Given the reaction AgNO_3 + NaCl → AgCl + NaNO_3, how many moles of AgCl are produced from 15.0 mol of AgNO_3, assuming excess NaCl?

• A. 30.0 mol
• B. 15.0 mol
• C. 7.5 mol
• D. 1.0 mol

Answer: (B)

Verified step by step guidance

1. Write the balanced chemical equation for the reaction: \(\mathrm{AgNO_3 + NaCl \rightarrow AgCl + NaNO_3}\). This shows a 1:1 mole ratio between AgNO_3 and AgCl.
2. Identify the given quantity: 15.0 moles of AgNO_3, and note that NaCl is in excess, so it will not limit the reaction.
3. Use the mole ratio from the balanced equation to relate moles of AgNO_3 to moles of AgCl. Since the ratio is 1:1, the moles of AgCl produced will be equal to the moles of AgNO_3 reacted.
4. Set up the calculation: \(\text{moles of AgCl} = 15.0 \text{ moles AgNO}_3 \times \frac{1 \text{ mole AgCl}}{1 \text{ mole AgNO}_3}\).
5. Conclude that the number of moles of AgCl produced is equal to the moles of AgNO_3 reacted, which is 15.0 moles.