Final answer:
The mole ratio between P4 and O2 is 1:5, and between P4 and P2O5 it's 1:2. For 2.5 moles of O2, approximately 61.95 grams of P4 is needed. To produce 82.2 grams of P2O5, about 36.26 grams of P4would be required.
Step-by-step explanation:
The mole ratio between P4 and O2 in the reaction P4 + 5 O2 -> 2 P2O5 is 1:5, which means that it takes 5 moles of O2 to react with 1 mole of P4. The mole ratio between P4 and P2O5 is 1:2, indicating that 1 mole of P4 produces 2 moles of P2O5. To find out how many grams of P4 are needed to fully react with 2.5 moles of O2, we first use the mole ratio (1 mole of P4 reacts with 5 moles of O2), then convert the moles of P4 needed to grams using the molar mass of P4 (approximately 123.895 g/mol). Therefore, (2.5 moles O2) x (1 mole P4 / 5 moles O2) x (123.895 g P4 / mole P4) = 61.9475 g of P4 required.
To create 82.2 g of phosphorus oxide (P2O5), we again use the mole ratio from the balanced chemical equation and the molar mass of P2O5 (approximately 141.944 g/mol) to determine the mass of P4 needed. We convert grams of P2O5 to moles, and then use the 1:2 mole ratio between P4 and P2O5 to find moles of P4. Finally, we convert moles of P4 to grams. So, (82.2 g P2O5) / (141.944 g/mol P2O5) x (1 mole P4 / 2 moles P2O5) x (123.895 g P4 / mole P4) ≈ 36.263 g of P4 required.