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# Which Equation is correct?

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Introduction

Chris Ellison Which Equation is correct? Introduction Copper has two oxides, Cu2O and CuO. When heated Copper carbonate, CuCO3 decomposes to form into one of these two oxides. An equation can be written for both- Equation 1: 2CuCO3(s)� Cu2O(s) + 2CO2(G) + 1/2O2(g) Equation 2: CuCO3(s) � CuO(s) + CO2(g) To find out which equation is correct we need to find out how many moles of CO2 and O2 are produced by one mole of CuCO3. Equation 1 1g of CuCo3 will produce 247.2cm3 of gas. Number of moles = Mass Mr 1 124 = 0.0081 moles of CO2 0.0081 = 0.0020 moles of O2 4 = 0.0103 moles of gas produced for 1g of CuCO3. ...read more.

Middle

Stop Watch Diagram Variables and Fair Test In this experiment I want to keep everything the same so I don't get anomalous results. The Copper Carbonate will need to be heated so the gas given off will also be hot, because of this the gas will need to be left to cool before being recorded. When weighing the copper carbonate first zero the scales with the conical flask on them then put 1g of Copper Carbonate in the flask. If the first result is anomalous then you should discard it as a 'practice run'. Between each experiment the conical flask will need to be cleaned well. ...read more.

Conclusion

Method 1. Get the required apparatus and set them up as in the diagram. 2. Weigh out 1g of the Copper Carbonate as shown in the 'Fair Test' paragraph. 3. Heat the Copper Carbonate using the Bunsen burner and collect the gas given off in the measuring cylinder. 4. Leave the gas cool for five minutes. 5. Record the amount of gas in the measuring cylinder. 6. Repeat steps 2-5 four times, if the first result in anomalous then discard it. 7. Get an average of the amount of gas from all reliable attempts. 8. If the average is nearest to 247.2cm3 then the first equation is correct. If it is about 194.4cm3 then the second equation is correct. SAFTY: Always wear goggles when performing experiments in labs. ...read more.

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