Final answer:
When 0.45 mole of PbO₂ decomposes, it produces 0.225 mole of oxygen, based on the stoichiometry of the balanced decomposition reaction.
Step-by-step explanation:
The question pertains to the decomposition reaction of lead(IV) oxide (PbO₂) and how many moles of oxygen can be produced from a given amount of this reactant. According to stoichiometry and the balanced chemical equation,
PbO₂(s) ⇒ Pb(s) + ½O₂(g)
From the balanced equation, we see that 1 mole of PbO₂ yields ½ mole of O₂. Using the mole ratio, we can set up a simple calculation:
(moles of O₂) = (0.45 mole of PbO₂) × (½ mole O₂ / 1 mole PbO₂) = 0.225 mole of O₂
Therefore, 0.45 mole of PbO₂ will produce 0.225 mole of oxygen when it decomposes. This stoichiometric calculation ensures that the units of moles of PbO₂ will cancel, and the result will be in moles of oxygen.