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

Determining the Correct Equation for the Decomposition of Copper Carbonate

Extracts from this document...


Aim: The aim of this experiment is to determine which of the following equations is correct: * Equation 1: 2CuCO3 (s) Cu2O(s) + 2CO2 + 1/2O2(g) * Equation 2: CuCO3 (s) CuO(s) + CO2(g) I will do this by decomposing the copper carbonate. I will need to calculate if the volume of carbon dioxide produced is equal to what the equation suggests. Equipment: * Bunsen burner - To heat the copper carbonate. * Heatproof Mat - To keep Bunsen burner on and to insure furniture is kept safe * Spatula - Used to take out copper carbonate from its packet and placed in dry weighing bottle to be measured. . * Digital Weighing Scales - To weigh the copper carbonate. * Clamp Stand and Clamp x2 - To secure the gas syringe and boiling tube. * Boiling Tube - To place copper carbonate in and then to be heated in. * Dry Weighing Bottle - To measure copper carbonate in. * Bung with Delivery Tube - To make sure gas doesn't escape boiling tube, and only gets delivered to the gas syringe. ...read more.


There is also the problem of the gas expanding in the heat, and having a larger volume than the gas syringe. To tackle this problem I will need to let the gas cool before measuring the volume, and may need to cool the gas as it enters the gas syringe. For my investigation I will use 0.30g of copper carbonate. For equation 1: Equation 1: 2CuCO3 (s) Cu2O(s) + 2CO2 + 1/2O2(g) The ratio of copper carbonate to gases is: 2:21/2 Molar Mass, Mr of copper carbonate = 63.5 + 12 + (16x3) = 123.5 So, in 0.30g of copper carbonate the number of moles will be: Number of moles = Mass / Mr n = 0.30/123.5 = 2.429149798x10-3 = 2.43x10-3 mols So the number of moles of gas will be: (2.43x10-3) X (21/2 / 2) = 2.43x10-3 X 1.25 = 3.04x10-3 mols The volume of a gas in cm3 is the number of moles multiplied by 24000 cm3 = 3.04x10-3 X 24000 = 72.96 cm3 For equation 2: Equation 2: CuCO3 (s) ...read more.


Broken glass must be dealt with maturely as it can easily cut the skin. Method: 1. Gather all apparatus and chemicals required. Set up both of the clamp with clamp stand. 2. Take a Dry Weighing Bottle and place it on the digital weighing scales. Take the weight measurement of this. Retrieve a spatula with the calcium carbonate and add 0.30g of calcium carbonate to the dry weighing bottle. 3. Carefully, pour the calcium carbonate into a boiling tube making sure everything has gone in with no spillages and attach a bung with delivery tube. 4. Fix the boiling tube onto a clamp stand and attach the delivery tube to the 100cm3 gas syringe. Place this gas syringe to the other clamp stand. (All attachments made should be airtight) 5. Retrieve Bunsen burner and place over heatproof mat and under the boiling tube. Being to heat the calcium carbonate. 6. As soon as colour change has turned from green to black (colour of copper oxide), stop heating. Allow all the apparatus to cool, and the gas to contract. When the plunger on the gas syringe has stopped moving, record the volume of gas given off. ...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. Enthalpy Investigation

    The experiments will be taking place in a laboratory so this means that the environment each experiment takes place in should be pretty constant i.e. room temperature etc, this will also help improve my results. Prediction I am expecting that the alcohols with a greater number of carbon atoms within

  2. Thermal Decomposition of Copper Carbonate

    How much copper carbonate should be used to produce a sufficient amount of gas for collection? *(Calculation methods are shown bellow the table.) Mass of copper carbonate [CuCO3]- grams (g) Calculated volume of gas that will be released - (cm3)

  1. F336- aspirin individual Investigation

    calibration curve using various concentrations of salicylic acid and reacting it with neutral iron III chloride. I then place the solutions in to a colorimeter to give me a numerical value from which I make a calibration curve I then add my manufactured aspirin to a solution of 50:50 ratio

  2. Comprehensive and Detailed Chemistry notes

    cleaned and recycled -- C18H38----------> 4CH2=CH2 + C10H22 -- This can yield small molecules such as ethylene and propylene * identify that ethylene, because of the high reactivity of its double bond, is readily transformed into many useful products Ethylene is more reactive than ethane or other alkanes.

  1. Enzyme catalysed decomposition of hydrogen peroxide

    Hypothesis: Preliminary experiment Before I began my actual investigation I had conducted 5 different preliminary experiment to decide on what apparatus I would need, what quantities of enzyme and substrate should be used in the investigation , and what the best method of getting a fair test would be.

  2. coursework plan for halogenalkanes

    I think the C-I bond will have the fastest rate of hydrolysis compared to the C-Br and C-Cl bonds. Not only that I can say the C-I bond has more shielding and a weak nuclear attraction, but because the electrons in the covalent bond are quite far away from the

  1. hydrated copper sulphate

    Errors in procedure and measurement > Some soot was formed at the bottom of the crucible. In turn this adds to the total mass, thus preventing me from obtaining the mass purely of the copper sulphate and crucible + lid.

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

    to find out, which reaction takes place in the lab. The definition of relative atomic mass is the average mass of the naturally occurring isotopes of an atom, taking in to account relative abundance, compared to carbon-12 (which is exactly 12).

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