Final answer:
The question cannot be answered with the provided information because it refers to a reaction involving silver nitrate and sodium chloride, not silver nitrite and sodium sulfide. So correct potion is (C).
Step-by-step explanation:
To answer this question, we first need to understand the stoichiometry of the reaction between silver nitrate (AgNO3) and sodium sulfide (Na2S). The balanced chemical equation is:
2AgNO3(aq) + Na2S(aq) → Ag2S(s) + 2NaNO3(aq)
This equation tells us that 2 moles of silver nitrate react with 1 mole of sodium sulfide to produce 1 mole of silver sulfide (Ag2S) and 2 moles of sodium nitrate.
Let's assume that we start with 35.5 g of both silver nitrate and sodium sulfide, which corresponds to one mole of each based on their molar masses.
During the reaction, all the silver nitrate will react, forming Ag2S. However, sodium sulfide is in excess, so it will not be completely consumed. The limiting reactant is silver nitrate.
The molar mass of silver nitrate (AgNO3) is approximately 169.87 g/mol, so 35.5 g corresponds to
35.5g/169.87g/mol moles of silver nitrate.
Since the balanced equation indicates a 1:1 ratio between silver nitrate and silver sulfide, the amount of silver sulfide formed will be the same, i.e., 35.5 g.
Now, sodium sulfide is in excess, so it will remain unreacted. The molar mass of sodium sulfide (Na2S) is approximately 78.04 g/mol, so 35.5 g corresponds to 35.5g/78.04g/mol moles of sodium sulfide.
Therefore, the correct answer is: C) 35.5 g of silver nitrite, 0 g of sodium sulfide
This assumes complete reaction and ideal conditions. In reality, reactions may not go to completion due to factors like impurities, side reactions, or incomplete mixing.