Final answer:
To find the masses of P4O6 and P4O10, we initially determine the limiting reagent by comparing mole ratios, and then use stoichiometry to convert moles of the limiting reagent to moles of the desired products, and finally convert those to grams.
Step-by-step explanation:
To determine the masses of P4O6 and P4O10 formed, we need to perform a stoichiometric analysis based on the balanced chemical equations for the formation of these phosphorus oxides and the initial amounts of phosphorus (P) and oxygen (O2) provided.
Step 1: Determine the limiting reagent
First, we convert the masses of P and O2 to moles by dividing by their respective molar masses:
- Mass of P: 105.5 g
- Molar mass of P (approx.): 31 g/mol
- Moles of P: 105.5 g ÷ 31 g/mol = 3.4 moles of P
- Mass of O2: 109.0 g
- Molar mass of O2: 32 g/mol
- Moles of O2: 109.0 g ÷ 32 g/mol = 3.41 moles of O2
Looking at the balanced chemical equations (a), for every 1 mole of P4, 5 moles of O2 are required. Thus, O2 is the limiting reagent.
Step 2: Calculate the mass of products formed
Using the balanced equations, we relate the moles of the limiting reagent to the moles of P4O6 and P4O10. Without the specific balanced equations for the formation of P4O6 and P4O10, we will not be able to provide the exact masses of products formed. However, you would generally convert the moles of the limiting reagent to moles of the products using the stoichiometry from the balanced equations, and then convert those moles to grams using the molar masses for P4O6 and P4O10.