# Thermal Decomposition of Copper Crabonate

The Thermal Decomposition of Copper Carbonate

Copper carbonate goes through thermal decomposition to form one of these oxides. The two possible equations are:

Equation 1: 2CuCO(s) CuO (s) + 2 CO (g) + 1/2 O (g)

Equation 2: CuCO (s) CuO (s) + CO (g)

Aim

To find out which of the above equations is correct. I will use the mole theory to work out the expected volume of gas released. This predicted will volume will prove which of the two equations is correct.

Apparatus

00 cm³ gas syringe

2 retort stands

Clamp

Delivery tube through bung

Test Tube

Bungs

Bunsen Burner

Heat Proof Mat

Top pan Balance

Spatula

Chemicals

Powered Copper Carbonate

Amounts and Errors

I will collect the amount of gas produced in a gas syringe, and aim to collect approximately 80cm³ . This volume is far enough from the 100cm³ to account for any errors that may cause the volume to increase beyond the scale, if too much gas is evolved. The gas syringes available have a maximum volume of 100cm³, hence why the chosen volume is lower than 100cm³.

There is also the possibility of the gas expanding in the heat, and resulting in the gas having a larger volume than the available volume in the gas syringe. To overcome this problem I will need to let the gas cool before measuring the volume, and may need to cool the gas as it enters the gas syringe.

At room temperature and pressure, the volume of one mole of gas is 24dm³. From this I can find the number of moles of gas each equation will produce, and therefore how much copper carbonate to use. I will use the formula:

Volume(dm³) = Number of Moles x 24dm³

80cm³ = 0.08dm³

Number of moles = 0.08

24

= 0.00333 moles

To get a idea of which equation will give off most gas, equation 2 can be changed to have the same amount of copper carbonate as in equation 1, to start ...