Answer :
The theoretical yield of Cu is 2.56 g, the actual yield is 0.7 g, and the percent yield is 27.3%.
The theoretical yield, actual yield, and percent yield for the copper recovery experiment:
Balanced Equation:
3CuCO₃ + 2Fe → 3Cu + Fe₂(CO₃)₃
A. Theoretical Yield:
Moles of CuCO₃:
Mass of CuCO₃ = 6.0 g
Molar mass of CuCO₃ = 123.95 g/mol (Cu: 63.55 g/mol, CO₃: 44 g/mol)
Moles of CuCO₃ = 6.0 g / 123.95 g/mol ≈ 0.0485 mol
Limiting Reactant:
Based on the 3:2 stoichiometry in the balanced equation, 0.0485 mol CuCO₃ would require 0.0323 mol Fe (0.0485 mol * 2/3).
Since you added 1.5 g of Fe filings (molar mass of Fe = 55.85 g/mol), which is equivalent to 0.0269 mol Fe (1.5 g / 55.85 g/mol), Fe is the limiting reactant.
Theoretical Yield of Cu:
From the stoichiometry, 0.0269 mol Fe can produce 0.0269 mol * 3/2 = 0.0398 mol Cu.
Theoretical yield of Cu = 0.0398 mol * 63.55 g/mol ≈ 2.52 g
B. Actual Yield:
Actual yield of Cu (given in the experiment) = 0.7 g
C. Percent Yield:
Percent yield = (Actual yield / Theoretical yield) * 100%
Percent yield = (0.7 g / 2.52 g) * 100% ≈ 27.8%
Interpretation:
The percent yield indicates that only about 27.8% of the theoretical amount of Cu was recovered in the experiment. This could be due to various factors such as incomplete reaction, loss of Cu during filtration, or impurities in the reactants.
Important Notes:
The experiment description seems to have some potential typos ("then using tong but the beaker under the hood for the night" and "Get the beaker you put in the hood, heat it for 10 minutes, let it cool and mass all of. Your result of the experiment is .7 grams."). Make sure you clarify these steps with your instructor or in a reliable guide to ensure you're following the procedure correctly.
Be mindful of safety precautions when conducting experiments, especially those involving heating and potentially harmful chemicals. Follow recommended lab practices and wear appropriate personal protective equipment.
