Final answer:
To find the mass of Cu produced from the reaction of 1.85 g of Al with excess copper (II) sulfate at a yield of 56.6%, calculate the moles of Al, determine the theoretical yield of Cu using stoichiometry, and apply the percentage yield to find the actual yield.
Step-by-step explanation:
To calculate the mass of Cu produced when 1.85 g of Al reacts with excess copper (II) sulfate with a percentage yield of 56.6%, we need to follow these steps:
Unfortunately, the balanced chemical equation is not provided, but assuming it is similar to the copper sulfate and zinc reaction where the stoichiometry would be 1 mol Al to 1 mol Cu, we can proceed with this assumption. The molar mass of Al is 26.98 g/mol, which we use to find the moles of Al:
Moles of Al = 1.85 g / 26.98 g/mol
Next is to find the theoretical yield of Cu:
Theoretical yield of Cu = Moles of Al × (1 mol Cu / 1 mol Al) × 63.55 g/mol (Molar mass of Cu)
Finally, we calculate the actual yield using the percentage yield:
Actual yield of Cu = Theoretical yield of Cu × (56.6% / 100%)
Carry out these calculations, and you will obtain the mass of Cu produced. (Note: Be sure to use the correct balanced equation if it differs from the one assumed here.)