Final answer:
To calculate the theoretical yield of an equilibrium reaction, the stoichiometry of the balanced chemical equation must be utilized. After obtaining the theoretical yield, the percent yield is computed by dividing the actual yield by the theoretical yield and multiplying by 100%. An example given shows that with a theoretical yield of 15.67g and an actual yield of 14.9g, the percent yield is approximately 95.1%.
Step-by-step explanation:
To find the theoretical yield of a reaction at equilibrium, we must first understand what theoretical yield is and how it is calculated. The theoretical yield is the maximum amount of product that could theoretically be obtained from a given amount of reactants, based on the stoichiometry of the balanced chemical equation. When calculating theoretical yield, one must consider the moles of reactants and the mole ratio between reactants and products.
Once the theoretical yield is determined, we can then calculate the percent yield by comparing the actual yield to the theoretical yield. The formula for percent yield is:
Percent Yield = (Actual Yield / Theoretical Yield) × 100%
For example, if the actual yield is known to be 14.9g and the theoretical yield is calculated to be 15.67g, then the percent yield would be calculated as follows:
Percent Yield = (14.9 / 15.67) × 100% ≈ 95.1%
This value represents the efficiency of the reaction and how closely the reaction approached equilibrium. Remember that in real-life reactions, some amount of product may be lost or side reactions may occur, leading to a percent yield less than 100%.