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 will use the law of conservation of mass, which states that the mass of the reactants must equal the mass of the products.

### Step-by-Step Solution:

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

2. **Set Up the Conservation of Mass Equation**:
According to the law of conservation of mass:
\[ \text{Mass of reactants} = \text{Mass of products} \]
The reactants in this case are silver nitrate (AgNO3) and sodium chloride (NaCl), and the products are silver chloride (AgCl) and sodium nitrate (NaNO3).

3. **Express the Mass of Silver Nitrate**:
Let the mass of silver nitrate be \( X \) g. Therefore, the total mass of the reactants can be expressed as:
\[ X + 5.85 \text{ g (mass of NaCl)} \]

4. **Calculate the Total Mass of Products**:
The total mass of the products is the sum of the masses of silver chloride and sodium nitrate:
\[ 14.35 \text{ g (mass of AgCl)} + 8.5 \text{ g (mass of NaNO3)} = 22.85 \text{ g} \]

5. **Set Up the Equation**:
Now we can set up the equation based on the conservation of mass:
\[ X + 5.85 = 22.85 \]

6. **Solve for \( X \)**:
Rearranging the equation gives:
\[ X = 22.85 - 5.85 \]
\[ X = 17 \text{ g} \]

7. **Conclusion**:
The mass of silver nitrate (AgNO3) that will react is 17 g.

### Final Answer:
The mass of silver nitrate that will react is **17 g**.