253ml of water was filled into the beaker alongside

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25.3mL of water was filled into the beaker alongside 8.014g of copper (II) sulfate. At the point of having the proper temperature, 1.100g of iron was included. The completion measure of copper that was made from this response was 0.738g. This was a deficient value due to human error. This was obvious when the chemical mixture was stirred as opposed to letting it sit and accumulate at the base of the beaker. This caused a portion of the copper flakes to remain ascended as opposed to sinking to the base, so, when the decanting process started, those flakes were lost. A portion of the steps that were taken to try and diminish error, were when measuring the iron and the copper (II) sulfate, it was pivotal to get them as close as possible to the exact amount that was described in the procedure. Additionally, while warming up the water, extra attention was used to ensure that the water didn't bubble and demolish the experiment.
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Table 1 : Calculations of the Copper Yields Produced Theoretical Actual Percentage 1 1.252g 1.054g 84.19% 2 1.878g 1.054g 56.12% Section 3: The claim made was that reaction 1 [CuSO 4 (aq) + Fe(s) FeSO 4 (aq) + Cu(s)] was the reaction that occurred. The claim was justified due to the fact that it was closer to 100% than reaction 2, which means it was closer to the maximum theoretical yield. To find the theoretical yield, these two equations were used: Reaction 1: (1.100g Fe x 1 mole Fe x 1 mole Cu x 63.55g Cu)/(55.85g Fe x 1 mole Fe x 1 mole Cu) = 1.252g; Reaction 2: (1.100g Fe x 1 mole Fe x 3 mole
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