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Which Equation Is Correct?

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WHICH EQUATION IS CORRECT? Introduction and Application * Copper has two oxides, Cu[2]O and CuO * Copper carbonate, CuCO[3] decomposes on heating to form one of the following oxides and an equation can be written for each possible reaction: [image001.gif] Equation 1: CuCO[3](s) 0.5Cu[2]O(s) + CO[2](g) + 0.25O[2](g) [image002.gif] Equation 2: CuCO[3](s) CuO(s) + CO[2](g) * The task of this experiment is to find out which of the two equations is correct by measuring the amount of gas produced by the reaction. * If equation 2 is correct then the following amount of gas should be produced: Number of grams in 1 mole of copper carbonate (Molecular mass) = 123.5g Number of grams to use in the experiment = 0.3g Number of Moles = Mass / Molecular mass So therefore: Number of moles of copper carbonate to use = 0.3g/123.5g =2.43 x 10^-3moles To work out the volume of carbon dioxide gas produced we use the following equation: Volume = 24000 x Number of moles Therefore: Volume = 24000 x (2.43 x 10^-3moles) Volume = 58.32g or 58.32ml produced from the reaction in Equation 2 � This gives us the volume for carbon dioxide as the ratio ...read more.


This can be used as a secondary check. * (This information is adapted from `Chemistry for You' - Ryan) Variable Control * There are a number of variables that could affect the experiment: 1. Temperature - To ensure that temperature remains constant when heating I shall use the same Bunsen burner and position the flame in the same place for each repetition of the experiment. The whole experiment will be performed under RTP (Room Temperature and Pressure). This is important to keep the heat on the copper carbonate constant and the heat also affects the volume of the gas by making it expand. 2. Surface Area - Although this will not directly affect the experiment the surface area will affect the time that the experiment takes. So I shall use a solid lump of Copper Carbonate with as closer shape as possible to the other ones I shall be using. 3. Pressure - I will not have the ability to keep the pressure constant all the time however I can perform all of the experiments within the same hour so as to reduce the risk of the outside air pressure changing and as this is a closed reaction the pressure will be constant throughout. ...read more.


Work out average 9. From this it should be possible to calculate which equation is correct by the amount of gas produced Apparatus * You will need: + One 100ml gas syringe + Five Large boiling tubes with bungs with holes in + One delivery tube + Two clamp stands * In addition to this you will need: * 1.5g Copper Carbonate split up into five equal sized lumps weighing 0.3g exactly * Apparatus set up: Risk Assessment * There are two chemicals in this reaction that carry warnings: 1. Copper Carbonate (CuCO3) - Labelled as harmful if swallowed and also the dust irritates both lungs and eyes 2. Copper Oxide (Cu2O and CuO) - Labelled as harmful if swallowed and also the dust irritates both lungs and eyes * Taking these warnings into account it will be necessary to wear safety goggles, however with the very small amounts of chemicals we are dealing with it is very unlikely that there will be any serious problems. * If the chemicals come into contact with the eyes then they must be washed in an eye bath, if swallowed medical attention should be sought and if inhaled the person needs to stand outside in the fresh air. ...read more.

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