`500 mL` of `0.2 M NaCl` sol. Is added to `100 mL` of `0.5 M AgNO_(3)` solution resulting in the formation white precipitate of `AgCl`. How many moles and how many grams of `AgCl` are formed? Which is the limiting reagent?

Explanation

To solve the problem, we need to determine the number of moles of AgCl formed and identify the limiting reagent in the reaction between NaCl and AgNO₃.

### Step 1: Write the balanced chemical equation
The reaction between sodium chloride (NaCl) and silver nitrate (AgNO₃) is a double displacement reaction that can be represented as:
\[ \text{NaCl} + \text{AgNO}_3 \rightarrow \text{NaNO}_3 + \text{AgCl} \]

### Step 2: Calculate the moles of NaCl and AgNO₃
1. **Calculate moles of NaCl:**
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