Silver nitrate, AgNO3, reacts with ferric chloride, FeCl3, to give silver chloride, AgCl and ferric nitrate, Fe(NO3)3. In a particular experiment, it was planned to mix a solution containing 25.0 g of AgNO3 with another solution containing 45.0 grams of FeCl3. Determine the mass of iodine AgCl that could be produced.

a. Which reactant is the limiting reagent and excess reactant?
b. How many grams of AgCl are formed?
c. How much of the excess reactant remains after the reaction?

Gresa format

To solve this problem, we'll use the **GRESA format** (Given, Required, Equation, Solution, Answer). Let's break it down step by step.

### 1. **Given:**
- **Mass of AgNO₃** = 25.0 g
- **Mass of FeCl₃** = 45.0 g
- **Molar masses**:
  - **AgNO₃** = 169.87 g/mol
  - **FeCl₃** = 162.2 g/mol
  - **AgCl** = 143.32 g/mol

### 2. **Required:**
We need to find:
- a. The limiting reagent and excess reagent.
- b. The mass of AgCl formed.
- c. The amount of excess reactant remaining after the reaction.

### 3. **Equation:**
The balanced chemical equation is:

\[
3 \text{AgNO₃} + \text{FeCl₃} \rightarrow 3 \text{AgCl} + \text{Fe(NO₃)₃}
\]

This tells us that **3 moles of AgNO₃** react with **1 mole of FeCl₃** to produce **3 moles of AgCl**.

### 4. **Solution:**

#### Step 1: Calculate the moles of each reactant.
- Moles of AgNO₃:
\[
\text{Moles of AgNO₃} = \frac{25.0 \, \text{g}}{169.87 \, \text{g/mol}} \approx 0.1472 \, \text{mol}
\]
  
- Moles of FeCl₃:
\[
\text{Moles of FeCl₃} = \frac{45.0 \, \text{g}}{162.2 \, \text{g/mol}} \approx 0.2774 \, \text{mol}
\]

#### Step 2: Determine the limiting reactant.
From the balanced equation, 3 moles of AgNO₃ react with 1 mole of FeCl₃, so we compare their molar ratio.

For **AgNO₃**:  
We need \(\frac{1}{3} \times 0.1472 = 0.0491\) moles of FeCl₃ to react with 0.1472 moles of AgNO₃.

For **FeCl₃**:  
We need \(3 \times 0.2774 = 0.832\) moles of AgNO₃ to react with 0.2774 moles of FeCl₃.

Since we have only 0.1472 moles of AgNO₃ (and need 0.832), **AgNO₃** is the limiting reagent, and **FeCl₃** is in excess.

#### Step 3: Calculate the amount of AgCl formed.
From the balanced equation, 3 moles of AgNO₃ produce 3 moles of AgCl. Therefore, the moles of AgCl formed are the same as the moles of AgNO₃.

\[
\text{Moles of AgCl} = \text{Moles of AgNO₃} = 0.1472 \, \text{mol}
\]

Now, calculate the mass of AgCl:

\[
\text{Mass of AgCl} = 0.1472 \, \text{mol} \times 143.32 \, \text{g/mol} \approx 21.10 \, \text{g}
\]

#### Step 4: Calculate the excess FeCl₃ remaining.
We already know that 0.0491 moles of FeCl₃ are required to react with the 0.1472 moles of AgNO₃. 

Moles of FeCl₃ remaining:
\[
\text{Moles of FeCl₃ remaining} = 0.2774 \, \text{mol} - 0.0491 \, \text{mol} = 0.2283 \, \text{mol}
\]

Convert the remaining moles of FeCl₃ to grams:
\[
\text{Mass of FeCl₃ remaining} = 0.2283 \, \text{mol} \times 162.2 \, \text{g/mol} \approx 37.0 \, \text{g}
\]

### 5. **Answer:**
- a. **Limiting reagent**: AgNO₃, **Excess reagent**: FeCl₃
- b. **Mass of AgCl formed**: 21.10 g
- c. **Mass of FeCl₃ remaining**: 37.0 g

Would you like any more details or have further questions? Here are five related questions:

1. What happens if the amount of AgNO₃ is increased?
2. How do you determine the molar mass of compounds?
3. Why does the limiting reagent determine the amount of product formed?
4. How would the reaction change if FeCl₃ were the limiting reagent?
5. What is the significance of a balanced chemical equation?

**Tip**: Always check the stoichiometric ratio from the balanced equation to find the limiting reagent.

Silver nitrate, AgNO3, reacts with ferric chloride, FeCl3, to give silver chloride, AgCl and ferric nitrate, Fe(NO3)3. In a particular experiment, it was planned to mix a solution containing 25.0 g of AgNO3 with another solution containing 45.0 grams of FeCl3. Determine the mass of AgCl that could be produced.

 a. Which reactant is the limiting reagent and excess reactant?
 b. How many grams of AgCl are formed?
 c. How much of the excess reactant remains after the reaction?

Learn how to determine the limiting reagent, calculate the mass of AgCl formed, and the excess reactant remaining in a reaction between AgNO3 and FeCl3. This stoichiometry problem involves molar mass calculations and is suitable for high school chemistry students.

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