Final answer:
The formation rate of dinitrogen pentaoxide is calculated using the disappearance rate of oxygen from the reaction, and the stoichiometric coefficients. The rate is 1.15 × 10⁻¹ mol L⁻¹ s⁻¹.
Step-by-step explanation:
The given balanced chemical equation is 4NO₂(g) + O₂(g) → 2N₂O₅(g). Using stoichiometry, we can relate the disappearance rate of O₂ to the formation rate of N₂O₅. Since two moles of N₂O₅ are formed for every one mole of O₂ that reacts, we can determine the formation rate of dinitrogen pentaoxide by dividing the disappearance rate of oxygen by its stoichiometric coefficient (1) and then multiplying by the stoichiometric coefficient of N₂O₅ (2).
To find the formation rate of N₂O₅, the calculation will be as follows:
Formation rate of N₂O₅ = Disappearance rate of O₂ × (Stoichiometric coefficient of N₂O₅ / Stoichiometric coefficient of O₂)
Using the given disappearance rate of O₂, which is 5.75 × 10⁻² mol L⁻¹ s⁻¹:
Formation rate of N₂O₅ = (5.75 × 10⁻² mol L⁻¹ s⁻¹) × (2/1) = 1.15 × 10⁻¹ mol L⁻¹ s⁻¹.
Therefore, the formation rate of N₂O₅ is 1.15 × 10⁻¹ mol L⁻¹ s⁻¹.