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Which oxide is formed when copper carbonate decomposes.

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Introduction

Introduction Aim Copper has two oxides, namely, CuO and Cu2O. Copper carbonate, CuCO3 decomposes on heating to form one of these oxides and an equation can be written for each possible reaction: Equation 1: 2CuCO3 (s) Cu2O (s) + 2CO2 (g) + 1/2O2 (g) Equation 2: CuCO3 (s) CuO (s) + CO2 (g) Our aim for the investigation is to find out which of the two equations above is correct and which oxide is formed when copper carbonate decomposes. Using the mole theory, an experiment is to be designed to measure the volume of gas, which will hence prove that which is the correct equation for the practical. The students also have to determine the quantities of reagents to be used in the experiment. Background Information Copper is a transition metal. It is found abundantly at many locations as a primary mineral in basaltic lavas and also as reduced from copper compounds. Copper pure is very malleable and ductile and can be rolled into sheets, hammered into thin leaves, and drawn into wire. ...read more.

Middle

so the amount of gas does not exceed 100 cm3. Due to this I have decided to use 0.5g of copper carbonate (CuCO3). Equation 1 2CuCO3 (s) Cu2O (s) + 2CO2 (g) + 1/2O2 (g) Mass of CuCO3 = 0.4g Molar Mass of CuCO3 = 63.5 + 12 + (16 * 3) = 123.5 g mol-1 ?Number of Moles of CuCO3 = mass of CuCO3 / molar mass = 0.4g / 123.5 g mol-1 = 0.00324 mols Molar Ratio = CuCO3 : CO2 = 2 : 2 = 1:1 Molar Ratio = CuCO3 : O2 2 : 1/2 ?Number of moles of CO2 = 0.00324 mols (3 sig. Fig) Volume of CO2 produced = number of moles of CO2 * 24000 cm3 = 0.00324 mols * 24000 cm3 = 77.7 cm3 (3 sig. Fig) ?Number of moles of O2 = 0.00324 / 4 = 0.0008097 mols Volume of O2 produced = number of moles of O2 * 24000 cm3 = 0.0008097 mols * 24000 cm3 = 19.4 cm3 (3 sig. ...read more.

Conclusion

Take the empty small beaker and put it on the digital weighing scale and bring the reading to 0.00. Then, using the spatula put 0.4g of copper carbonate in the beaker. 3) Pour copper carbonate into the test tube and close the mouth of the test tube using a rubber bung. Ensure that the delivery tube is attached firmly in the rubber bung. 4) Make sure that the gas syringe is at 0 cm3 and that the delivery tube is securely fastened to the end of the syringe. 5) Turn the Bunsen burner on putting it on a yellow - orange flame. Then bring the tube near the Bunsen burner using the tongs and turn the flame to blue. Start heating the test tube. Using the tongs prevents your fingers from burning. 6) Wait for a reaction to take place. 7) As a reaction starts to take place, gas will be formed and the gas syringe will start moving indicating the volume of gas that has been formed. The reaction will stop when the gas stops forming. This will be indicated clearly when the gas syringe stops moving. 8) The total volume of gas formed can now be recorded in the results table along with any other observations. 1 ...read more.

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