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Copper carbonate thermal decomposition

Decomposition of lead and copper carbonate

Decomposition of copper carbonate

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Determining the Correct Equation for the Decomposition of Copper Carbonate Introduction and background information: Important points to note: ‘At room temperature, 25°C and atmospheric pressure at 1 atmosphere, I mole of any gas will occupy a volume of 24 dm³.’ We will need this to work out how much copper carbonate to decompose to obtain a sufficient amount of carbon dioxide gas. To work out the amount of copper carbonate to use I will need to use the following equations: Number of moles = Mass / Mr PV = nRT P = Pressure V = Volume n = Number of moles R = Gas constant T = Temperature We can substitute n (number of moles) with the first equation to get: PV = (mass/Mr) x RT When rearranged this gives: Mass = (Mr x PV) / RT This will allow me to work out the mass needed. Aim: The aim of this experiment is to determine which of the following equations is correct: [IMAGE]Equation 1: 2CuCO3 (s) Cu2O (s) + 2CO2 (g) + ½ O2 (g) [IMAGE]Equation 2: CuCO3 (s) CuO (s) + CO2 (g) I will do this by decomposing the copper carbonate. I will need to calculate if the volume of carbon dioxide produced is equal to what the equation suggests. Equipment: * Heatproof mat * Bunsen burner * Boiling tube * Bung * Delivery tube * Water bath * Measuring cylinder (250 cm³) * Digital weighing scales * Spatula * Clamp and stand * One molar copper carbonate (1 gram) * Two molar copper carbonate (1 gram)

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