Final answer:
The decomposition of 1.840 moles of H₂O₂ produces 29.44 grams of oxygen, based on the stoichiometry of the reaction and using the molar mass of O₂.
Step-by-step explanation:
To determine the mass of oxygen produced from the decomposition of 1.840 moles of H₂O₂, we use the balanced chemical equation 2H₂O₂ (aq) ⟶ 2H₂O(l) + O₂(g). According to the stoichiometry of the reaction, 2 moles of H₂O₂ produce 1 mole of O₂. Therefore, 1.840 moles of H₂O₂ will produce half that amount in moles of O₂, which is 0.920 moles of O₂.
Next, we calculate the mass of O₂ produced using the molar mass of O₂, which is approximately 32.00 g/mol. Hence, the mass of oxygen produced is:
Mass of O₂ = moles of O₂ × molar mass of O₂
= 0.920 moles × 32.00 g/mol
= 29.44 grams of O₂.