Percentage Yield in Chemical Reactions

Percentage Yield in Chemical Reactions

Read each question carefully and provide your answer in the space provided. Show all your work for calculation problems.

1. The   is the maximum amount of product that can be formed from a given amount of reactants.

2. The   is the amount of product actually obtained from a chemical reaction.

3. Percentage yield is calculated by dividing the   by the theoretical yield and multiplying by 100%.

1. Why is the actual yield often less than the theoretical yield?

1. In a reaction, 10.0 g of hydrogen gas reacts with excess oxygen gas to produce water. If 85.0 g of water is produced, calculate the theoretical yield and the percentage yield of water. (Molar mass of H₂ = 2.02 g/mol, O₂ = 32.00 g/mol, H₂O = 18.02 g/mol)

2. When 25.0 g of calcium carbonate (CaCO₃) is heated, it decomposes to form calcium oxide (CaO) and carbon dioxide (CO₂). If the actual yield of CaO is 12.0 g, and the theoretical yield is 14.0 g, what is the percentage yield of CaO? (Molar mass of CaCO₃ = 100.09 g/mol, CaO = 56.08 g/mol, CO₂ = 44.01 g/mol)

1. A percentage yield of 100% means that all reactants were converted into products with no loss.