`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 step by step, we will follow these main steps:

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

### Step 2: Calculate the moles of NaCl
We have a solution of NaCl with a concentration of 0.2 M and a volume of 500 mL. To find the number of moles, we use the formula:
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