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Chemistry Aim: I am trying to find out whether the equation 2CuCO3 ® Cu2O + 2CO2 + ½O2 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
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. Which ever value is closest to the actual value is the correct value and so its equation will be the correct equation.

Method

I will now carry out a risk assessment of the