Final answer:
The mass of phosphorus(III) oxide produced from 6.2 g of phosphorus is approximately 11.0 g, as determined by using stoichiometry and molar masses in accordance with the balanced chemical equation for the reaction.
Step-by-step explanation:
The reaction between phosphorus and oxygen to form phosphorus(III) oxide is a stoichiometric problem where the mass of a product formed from a given reactant can be determined using molar masses and coefficients from the balanced chemical equation. The balanced equation for the reaction is 4P(s) + 3O₂(g) → 2P₂O₃(s). To solve this problem, we need to find the molar mass of phosphorus (P), which is approximately 30.97 g/mol, and the molar mass of phosphorus(III) oxide (P₂O₃), which is approximately 109.94 g/mol.
First, we convert the mass of phosphorus to moles:
6.2 g P × (1 mol P / 30.97 g P) = 0.2 mol P
According to the balanced equation, 4 moles of phosphorus produce 2 moles of phosphorus(III) oxide. Therefore, 0.2 moles of phosphorus will produce (0.2 moles P / 4 moles P) × 2 moles P₂O₃ = 0.1 moles P₂O₃. Finally, we convert moles of phosphorus(III) oxide to grams:
0.1 mol P₂O₃ × (109.94 g P₂O₃/mol) = 10.994 g P₂O₃
Thus, the mass of phosphorus(III) oxide produced from 6.2 g of phosphorus is approximately 11.0 g.
Regarding phosphorus and its reactions with oxygen, it is worth noting that the element forms two common oxides: phosphorus(III) oxide and phosphorus(V) oxide. Phosphorus(III) oxide is a white crystalline solid that transforms into phosphoric acid upon reaction with water, while phosphorus(V) oxide can be used in preparing orthophosphoric acid, which has several applications including in fertilizers and cola drinks.