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

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Introduction

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.

Middle

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.

Conclusion

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.

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