in Pipet 1 Iron (III) Chloride‚ 2 M - 3 mL in Pipet 1 Iron Metal‚ 2 pc in Bag 2"x 3" Magnesium Metal (ribbon) - 2 Small Pieces in Bag 2"x 3" 1 Magnesium Sulfate‚ 2 M - 3 mL in Pipet 1 Lead metal‚ 4 small pieces in bag 2 x 3” 1 Sodium Sulfate‚ 1 M - 3 mL in Pipet 1 Zinc Metal - 2 Small Pieces in Bag 2"x 3" 1 Zinc Nitrate‚ 2 M - 3 mL in Pipet Procedure 1. Place 10 drops of Sodium sulfate‚ Na2SO4 into well A1 of the 24-well plate
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Guess Paper – 2009 Class – X Subject – Chemistry (P- Block Elements) Kalra sir 09460472649 kalra1977@rediffmail.com Group 15 elements: |Symbol |Atomic |Electronic configuration | | |number | | | |7 |[He]2s22p3 | |N | | | |P |15 |[Ne] 3s23p3 | |As |33 |[Ar]3d104s24p3
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this experiment‚ you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride‚ determine the number of moles of iron used up in the reaction of iron and copper (II) chloride‚ determine the ratio of moles of iron to moles of copper‚ and determine the number of atoms and formula units involved in the reaction. Through
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extracted by heating the compound. 1b. Anhydrous compound: a compound without water. 2a. The dot means that there are water molecules present in the crystal lattice in a specific ratio. 2b. For every mole of copper sulfate‚ there are five moles of water. 2c. The molar mass of copper (II) sulfate is 159.61 grams/mol 2d. The molar mass of 5H2O is 90.10 grams/mol 2e. The molar mass of the entire compound is 159.61 + 90.10 = 249.71 grams/mol 2f. The percent of water in the compound is mass of water/mass
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