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 moleCu x 63.55g Cu)/(55.85g Fe x 2 mole Fe x 1 mole Cu) = 1.878g. The percent yield for both reactions was found using the equation (actual yield)/(theoretical yield) x 100. These values can be found in Table 1. With these values found it was concluded that reaction 1 occurred during the experiment. The result of the reaction was Fe(SO4)(aq) + Cu(s). In light of the percent yield, there more likely had been some copper lost while decanting if both of the responses had been over 100%, which was the same thing that a portion of different groups concluded as well. Iron was the limiting reactant in both of the equations. The validity and reliability of the information was that it turned out with the best possible answer for the percent yield. Compared with different groups, the main errors could have been the stirring of the mixture while it was attempting to react, and the different measurements of the weights. A portion of the potential errors during the experiment could have been: losing copper while decanting, boiling the water as opposed to getting it around 50° to 75° C, and not permitting the copper(II) sulfate to completely dissolve into the water.
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