Fe + CuSO4 –> Cu + FeSO4 Calculate the theoretical yield of elemental copper metal in your reaction, in grams, if the other product of the reaction is iron (II) sulfate. 100 mL of 1M CuSO4 Fe: 2.02 g FeSO4: 2.747 g I’ve worked it out a few times and feel like my answer isn’t correct.
The Correct Answer and Explanation is:
To calculate the theoretical yield of copper (Cu) from the reaction between iron (Fe) and copper(II) sulfate (CuSO4), we need to use stoichiometry. Let’s break down the process step-by-step:
Given:
- Volume of CuSO4 solution = 100 mL = 0.100 L
- Concentration of CuSO4 solution = 1 M (moles per liter)
- Molar mass of Fe (Iron) = 55.85 g/mol
- Molar mass of Cu (Copper) = 63.55 g/mol
- Molar mass of FeSO4 (Iron(II) sulfate) = 151.91 g/mol
Step 1: Calculate moles of CuSO4
Since we have a 1 M solution, the number of moles of CuSO4 in 100 mL (0.100 L) is: moles of CuSO4=1 mol/L×0.100 L=0.100 mol\text{moles of CuSO4} = 1 \, \text{mol/L} \times 0.100 \, \text{L} = 0.100 \, \text{mol}moles of CuSO4=1mol/L×0.100L=0.100mol
Step 2: Stoichiometry of the reaction
The balanced reaction is: Fe+CuSO4→Cu+FeSO4\text{Fe} + \text{CuSO4} \rightarrow \text{Cu} + \text{FeSO4}Fe+CuSO4→Cu+FeSO4
This indicates that 1 mole of Fe reacts with 1 mole of CuSO4 to produce 1 mole of Cu and 1 mole of FeSO4. Hence, the number of moles of Cu produced will be the same as the moles of CuSO4 used, which is 0.100 mol.
Step 3: Calculate the mass of Cu produced
Now that we know we have 0.100 mol of Cu being produced, we can calculate the mass of copper using its molar mass: mass of Cu=moles of Cu×molar mass of Cu\text{mass of Cu} = \text{moles of Cu} \times \text{molar mass of Cu}mass of Cu=moles of Cu×molar mass of Cu mass of Cu=0.100 mol×63.55 g/mol=6.355 g\text{mass of Cu} = 0.100 \, \text{mol} \times 63.55 \, \text{g/mol} = 6.355 \, \text{g}mass of Cu=0.100mol×63.55g/mol=6.355g
Step 4: Conclusion
The theoretical yield of copper (Cu) in this reaction is 6.355 grams.
If you were using the amount of iron (Fe) in the reaction as a limiting reagent, you’d need to confirm the amount of iron available. However, from the information given, it looks like copper sulfate (CuSO4) is in excess, so copper is the limiting reactant.
