How much mass of silver nitrates will react with 5.85 g of sodium chloride to produce 14.35 g of silver chloride and 8.5 g of sodium nitrates if law of conservation of mass is followed?

Options

A. 22.85 g
B. 108 g
C. 17.0 g
D. 28.70 g

Explanation

To solve the problem, we need to apply the law of conservation of mass, which states that mass cannot be created or destroyed in a chemical reaction. This means that the total mass of the reactants must equal the total mass of the products.

### Step-by-Step Solution:

1. **Identify the Given Data:**
- Mass of sodium chloride (NaCl) = 5.85 g
- Mass of silver chloride (AgCl) produced = 14.35 g
- Mass of sodium nitrate (NaNO3) produced = 8.5 g

2. **Write the Conservation of Mass Equation:**
According to the law of conservation of mass:
\[ \text{Mass of reactants} = \text{Mass of products} \]

Here, the reactants are silver nitrate (AgNO3) and sodium chloride (NaCl), and the products are silver chloride (AgCl) and sodium nitrate (NaNO3).

3. **Set Up the Equation:**
Let \( x \) be the mass of silver nitrate (AgNO3) that reacts. The equation can be set up as:
\[ x + \text{mass of NaCl} = \text{mass of AgCl} + \text{mass of NaNO3} \]
Substituting the known values:
\[ x + 5.85 \, \text{g} = 14.35 \, \text{g} + 8.5 \, \text{g} \]

4. **Calculate the Total Mass of Products:**
First, calculate the total mass of the products:
\[ 14.35 \, \text{g} + 8.5 \, \text{g} = 22.85 \, \text{g} \]

5. **Rearrange the Equation to Solve for \( x \):**
Now, rearranging the equation gives:
\[ x = 22.85 \, \text{g} - 5.85 \, \text{g} \]

6. **Perform the Calculation:**
\[ x = 22.85 \, \text{g} - 5.85 \, \text{g} = 17.00 \, \text{g} \]

7. **Conclusion:**
Therefore, the mass of silver nitrate (AgNO3) that will react is **17.00 g**.