The purpose of the experiment is to perform a series of chemical reactions involving copper. The goal is then to perform precipitation, acid-base, decomposition, and redox reactions using the copper cycle. The mass of the copper was then analyzed using the percent recovery formula.
Reaction 1: The Formation of Cu(NO3)2: Reaction 1 of the experiment involved performing a redox reaction to create Cu(NO3)2. Immediately after HNO3 was added to the copper wire (Cu), the brown NO2 gas was emitted from the solution. As the copper wire dissolved, the solution green and eventually blue. Once the reaction was complete, the solution ceased to emit gas. It was evident that the reaction was exothermic since the beaker was hot, indicating that there was …show more content…
Once the solution had been heated and stirred, the solution became clear and a black precipitate was present. Since heat was applied to the beaker (energy went into the system), the reaction was classified as endothermic.
Decomposition Reaction:
Balanced Chemical
Equation Cu(OH)_(2 (s))→CuO_((s))+H_2 O_((g))
Reaction 4: The Formation of CuSO4: Reaction 4 involved an acid-base reaction between CuO, the Arrhenius base, and H2SO4, the Arrhenius acid to form the CuSO4 salt and water (H2O). After the acid had been added into the solution, the solution became uniformly clear and light blue. It was evident that the reaction was exothermic since the beaker was hot, indicating that there was a release of energy in the form of heat.
Acid-Base Reaction:
Formula …show more content…
Theoretically, the experiment’s final mass should be equal to the initial mass of copper. The resulting mass of the copper was determined to be .422 g whereas the initial mass was .441 g. Therefore, the percent recovery was calculated to be 95.692% recovery of the initial copper mass. Although the experiment produced a relatively high percent recovery, it does not support the Law of Conservation of Mass because the result still was not 100%, thus concluding that mass had to have been lost. One possible explanation of the loss of copper mass is that not all the Copper on the Aluminum wire of Reaction 5 came off or the reaction was not fully complete. Alternatively, when the irrelevant solutions were discarded into a waste beaker, some of the remaining copper oxide from Reaction 3 did not sink to bottom after having given time to settle. Thus, more mass could have been lost during the decanting
Reaction 1: The Formation of Cu(NO3)2: Reaction 1 of the experiment involved performing a redox reaction to create Cu(NO3)2. Immediately after HNO3 was added to the copper wire (Cu), the brown NO2 gas was emitted from the solution. As the copper wire dissolved, the solution green and eventually blue. Once the reaction was complete, the solution ceased to emit gas. It was evident that the reaction was exothermic since the beaker was hot, indicating that there was …show more content…
Once the solution had been heated and stirred, the solution became clear and a black precipitate was present. Since heat was applied to the beaker (energy went into the system), the reaction was classified as endothermic.
Decomposition Reaction:
Balanced Chemical
Equation Cu(OH)_(2 (s))→CuO_((s))+H_2 O_((g))
Reaction 4: The Formation of CuSO4: Reaction 4 involved an acid-base reaction between CuO, the Arrhenius base, and H2SO4, the Arrhenius acid to form the CuSO4 salt and water (H2O). After the acid had been added into the solution, the solution became uniformly clear and light blue. It was evident that the reaction was exothermic since the beaker was hot, indicating that there was a release of energy in the form of heat.
Acid-Base Reaction:
Formula …show more content…
Theoretically, the experiment’s final mass should be equal to the initial mass of copper. The resulting mass of the copper was determined to be .422 g whereas the initial mass was .441 g. Therefore, the percent recovery was calculated to be 95.692% recovery of the initial copper mass. Although the experiment produced a relatively high percent recovery, it does not support the Law of Conservation of Mass because the result still was not 100%, thus concluding that mass had to have been lost. One possible explanation of the loss of copper mass is that not all the Copper on the Aluminum wire of Reaction 5 came off or the reaction was not fully complete. Alternatively, when the irrelevant solutions were discarded into a waste beaker, some of the remaining copper oxide from Reaction 3 did not sink to bottom after having given time to settle. Thus, more mass could have been lost during the decanting