When 130 grams of zinc (Zn) reacts with excess silver nitrate (AgNO_3) according to the equation Zn + 2AgNO_3 → Zn(NO_3)_2 + 2Ag, how many moles of silver (Ag) are produced?

• A. 1.0 mole
• B. 2.0 moles
• C. 0.5 mole
• D. 4.0 moles

Answer: (B)

Verified step by step guidance

1. Identify the balanced chemical equation: \(\text{Zn} + 2\text{AgNO}_3 \rightarrow \text{Zn(NO}_3)_2 + 2\text{Ag}\).
2. Calculate the number of moles of zinc (Zn) used by dividing the given mass by the molar mass of zinc: \(\text{moles of Zn} = \frac{130\ \text{g}}{\text{molar mass of Zn}}\).
3. Use the mole ratio from the balanced equation to find the moles of silver (Ag) produced. According to the equation, 1 mole of Zn produces 2 moles of Ag, so multiply the moles of Zn by 2: \(\text{moles of Ag} = 2 \times \text{moles of Zn}\).
4. Since silver nitrate (AgNO\(_3\)) is in excess, it does not limit the reaction, so all zinc will react completely.
5. The result from step 3 gives the number of moles of silver produced.