The Decomposition of Copper Carbonate Essay Example for Free

The Decomposition of Copper Carbonate EssayPlanning CourseworkAimOur project is to rally come in what products are formed when copper carbonate decomposes. Copper has 2 oxides, Cu2O and CuO. We are told that one of the following two equations are worsenEquation 1 (Eqn1) 2 CuCO3 (s) Cu2O (s) + 2 carbon dioxide (g) + 1/2 O2 (g)Equation 2 (Eqn2) CuCO3 (s) CuO (s) + CO2 (g)CalculationsI have to find out which of the two are correct by experimentation. By looking at the equations, I preserve see that gas is given out. assembling this gas will be a good way to find out which equation is correct. I will collect the gas in a 100cm3 gas syringe. thitherfore I privation to be collecting virtually 80cm3 of gas per tote up of copper carbonate.Eqn1 Ratio copper carbonate gas2 2 + 1/21 1.25Eqn2 Ratio copper carbonate gas1 1Above states that 2 1/2 moles of gas are produced in Eqn1. I know that 1 mole of gas occupies 24000cm3 in standard room temperature and pres for sure. I hav e stated that I want to collect about 80cm3. This means that I wasnt to collect 80/24000 moles of gas. This is equal to 0.00333. (recurring) moles of gas. Out of the 0.0033 moles of gas collected,2 of them have to be moles of CO2 and 0.5 of them are moles of 022.5 2.5So in Eqn1 we want 2 x 0.0033 moles of CO2 to be collected which is 0.00266 moles2.5According to the Eqn, the mole ratio of CuCO3 to CO2 is 22. This means we consume 0.00266 moles CuCO3 to be decomposed in oreder to create the 80cm3 of gas. From this we can find the mass of CuCO3 to be used, by using the formula hoi polloi = moles x RFM (relative formula mass)= 0.00266 x (63.5 + 12 + (16 x 3) )= 0.329gSo in Eqn1, using 0.329g CuCO3 should produce about 80cm3 gas. Using 0.329g CuCO3 in Eqn2 should give less than 80cm3 gas. I shall prove thisCuCO3 (s) CuO (s) + CO2 (g)Mass of CuCO3 0.329gMoles of CuCO3 0.00266Moles of CO2 produced 0.00266 peck of CO2 produced 0.00266 x 24000 = 63.9cm3Therefore, I know that whichever Eqn is correct, using 0.329g CuCO3 will not produce over 80cm3, and and so the gas will definitely be able to fit into the gas syringeDiagram tonalityThis represents the syringe existence held by a retort stand and also the boiling tube being held by tonguesMethod* Weigh exactly about 0.329g powdered copper carbonate* Set out apparatus as above* Put copper carbonate into boiling tube and put tiptoe on. Bung should be as tight as possible to ensure it is air tight and to denigrate the amount of gas lost* Attach delivery tube to gas syringe making sure plunger is fully depressed* Light the bunsen on a yellow flame for gum elastic and then turn it to a blue flame when ready to begin experiment* Apply Bunsen burner under boiling tube, wafting it under the copper carbonate* I know when the reaction has stopped by when the copper carbonate has gone red or black (depending whether Cu2O or CuO is produced).* Also, when the reaction stops, the plunger on the gas syringe will stop mov ing* It might be necessary to wait to allow the syringe and its contents to cool down so that the gas occupies the correct volumeI need to make sure the experiment is fair to ensure accurate results. From past experience, I know that when the syringe is fully depressed, but then the bung is added, the syringe plunger extends a bit. However in this experiment, the reaction wont start straight away. Therefore I will need to make sure that I push the plunger back in before heat is applied. The experiment will be perennial 3 times and a mean of the results will be taken. All of the results must be harmonized with the mean. This will reduce chance of any anomalous data being used. The condition must persist constant throughout each experiment. The collected gas should be at standard room temperature and pressure.There is another test that could help find which equation is correct. In both equations CO2 is produced. To check this, we could spill the beans the gas through limewater, w hich turns milky in social movement in CO2. However, in eqn1 O2 is also produced. The test for the presence of O2 is to place a glowing splint into the gas. If it relights, O2 is present. However, this method is not very adequate as the amount of O2 produced is very small in comparison to the CO2, and even if it was present it still might not take a glowing splintResultsProviding under about 70cm3 of gas is produced, it shows that no oxygen is produced and so we can say that the 2nd equation is correctPrecautionsDuring experiment, safety goggles should be worn throughout. Wear a lab coat so that it may be removed, without problem, if chemicals spill onto it. Plastic gloves should be worn to hold chemical contact with contend. Also, when handling Bunsen burners, care should be taken.Copper (I) oxide (Cu2O) may be bruising if swallowed or if inhaled, could irritate lungs. If in contact with eye, rinse thoroughly with water for 15 mins and seek health check attention if problem persists. If in contact with skin, rinse with soap and water, and if swallowed in reasonable quantity, seek medical examination attentionCopper (II) Oxide (CuO) Causes eye irritation, can damage cornea. Flush eyes with water for 15 mins. Irritates skin and can discolour it. If contact should occur, wash skin with soap and water. If swallowed, can cause damage to kidneys and liver. may also cause vascular collapse. However, do not induce vomiting, but drink cupfuls of milk. Id breathing is exhausting do not give mouth to mouth resuscitationCopper Carbonate (CuCO3) risks are similar, yet not so hazardous. However treat with similar care. Do induce vomiting if swallowedBibliographyhttp//ptcl.chem.ox.ac.uk/hmc/hsci/chemicals/copper_I_oxide.html chemical safety on Copper (I) Oxidehttp//avogadro.chem.iastate.edu/MSDS/CuO.htm chemical safety on Copper (II) Oxidehttp//en.wikipedia.org/wiki/Copper%28I%29_oxide general information on the copper oxides