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

am trying to find out whether the equation 2CuCO3 Cu2O + 2CO2 + O2

Extracts from this document...


Chemistry Coursework Aim: I am trying to find out whether the equation 2CuCO3 ? Cu2O + 2CO2 + 1/2O2 or the equation CuCO3 ? CuO + CO2 is correct for the decomposition of copper carbonate. Introduction: This is my background research, this information may help me when I am trying to see which equation is correct. I have used the book Chemistry 1 by OCR as my reference. Relative Atomic Mass: This is the mass of an atom of the element relative to the mass of an atom of carbon-12 which has a mass of exactly 12. Relative Molecular Mass: This is the mass of a molecule of a compound relative to an atom of carbon-12. Mole: This is the unit of an atom of substance. One mole of a substance is the mass that has the same number of particles (Molecules, Ions or Electrons) as there are atoms in exactly 12g of carbon-12 Avagadro's Constant: This is the number of atoms or molecules in one mole of a substance. ...read more.


Equation 1 produces the most gas. Number of moles = Volume of Gas (cm3) = 80cm3 Molar Volume (cm3) 24000cm3 = 0.0033 moles of gas 1.25 moles of gas is produced from 1 mole of copper carbonate (CuCO3) ? 0.0033 moles of gas is produced from (0.0033) 1.25 = 0.00264 moles of Copper Carbonate m = n x M ? M[CuCO3] = [63.5 + 12 + (3 x 16)] = 123.5g mol 1 ? 0.00264 x 123.5g mol 1 = 0.33g of CuCO3 I can now work out how much gas 0.33g of CuCO3 will give in equation 2: n = m = 0.33g = 0.00267 moles of Copper Carbonate M 123.5g mol 1 1 mole of CuCO3 gives 1 mole of gas ? 0.00267 moles of CuCO3 gives 0.00267 moles of gas. Volume of gas (cm3) = number of moles x molar volume (cm3) = 0.00267 x 24000 cm3 = 64cm3 I can now carry out the experiment and compare the actual value with the two predicted values I have just calculated. ...read more.


5) Light the Bunsen burner and make it at it's hottest temperature, place under the Bunsen burner with the hottest part of the flame touching the boiling tube. Heat the copper carbonate until it has turned black and no more gas is being evolved. 6) Let the gas cool before taking a reading 7) Write down your results and then repeat the experiment twice more to obtain reliable results. Results: Mass of CuCO3/g Volume of Gas Predicted Volumes Actual Volumes Equation 1 Equation 2 0.33g 80cm3 64cm3 64cm3 0.33g 80cm3 64cm3 60cm3 0.33g 80cm3 64cm3 64cm3 Evaluation: From my experiment I have found that equation 1 seems to be the correct equation as my results show that it was almost equal every time to the predicted volume I calculated. When doing my experiment I could have changed some things which could have made the result more accurate. I should have waited until the temperature was at room temperature before taking a reading. I have calculated any inaccuracies I could have made; In weighing --> accuracy or balance x 100 Average mass measured = 0.005g x100 0.33g = 1.52% In gas syringe--> 0.5 x 100 62.7 =0. ...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 War Poetry 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 War Poetry essays

  1. Marked by a teacher

    The idea of the experiment is to determine which equation is correct. There are ...

    5 star(s)

    I also bubbled the gas given off through limewater. The limewater turned milky due to the precipitation of insoluble calcium trioxocarbonate (IV). I am going to heat the cupric carbonate and see what colour the residue will be. If it is black, this shows that CuO is present hence

  2. Which Equation is Correct?

    The gas syringe should be cooled down for a short period of time after the copper carbonate has been heated. This is because gas at a higher temperature expands and so occupies a larger area than corresponding cooler gas. The gas syringe must be a 0 before the experiment is started.

  1. Decompose copper carbonate by heating and measure the amount of gas produced.

    The glass won't melt and won't react with the chemical substance. Tripod- holds the conical flask above Bunsen burner. Bunsen Burner- used as heat source Gauze mat- to place over tripod and to make sure that the heat is more evenly distributed, also makes sure that the conical flask doesn't fall through the tripod.

  2. Determination of the Value of the Gas Constant and the Molar Volume of Oxygen ...

    STP): TIME AFTER HEAT REMOVED (minutes) FINAL VOLUME (cm3) |ERROR| (cm3) 10 89.0 ? 0.5 *NOTE: Time is not a relevant factor for analysis, so errors associated with time are not included, but did remain constant at ? 0.5s Fig.

  1. Free essay

    Which equation is correct?

    The gas burette will start to collect bubbles and every time this happens water will be lost and the gas will come out on top of the gas burette. 7. The rate of gas release will begin to slow down when decomposition is near completion.

  2. Right equation

    How ever e can distinguish the oxidation state by looking at their oxides. Copper I when heated and reacted turn a red compound and Copper II when heated and reacted turn into a black compound Calculation RMM (relative molecular mass)

  1. This experiment involves the decomposition of copper carbonate whereby we want to find out ...

    Accuracy of Equipment and Reagents * All my results have been given to 3 significant figures except for the mass of copper carbonate, which is given to 2 decimal places because the scale can only measure to 2.d.p. Graduated Gas Syringe, Mass and Range: Equation 1 - 2CuCO3(s) Cu2O(s)

  2. The aim of this experiment is to prove which of these two equations is ...

    The largest gas syringe available can hold 100cm�. It would not, however, be sensible to attempt to produce 100cm� because if Equation 1 turns out to be the correct one, which would mean oxygen is also produced and there would consequently be more gas.

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