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Chemistry coursework plan - Which equation is correct?

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*Copper has two oxides, Cu2O and CuO.*

Copper carbonate, CuCO3 decomposes on heating to form one of these oxides and an equation can be written for possible reaction:

Equation 1: 2CuCO3(s) Cu2O(s) +2CO2 (g) + ½ O2 (g)

Equation2: CuCo3(s) CuO (s) +CO2 (g)

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Copper has two oxides, Cu2O and CuO.

Copper carbonate, CuCO3 decomposes on heating to form one of these oxides and an equation can be written for possible reaction:

Equation 1: 2CuCO3(s) Cu2O(s) +2CO2 (g) + ½ O2 (g)

Equation2: CuCo3(s) CuO (s) +CO2 (g)

To find out which equation is correct I will collect the gas that is produced by both equation, to do I must work out how much gas both equation for a given amount of copper carbonate, so I must first work out how much copper carbonate to use to do this I will estimate how much gas will be produced in the second equation and then work out how much copper carbonate I will need do produce that much gas.

So say 100cm3 of gas is produced in the second equation

Number of moles =Volume of gas = 100 =4.167x10-3 mol

24000 24000

The ratio of copper carbonate : carbon dioxide is 1:1 so number of moles is the same as the number of moles as carbon dioxide which is the only gas that is produced in the second equation so the number of moles of carbon dioxide is 4.167x10-3 and so is the number of moles of copper carbonate.

So there is 4.167x10-3 of copper carbonate

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