If 4.00 g of NaCl react with 10.00 g of AgNO3, what is the maximum mass of AgCl that can be formed?

• A. 6.74 g
• B. 4.00 g
• C. 8.45 g
• D. 10.00 g

Answer: (A)

Verified step by step guidance

1. Write the balanced chemical equation for the reaction: \(\mathrm{NaCl + AgNO_3 \rightarrow AgCl + NaNO_3}\).
2. Calculate the number of moles of each reactant using their molar masses: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\). For NaCl, use molar mass approximately 58.44 g/mol; for AgNO\(_3\), use molar mass approximately 169.87 g/mol.
3. Determine the limiting reactant by comparing the mole ratio of the reactants to the stoichiometric ratio from the balanced equation (which is 1:1). The reactant with fewer moles relative to the required ratio limits the reaction.
4. Calculate the moles of AgCl formed, which will be equal to the moles of the limiting reactant (since the ratio is 1:1).
5. Convert the moles of AgCl to mass using its molar mass (approximately 143.32 g/mol) with the formula: \(\text{mass} = \text{moles} \times \text{molar mass}\).