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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Determination of Water in a Hydrate DESIGN – Aspect 1: Defining the problem & selecting variables Research Question: What percentage of Copper Sulfate Hydrate is water? Background Information: There are many ionic compounds that contain one or more waters of hydration in their formulae. They exists either in anhydrous or hydrated form. Most anhydrous compounds have a strong tendency to absorb water from the humidity in the atmosphere and shifts into a hydrated form. Because of
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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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© 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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charged ions. * Giant ionic lattice. * Electrostatic bonds hold lattices together. * Structure is simple cubic. * Some ionic crystals contain water. * Known as water of crystallisation. * These crystals are hydrated. * Blue copper sulphate crystals are the pentahydrate crystals – CuSO4.5H2O * If there is no water of crystallisation then the ionic crystal is said to be anhydrous. Ionic substances in solution: * Many dissolve in water without difficulty. * Ions become
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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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solution until the solution was either cloudy or had small amounts of solid unknown‚ unable to dissolved‚ at the bottom of the beaker. The solubility was then put into terms of moles per liter. Enthalpy change is the amount of heat that is released or absorbed in a chemical reaction at constant pressure. For enthalpy change to be calculated‚ 30 mL of deionized water was measured out and put in a coffee cup calorimeter. The initial temperature of the water was record. 1 g of the unknown was measured out
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Edexcel A2 Chemistry Questions and Answers Contents Introduction . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 3 Unit 4 Rates‚ equilibria and further organic chemistry Multiple-choice questions ..............................................................................7 Structured questions . . . . . . . . . . . .
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filings and place the end with the filings inside a beaker. Separation of a Mixture of sand and copper salt • In a test tube stir 2 g of sand copper and 5ml of water. • In a hot plate heat up the beaker with the supernatant until water is evaporated. Separation of a Mixture of sand‚ calcium‚ and copper • In a beaker add 3g of sand‚ calcium‚ copper and deionized water and stir until copper dissolves. • Put a filter paper into a funnel‚ then pour the mixture into the filtering apparatus
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–2– N10/4/CHEMI/SP2/ENG/TZ0/XX SECTION A Answer all the questions in the spaces provided. 1. The data below are from an experiment to measure the enthalpy change for the reaction of aqueous copper(II) sulfate‚ CuSO4 (aq) and zinc‚ Zn (s). Cu 2+(aq ) + Zn (s) → Cu (s) + Zn 2+(aq ) 50.0 cm3 of 1.00 mol dm–3 copper(II) sulfate solution was placed in a polystyrene cup and zinc powder was added after 100 seconds. The temperature-time data was taken from a data-logging software program
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