Chemical Reaction Yield Calculation PDF

7.5 The yield of a chemical reaction *Most reactions do not produce the exact amount of product that is predicted by the balanced chemical equation 1) Theoretical Yield: the maximum possible mass of product that could be produced in a chemical reaction. 2) Actual Yield: the mass of product actu...

7.5 The yield of a chemical reaction *Most reactions do not produce the exact amount of product that is predicted by the balanced chemical equation 1) Theoretical Yield: the maximum possible mass of product that could be produced in a chemical reaction. 2) Actual Yield: the mass of product actually obtained from a reaction 3) Percentage Yield: a method of expressing how efficiently a reactant can be converted into a product in a chemical reaction. actual yield % yield   100% theoretical yield Example Bromine was made according to the following reaction: HBrO3 + 5HBr 3Br2 + 3H2O If 10.0 g of HBrO3 was reacted with an excess of HBr and 26.3 g of Br2 was produced, what was the percentage yield of the reaction? i) Determine number of moles of reactant used. ii) Determine the theoretical yield of product          mass of Br2 expected iii) Determine % Yield b) If this process was 82% efficient, what is the actual yield? HOMEWORK: p. 339 4-10