Final answer:
The question seems to involve stoichiometry and the reaction of lead (Pb) with lead (II) oxide (PbO), but the given chemical equation is incorrect. Based on typical reactions, Pb ordinarily reacts with oxygen to form PbO, not with PbO itself. The student would need the correct balanced equation to determine the mass of PbO required.
Step-by-step explanation:
The student appears to be confused about the reactant in the equation.
The chemical equation provided is incomplete and incorrect as it stands, but the question seems to be about a lead reaction and stoichiometry, which likely involves lead (II) oxide (PbO) reacting with lead (Pb) to form a product.
However, in standard reactions, PbO would not react with Pb; instead, it is usually Pb reacting with oxygen to form PbO.
Additionally, the options given for the mass of PbO required seem to refer to a reaction between Pb and PbO, which is not a standard chemical reaction.
Looking at an example provided in the information, 207 g of lead combines with oxygen to form 239 g of a lead oxide. This does not seem to align with the student's question, but it does illustrate the typical reaction of lead with oxygen to form a lead oxide.
Such stoichiometry problems require balanced chemical equations to determine the reactant proportions and the limiting reactant to calculate the mass of products formed or reactants needed.
In the absence of a correct equation and clearer context, I cannot provide an accurate response to the student's original question about the mass of PbO needed to react with 10 grams of Pb.
To assist the student, I would advise them to review the proper balanced chemical equation for the reaction in question and to use stoichiometry for determining the mass relationships between reactants and products.