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)
The Decomposition of Copper Carbonate 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 each possible reaction Equation 1: 2CuCO3 (s) [IMAGE] Cu2O (s) + 2CO2 (g) + 1/2O2 (g) Equation 2: CuCO3 (s) [IMAGE] CuO (s) + CO2 (g) The aim of this investigation is to prove which of these two equations is correct. From the equations above we can see that in both reactions gas is evolved and by collecting the volume of gas produced we can accurately say which reaction is taking place. To find which equation is correct, we can use ideas about the mole and the volume one mole of gas occupies at standard conditions. Background Information Basic copper carbonate occurs in nature as the mineral malachite (CuCO3) it can be synthesised in the laboratory regardless of its source; basic copper carbonate has the same composition (CuCO3).
will result in an increase in the speed of the rate of reaction it has
I left the HCl alone, for the 1.5M solution I put 75 cm3 of HCl and 25
Aim: - An experiment on how a volume of nitrogen gas is affected by the pressure exerted on it.
n is the number of moles, R is the gas constant (8.31 J/Kmol), and ΔT is the change in temperature measured in Kelvins.
Investigation of the Thermal Decomposition of Copper Carbonate. Aim: To be able to 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 each possible reaction. Equation 1: 2CuCO3 (s) Cu2O (s) + 2CO2 (g) + O2 (g). Equation 2: CuCO3 (s) CuO (s) + CO2 (g).
Investigating the Thermal Decomposition Of Metal Carbonates Aim: To investigate a range of metal carbonates and see if they thermally decompose. Thermal Decomposition INVESTIGATION [IMAGE] ------- Written By Tauqir Sharif ------------------------ Research: When a metal is thermally decomposed the bond between the metal and its carbonate (carbon and oxygen) is removed and the carbonate is released as carbon dioxide. Metal Carbonate = Metal Oxide + Carbon Dioxide Malachite is an ore of copper.
Avogadro is well known for his hypothesis known as Avogadro's Law. His law states that at a given temperature, equal volumes of gas contain the same number of molecules equal to about 6.0221367 x 10 to the 23rd power.A Mole of a substance is the quantity of the substance that weights the same as its molecular mass. One mole of any substance is Equal to Avogadro's number. Therefore Avogadro's law can be stated in terms of moles, namely that equal volumes of gases at the same temperature and pressure contain the same number of moles.
... of gas particles and molecules, which help define the gas. If there is more volume in a container, then the gas will spread out to fill the full size of the container. All of the properties of gases add some complication to the subject, and many formulas, laws, theories, and hypotheses allow any unknown information on the gas to be discovered, including laws such as Boyle’s Law, which compares pressure to volume, Charles’s Law, which compares temperature to volume, and Avogadro’s Hypothesis, which compares volume to the amount of gas. The Kinetic Molecular Theory is the theory on how the movement of the molecules work, and how they are powered has been created and improved throughout history, up to the twentieth century. The ideal gas law is the connector to the chemical reaction part of gases. Essentially, gases are full of equations, concepts, and properties
So we can work out through this method that the volume of a box with
For an ideal gas at constant temperature, pressure and volume are inversely proportional to each other.
In my experiment, I will use an overall volume of 50 cm³ of 2moles of
First we pour 10mL of infiltration solution and 30mL of sodium bicarbonate in a small beaker.
of Copper Sulphate. To do this I plan to work out the amount of water