# Cuso4 Reaction Lab

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Finding the % of Yield of a Single Displacement Reaction Purpose: To determine the % of yield of the reaction of copper sulphate and iron with water, in order to learn to use and apply theoretical and actual yield into real life scenarios. Hypothesis: I believe that the mass of the actual yield will be lower than the mass of the theoretical yield because of the decanting. This process can make the precipitate leave the beaker and fall into the sink. Procedure: Refer to handout Lab: Finding the % of Yield of a Single Displacement. Observations Qualitative Before During After Copper (II) Sulphate CuSO4(aq) -Blue -Powdery -Dissolved in water/soluble -Bubbles produced -White residue on top -Gas produced/vapour -Colour changing to green -Very…show more content…
0.03132 mol > 0.27663 mol ∴ CuSO4 is the excess reactant. 3. G: 1.03g Fe, 0.018842 mol Fe, 0.027763 Cu R: theoretical yield of…show more content…
The actual yield is 1.35g, and the theoretical yield is 1.76 g. The yield is higher in the theoretical yield in the actual yield, concluding in the fact that 0.41g of the precipitate has been lost. 1.35g/1.76g=0.767 x 100%=76.7% The percentage yield is 76.7% Communicate Various things could have been the reason for the actual yield. There could have been human error, such as measuring the mass of the beaker wrong or having an unbalanced scale, which would make us miscalculate the mass of the copper that was originally put in. Also, decanting it improperly and letting the precipitate fall can affect this. In this experiment, we used a laboratory technique—decanting. In this process, we removed the solution from the beaker without removing the precipitate, by using a glass rod to separate the water and pour it down the sink. This technique did affect our yield. It is possible that while decanting, some of the precipitate went down the drain with the solution. It is very difficult to decant without losing any