Final answer:
The mass of hydrogen peroxide needed to produce 64g of oxygen is calculated using the molar mass of H2O2 and the balanced chemical equation. The stoichiometry indicates that 136.04g of H2O2 is required, which does not match any of the provided answer choices.
Step-by-step explanation:
To calculate the mass of hydrogen peroxide (H2O2) needed to produce 64g of oxygen, we can use stoichiometry and the balanced chemical equation:
2H2O2 -> 2H2O + O2
From the equation, it can be seen that two moles of hydrogen peroxide yield one mole of oxygen gas. Also, one mole of oxygen gas has a mass of 32.00g.
If 64g of oxygen are produced, then:
- 64g O2 / 32.00g/mol = 2 mol O2
- According to the reaction stoichiometry, the mole ratio of H2O2 to O2 is 2:1, so we need 2 times more moles of H2O2, which is 4 mol H2O2.
- Now we need to find the mass of 4 moles of H2O2. The molecular weight of H2O2 is approximately 34.01g/mol, so:
- 4 mol H2O2 x 34.01g/mol = 136.04g H2O2
However, we need to consider that the question possibly contains an error as none of the provided answer options are correct based on the stoichiometric calculation.