Tetraphosphorus hexaoxide is formed by the reaction of phosphorus with oxygen gas. If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆, what is the percent yield for the reaction? A) 57.5% B) 48.8% C) 38.0% D) 89.4% E) 16.3%

Question

Quizplus · Accepted Answer

The percent yield is calculated using the formula: (actual yield/theoretical yield) * 100. First, determine the limiting reactant. The molar mass of phosphorus (P) is approximately 31 g/mol, and oxygen (O) is 16 g/mol. The molecular formula for tetraphosphorus hexaoxide is P4O6. Using stoichiometry, we find that the theoretical yield of P4O6 from the given amounts of reactants is higher than 43.3 g, making 43.3 g the actual yield. Calculating the percent yield: (43.3 g / theoretical yield) * 100 gives a value close to 48.8%, indicating that option B is correct.

Tetraphosphorus Hexaoxide Is Formed by the Reaction of Phosphorus with Oxygen