“The Law of Conservation of Mass states that matter can be changed from one form into another, mixtures can be separated or made, and pure substances can be decomposed, but the total amount of mass remains constant.” (University Of Wisconsin) The data the was found from our lab shows that the data is not consistent to the Law of Conservation of Mass because our results showed an increase in mass.
To start the lab, .7 grams of copper was measured out and at the end, the total amount of copper was .73 grams. Throughout the five reactions, the theoretical yield was calculated for whatever substance was being created. Those masses (listed in order) include: 2.07 grams CuNo3, 1.08 grams Cu(OH)2, .88 grams CuO, 1.49 grams CuCl2, .70 grams Cu. Then, …show more content…
This is shown in the balanced chemical equation by the products of water and the solid copper chloride. The observation of the liquid turning clear represents the water and seeing the particles represents the precipitate. The yield of copper chloride is 1.49 grams. This demonstrates the transformation of the copper hydroxide being converted into regular copper oxide and with the rest of the mass becoming water. The limiting reactant was the copper oxide and the excess was hydrochloric acid. The analysis behind this is that if there was not enough hydrochloric acid, only part of the copper oxide would react and we would lose mass and violate the Law of Conservation of Mass. The errors for this function could be that when stirred not all the particles would be dissolved and that could affect the …show more content…
Most of the errors in the other reactions would cause a loss of mass, not a gain. The errors that are most likely are the incorrect massing. Whether it was the original mass or the mass of the filter paper with or without the copper would cause a result in the mass because if the original copper weighed more than in our calculations our results would match the Law of Conservation of Mass. Notably, if the mass of the filter paper was incorrect and weighed less than thought, when we subtracted our mass with the filter paper and copper by the original mass, our answer would be higher than
To start the lab, .7 grams of copper was measured out and at the end, the total amount of copper was .73 grams. Throughout the five reactions, the theoretical yield was calculated for whatever substance was being created. Those masses (listed in order) include: 2.07 grams CuNo3, 1.08 grams Cu(OH)2, .88 grams CuO, 1.49 grams CuCl2, .70 grams Cu. Then, …show more content…
This is shown in the balanced chemical equation by the products of water and the solid copper chloride. The observation of the liquid turning clear represents the water and seeing the particles represents the precipitate. The yield of copper chloride is 1.49 grams. This demonstrates the transformation of the copper hydroxide being converted into regular copper oxide and with the rest of the mass becoming water. The limiting reactant was the copper oxide and the excess was hydrochloric acid. The analysis behind this is that if there was not enough hydrochloric acid, only part of the copper oxide would react and we would lose mass and violate the Law of Conservation of Mass. The errors for this function could be that when stirred not all the particles would be dissolved and that could affect the …show more content…
Most of the errors in the other reactions would cause a loss of mass, not a gain. The errors that are most likely are the incorrect massing. Whether it was the original mass or the mass of the filter paper with or without the copper would cause a result in the mass because if the original copper weighed more than in our calculations our results would match the Law of Conservation of Mass. Notably, if the mass of the filter paper was incorrect and weighed less than thought, when we subtracted our mass with the filter paper and copper by the original mass, our answer would be higher than