Final answer:
To produce 64g of oxygen gas, 136.16g of hydrogen peroxide is required, according to stoichiometry based on the balanced chemical reaction.
Step-by-step explanation:
To calculate the mass of hydrogen peroxide (H₂O₂) needed to produce 64g of oxygen (O₂), we need to use stoichiometry based on the balanced chemical equation:
2 H₂O₂ (aq) → 2 H₂O (l) + O₂ (g)
From the balanced equation, we can see that 2 moles of hydrogen peroxide yield 1 mole of oxygen gas. The oxygen gas's (O₂) molar mass is 32.00 g/mol. Therefore, 64g of O₂ corresponds to 64g / 32.00 g/mol = 2 moles of O₂. Since 2 moles of H₂O₂ produce 1 mole of O₂, we will need 4 moles of H₂O₂ to produce 2 moles of O₂.
The molar mass of hydrogen peroxide (H₂O₂) is approximately (2 x 2.02 g) + (2 x 16.00 g) = 34.04 g/mol. Hence, the mass of hydrogen peroxide needed is 4 moles x 34.04 g/mol = 136.16 g of H₂O₂.