Abstract The main goal of this lab was to find the percent yield of a chemical reaction in which copper (II) chloride and sodium carbonate react to make copper (II) carbonate and sodium chloride. A solution of sodium carbonate and copper (II) chloride solutions were mixed to start the reaction. Then, a paper filter had to be used to separate the copper (II) carbonate precipitate from the rest of the mixture. The experiment determined the actual percent yield of 77.2%. Introduction: The percent yield can give the ability to show the progress of a reaction and see how a chemical reaction worked in an experiment. To find the percent yield and see how well the reaction worked, the actual yield and the theoretical yield can be used. This …show more content…
Qualitative Data: Prior to combining the solution CuCl2 was a transparent blue and Na2CO3 was clear While combining the solutions CuCl2 and Na2CO3, the solution became a cloudy blue After filtering the a dry blue powder was left inside the filter paper and a clear solution had drained through the paper filter. Calculations: Molar Mass and Number of Moles of Reactants CuCl2 and Na2CO3 Molar Mass of CuCl2 = 63.55g Cu + (2 35.45g Cl) Molar Mass of CuCl2 = 134.45g CuCl2 Molar Mass of Na2CO3 = (2 22.99g Na) + (3 16.00g O) + 12.01g C Molar Mass of Na2CO3 = 105.99g Na2CO3 Moles of CuCl2 = Mass of CuC = 9.72 10-3 mol Limiting Reactants : CuCl2 and Na2CO3 Molar Mass CuCO3 = 63.55g Cu + 12.01g C + (2 16.00g O) Molar Mass CuCO3 = 123.56g Mass of CuCO3 = Moles of CuCl2 1Mole of CuCO3Moles of CuCl2Molar Mass of CuCO3Mole of CuCO3 Mass of CuCO3 = 7.96 10-3 mol11 mol1 mol123.56g1 mol Mass of Moles and Mass of the Precipitate Produced (CuCO3) Moles of CuCO3 = Moles of CuCl2 1Mole of CuCO3Moles of CuCl2 Moles of CuCO3 = 7.96 10-3 mol 11 mol1 mol Moles of CuCO3 = 7.96 10-3 mol Mass of CuCO3 = Moles of CuCl2 1Mole of CuCO3Moles of CuCl2Molar Mass of CuCO3Moles of CuCO3 Mass …show more content…
The results of the experiment indicate the limiting reactant to be the 1.07g CuCl2 and 0.984g to be the most CuCO3 that has the ability to be produced. The variation from one hundred percent yield could have caused various circumstances that could have affected the actual percent yield of the experiment. One potential source of error could be during the weighing of CuCl2 and Na2CO3. It is possible that some of the CuCl2 and Na2CO3 remained in the glass stirring rods. This would affect the accuracy of the measurements and change the balance of the reaction, leading to a lower percent yield. Another possible source of error could come from the complete filtration of the precipitate (CuCO3). This would lead to lower measurement of the mass of CuCO3 and filter paper and a lower overall percent yield. In future experiments, to eliminate errors in the percent yield, the experiment should include multiple trials for more reliable data and a close actual percent yield to 100 percent. The experiment could also be performed with a higher grade filter paper to ensure most precipitates do not pass through to the filtered solution, leading to a more precise measurement of the mass of CuCO3 and filter paper and an overall more accurate calculation of the actual percent yield. The measured percent yield may have been affected by the errors,