Given the reaction Zn + 2AgNO_3 → Zn(NO_3)_2 + 2Ag, how many grams of zinc (Zn) are required to react completely with 8.0 moles of silver nitrate (AgNO_3)?

• A. 65.4 g
• B. 262 g
• C. 524 g
• D. 130.8 g

Answer: (B)

Verified step by step guidance

1. Identify the balanced chemical equation: \(\mathrm{Zn} + 2\mathrm{AgNO}_3 \rightarrow \mathrm{Zn(NO}_3)_2 + 2\mathrm{Ag}\). This tells us that 1 mole of Zn reacts with 2 moles of AgNO\(_3\).
2. Determine the mole ratio between Zn and AgNO\(_3\) from the balanced equation. For every 2 moles of AgNO\(_3\), 1 mole of Zn is required.
3. Calculate the moles of Zn needed to react with 8.0 moles of AgNO\(_3\) using the mole ratio: \(\text{moles of Zn} = \frac{1}{2} \times 8.0\) moles of AgNO\(_3\).
4. Find the molar mass of zinc (Zn) from the periodic table, which is approximately 65.4 g/mol.
5. Calculate the mass of zinc required by multiplying the moles of Zn by its molar mass: \(\text{mass of Zn} = \text{moles of Zn} \times 65.4 \text{ g/mol}\).