Final answer:
The correct answer to how many moles of silver nitrate are needed to react with 9.1 moles of lead is C. 18.2 moles, according to the mole ratio from the assumed balanced equation: 2 AgNO3 + Pb -> 2 Ag + Pb(NO3)2.
Step-by-step explanation:
The student is asking how many moles of silver nitrate (AgNO3) are needed to completely react with 9.1 moles of lead (Pb). In any stoichiometric problem, it is essential to know the balanced chemical equation to determine the mole ratio between the reactants.
Unfortunately, the question doesn't provide a chemical equation involving silver nitrate and lead. However, the question might be referring to a common reaction where lead reacts with a silver nitrate solution, resulting in the formation of lead (II) nitrate (Pb(NO3)2) and silver. This reaction can be represented as:
2 AgNO3 (aq) + Pb (s) → 2 Ag (s) + Pb(NO3)2 (aq)
According to this equation, 2 moles of AgNO3 are needed to react with 1 mole of Pb. Thus, to completely react with 9.1 moles of Pb, we would need:
2 moles AgNO3/mole Pb × 9.1 moles Pb = 18.2 moles AgNO3
Therefore, the answer is C. 18.2 moles.