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# This experiment involves the decomposition of copper carbonate whereby we want to find out whether CuO(3/4) or Cu20(s) is formed upon the decomposition of copper carbonate when heated. I intend to use mole equations

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Introduction

AS - Assessed Practical 1 Which Equation is Correct? Task: This experiment involves the decomposition of copper carbonate whereby we want to find out whether CuO(?) or Cu20(s) is formed upon the decomposition of copper carbonate when heated. I intend to use mole equations to find the volume of gas produced in both equations in order to solve the problem set. Equation 1 - 2CuCO3(s) Cu2O(s) + 2CO2(g) + 1/2O2 Equation 2 - CuCO3(s) CuO(s) + CO2(g) By using the formula for moles and the volume of gas, I am able to predict the volume of gas produced before I have actually implemented the experiment. Equipment and Reagents * Tripod and Mat * Bunsen Burner and Rubber Bung * Boss and Clamp Stand * 100ml Conical Flask * 100cm� Graduated Gas Syringe * Weighing Scale (�0.01g) * ?g of copper carbonate ( The mass will be decided later on because we are limited to 100cm� volume of gas in the syringe. Background Information Copper carbonate is a green solid when reacted. Once it decomposes upon heating a colour change from green to black will occur. ...read more.

Middle

Cu2O(s) + 2CO2(g) + 1/2O2 Mole ratio: 2 : 1 : 2 : 0.5 2CO2 : The ratio is the same as 2CuCO3, therefore the moles is also equal to 0.008 moles. Volume of Gas = Moles x 24dm� = 0.008 x 24 = 0.190dm� or (x1000) = 190cm� 1/2O2 : The ration is a 1/4 of the mole ratio, therefore the moles for oxygen is: =0.008/4 = 0.002 moles Volume of gas = Moles x 24dm� = 0.002 x 24 = 0.048dm� or (x1000) = 48.0cm� * The total amount of gas in the syringe therefore would be: 190cm� + 48.0cm� = 238.0cm� * This is a problem because the gas syringe cannot hold this amount of gas. * If I were to multiply the total gas by 3/10 we would get 71.4cm�total volume of gas. * This means that if we multiply the mass by 3/10, we would get 0.30g of copper carbonate. * Thus, I will use 0.30g of copper carbonate, and if this value produced a volume that was less than 100cm� in the second equation: Equation 2 - CuCO3(s) ...read more.

Conclusion

CuO(s) + CO2(g) * This equation will produce 58.3cm� of gas. The syringe, which collects the gas, has an accuracy to the nearest decimal place, �0.5cm�. The percentage error is: * (�0.5/58.3) � 100 = 0.86%. * The range of the syringe allows values between 58.2<cm�<58.4. * The total error for equation 2 is: * 0.86% + 1.67% = 2.53% * This indicates that these errors are insignificant and should not affect the results. * I think that this is the least error possible, because if the copper carbonate is not pure, then we will not produce these results and the accuracy. Precision * To make sure that I produce accurate results, I intend to repeat the experiment several times until I achieve consistent results. Safety * Lab coats must be worn during the experiment. * Goggles must be worn at all times. * Make sure that you not using any faulty equipment. * Make sure that the gas syringe moves smoothly and its slider does not get stuck when collecting the gas, which will increase the pressure exerted on it, causing it to break. * Allow the experiment to cool before clearing up because if the conical flask is washed immediately then it will break and also the equipment will be very hot. ...read more.

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