Final answer:
To find the amount of diphosphorus trioxide (P₂O₃) required to react completely with 4.0 moles of water (H₂O), we can use stoichiometry and the balanced chemical equation. By using the ratio from the equation, we can calculate that 1.33 moles of P₂O₃ are required. And with the molar mass of P₂O₃, we can determine that 146.19 grams of P₂O₃ are needed.
Step-by-step explanation:
To determine the amount of diphosphorus trioxide (P₂O₃) required to react completely with 4.0 moles of water (H₂O), we need to use the balanced chemical equation and stoichiometry.
The balanced equation is: P₂O₃ + 3H₂O → 2H₃PO₃
From the equation, we can see that 1 mole of P₂O₃ reacts with 3 moles of H₂O. Therefore, to find out how many moles of P₂O₃ react with 4.0 moles of H₂O, we can use the ratio:
1 mole P₂O₃ : 3 moles H₂O = x moles P₂O₃ : 4.0 moles H₂O
By cross-multiplying and solving for x, we get:
x = (1 mole P₂O₃ x 4.0 moles H₂O) / 3 moles H₂O
x = 1.33 moles P₂O₃
Since we need to find the mass of P₂O₃ in grams, we can use its molar mass which is 109.95 g/mol. Therefore, the mass of P₂O₃ required would be:
Mass = moles x molar mass = 1.33 moles x 109.95 g/mol = 146.19 grams