Let's solve this problem step-by-step to determine how many moles of \(AgCl\) can be formed from the given amount of \(NaCl\):
1. Identify the key information:
- Volume of \(NaCl\) solution \((V) = 35.0\) mL
- Molarity of \(NaCl\) solution \((M) = 1.00\) M
2. Convert the volume of \(NaCl\) solution from milliliters to liters:
[tex]\[
V_{NaCl} = 35.0 \, \text{mL} \times \frac{1 \, \text{L}}{1000 \, \text{mL}} = 0.0350 \, \text{L}
\][/tex]
3. Calculate the moles of \(NaCl\) using its molarity and volume:
[tex]\[
\text{Moles of NaCl} = M \times V_{NaCl}
\][/tex]
Plugging in the values:
[tex]\[
\text{Moles of NaCl} = 1.00 \, \text{M} \times 0.0350 \, \text{L} = 0.035 \, \text{moles}
\][/tex]
4. Determine the moles of \(AgCl\) that can form:
The reaction between \(AgNO_3\) and \(NaCl\) is given by:
[tex]\[
AgNO_3 + NaCl \rightarrow AgCl + NaNO_3
\][/tex]
The stoichiometry of the reaction shows a 1:1 molar ratio between \(NaCl\) and \(AgCl\). Thus, the moles of \(NaCl\) will be directly converted to moles of \(AgCl\).
5. Moles of \(AgCl\) that can form:
[tex]\[
\text{Moles of AgCl} = \text{Moles of NaCl} = 0.035 \, \text{moles}
\][/tex]
So, the number of moles of [tex]\(AgCl\)[/tex] that can form from the [tex]\(NaCl\)[/tex] is [tex]\(\boxed{0.035}\)[/tex] moles.
