When benzene 1C6H62 reacts with bromine 1Br22, bromobenzene 1C6H5Br2 is obtained: C6H6 + Br2¡C6H5Br + HBr (b) If the actual yield of bromobenzene is 42.3 g, what is the percentage yield?

Verified step by step guidance

1. insert step 1: Begin by writing the balanced chemical equation for the reaction: C_6H_6 + Br_2 \rightarrow C_6H_5Br + HBr.
2. insert step 2: Calculate the molar mass of C_6H_6 (benzene) and C_6H_5Br (bromobenzene) using the periodic table.
3. insert step 3: Determine the theoretical yield of C_6H_5Br by using stoichiometry. Start with the amount of C_6H_6 you have, convert it to moles, and use the balanced equation to find the moles of C_6H_5Br that should be produced.
4. insert step 4: Convert the moles of C_6H_5Br to grams using its molar mass to find the theoretical yield in grams.
5. insert step 5: Calculate the percentage yield using the formula: \text{Percentage Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\%.

Key Concepts

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows chemists to determine the theoretical yield of a product from a given amount of reactants, which is essential for calculating percentage yield.

Theoretical Yield

Theoretical yield is the maximum amount of product that can be produced from a given amount of reactants, assuming complete conversion and no losses. It is calculated using stoichiometric ratios derived from the balanced equation, providing a benchmark against which actual yield can be compared.

Percentage Yield

Percentage yield is a measure of the efficiency of a reaction, calculated by dividing the actual yield by the theoretical yield and multiplying by 100. This value indicates how much of the expected product was actually obtained, helping to assess the effectiveness of the reaction and any potential losses.