• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Experiment to ascertain the products of the thermal decomposition of copper (II) oxide.

Extracts from this document...


Experiment to ascertain the products of the thermal decomposition of copper (II) oxide. Background information Copper carbonate (also known as cupric carbonate) is a compound with the molecular CuCO3 and has a molar mass of 123.5 g/mol. Its boiling point is 200oC, therefore it is a solid at room temperature. It is a blue-green compound often used in artist's paint and some types of make-up. Copper carbonate, CuCO3, thermally decomposes and two reactions could take place: 2CuCO3(s) � Cu2O(s) + 2CO2(g) + 1/2O2(g) CuCO3(s) � CuO(s) + CO2(g) I will be using the moles theorem to calculate, which reaction takes place in the lab. A mole of a solid substance is the mass, which contains the same number of particles as there are in 12g of carbon-12. This number is known as the Avogadro constant, L, which is � 6 x 1023 mol-1. It is important as we can use it to calculate how much of each substance is needed to produce a certain volume or mass of a substance, as I will be doing in this experiment. ...read more.


Variables My independent will be the volume of gas produced during the reaction, as this is what I will be measuring, however I have no dependent variable as there is nothing that I am changing. Calculations Equation 1: 2CuCO3 (s) � CuO (s) + 2CO2 (g) + 1/2O2 (g) * Start with a known volume of gas - 24cm3 of CO2 * Moles (for any gas at room temperature and pressure) = ==> moles of CO2 = = 0.001 moles * The ratio of moles of CO2:O2 is 2:1/2 or 1:1/4, therefore if there is 0.001 moles of CO2 there is 0.00025 moles of O2 * Volume in cm3= moles � 24000 = 0.00025 � 24000 = 6cm3 ==> Volume of gas produced = 6 + 24 = 30cm3 * As 2 moles of CO2 : 2 moles of CuCO3, 0.001 moles of CO2 : 0.001 moles of CuCO3 * Mass of CuCO3 required = moles � Relative Atomic Mass (RAM) ...read more.


It will then be placed inside the boiling tube and the apparatus setup as above. The Bunsen burner will then be lit and switched off once all the copper carbonate has thermally decomposed. I will know the reaction has finished when the gas syringe stops moving out. The gas trapped inside the gas syringe will then be allowed to cool to room temperature (so that the amount of gas can be accurately measured) and the volume measured. This will then be repeated until two results have been collected that are within 0.2 cm3 of each other. I will be careful when handling the copper carbonate as it is harmful if swallowed or inhaled, and I will also need to take precautions, because I am using a Bunsen burner. As a result, I will need to tie my hair back, wear safety glasses and wear a lab coat at all times. Also, I will use a heat proof mat and gauze (so that the equipment doesn't become damaged), and be careful when the Bunsen burner is on, which includes leaving the flame on orange when I am not using it. Furthermore, I will clean my workspace thoroughly afterwards. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Organic Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related AS and A Level Organic Chemistry essays

  1. Thermal Decomposition of Copper Carbonate

    Equation1: Cu2O Equation2: CuO 1.2 291.5 233.2 1 242.88 194.4 0.5 121.44 97.2 0.2 48.58 38.87 EQUATION 1: The number of moles of CuCO3 = = = 0.0016194 The mole ratio between carbon dioxide and copper (I) oxide is 1:1 therefore there will be 0.0016194 moles of carbon dioxide present in the reaction.

  2. Determination of the formula of Hydrated Iron (II) Sulphate crystals

    Firstly, the ions are transferred from the weighing boat to a container to be mixed with the H2SO4 and water and then the ions are transferred to the volumetric flask. In this interlude, some of the Fe2+ ions would have been lost in the containers and on the mixing rod.

  1. The aim of this experiment is to produce Aspirin. This is an estrification in ...

    * The reaction is faster * It gave reliable results * The number of moles present in aspirin was easily calculated and the highest percentage yield that reacted was achieved. Evaluating results and procedures Introduction The evaluation is a critical look at the method, results and conclusions and deciding how accurate and how reliable they are.

  2. Comprehensive and Detailed Chemistry notes

    flow -- In a galvanic cell there are 2 conducting terminals called electrodes. One is called anode and the other cathode -- Electrons leave the anode (-)

  1. Free essay

    Group II metals

    The same process was followed using magnesium and Barium but the Barium had to be done in a fume cupboard and pH value and other observations were recorded. Experiment 2: Reaction of the oxides with water and acid Equipments: Test tubes Spatula Chemicals: Magnesium oxide Calcium oxide Barium oxide Universal

  2. Enzyme catalysed decomposition of hydrogen peroxide

    (5 vol, 10 vol, 15 vol, 20 vol, 25 vol) Variables: I will; Keep the temperature constant at 40 oC by using a water bath. Keep the pH constant at pH 7 using a buffer Keep the volume and concentration of catalase (yeast)

  1. I am going to investigate the difference in enthalpy of combustion for a number ...

    of reactants and products, they are shown with the amount of energy, measured in kilo joules per mole (DH/KJ mol-1) released or required for the particular bond Methanol Oxygen Carbon Dioxide Water CH3OH 1.5 O2 CO2 2H2O 3 C__H 413 1.5O=O 497 2C=O 740 4O__H 463 C__O 360 O__H 463

  2. hydrated copper sulphate

    However this experiment was open to various errors which hindered the chances of obtaining accurate results. Furthermore on many occasions in my calculations, I had to round off number of moles in order to deal with simpler numbers. The reasons for these inaccuracies may have been due to errors in measurement and procedure as will be explained later.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work