Final answer:
To calculate the percent yield, one would compare the actual mass of Sb₄O₆ produced to the theoretical mass expected from stoichiometry. The percent yield is found by dividing the actual yield by the theoretical yield and multiplying by 100%. The specific question cannot be answered without the balanced chemical equation and molar masses.
Step-by-step explanation:
To determine the percent yield of the reaction between antimony sulfide (Sb₂S₃) and excess oxygen that produces antimony tetroxide (Sb₄O₆), we need to follow several steps. Firstly, calculate the theoretical yield of Sb₄O₆ from the given amount of Sb₂S₃. This involves using stoichiometry to convert grams of Sb₂S₃ to moles and then use the balanced chemical equation to find moles of Sb₄O₆. Subsequently, the moles of Sb₄O₆ are converted back to grams to find the theoretical yield. The percent yield is then calculated by taking the actual yield (the given 72.4 g of Sb₄O₆) and dividing it by the theoretical yield, then multiplying by 100%.
For this question, we are missing the balanced chemical equation and molar masses needed to perform the stoichiometric calculations. However, the steps to calculate percent yield would be consistent: measure the actual yield, compare it to the theoretical yield, and then apply the formula: Percent Yield = (Actual Yield / Theoretical Yield) x 100%.