Final answer:
After conducting the calculations, the correct percentage yield for the reaction is 94.63%, although this does not match any of the provided answer choices.
Step-by-step explanation:
To calculate the percentage yield of the reaction 4As + 3O₂ → As₄O₆ when 10.0g of arsenic (As) is heated in excess oxygen to produce 12.5g of As₄O₆, we first need to determine the theoretical yield of As₄O₆. Using the molar mass of As (74.92 g/mol), we convert the mass of arsenic to moles:
10.0g As × (1 mol As/74.92 g As) = 0.1335 mol As
According to the balanced equation, 4 moles of As produce 1 mole of As₄O₆. Therefore, the moles of As₄O₆ that the reaction could produce theoretically is:
0.1335 mol As × (1 mol As₄O₆ / 4 mol As) = 0.0334 mol As₄O₆
Then, we convert the moles of As₄O₆ to grams using its molar mass (1 mol As₄O₆ = (4×74.92) + (6×32.00) g):
0.0334 mol As₄O₆ × 395.68 g/mol = 13.21 g of As₄O₆ (theoretical yield)
Percentage yield is calculated as (actual yield/theoretical yield) × 100%, which in this case is:
(12.5 g / 13.21 g) × 100% = 94.63%
This percentage does not match any of the given options, suggesting a possible error in the question or in the answer choices provided. However, based on the calculations, none of the options A) 80%, B) 125%, C) 62.5%, or D) 100% are correct.