It states that matter can neither be created nor destroyed.
This law was put forth by Antoine Lavoisier in 1789 . He performed rections for reaching to the above conclusion. This law formed the for several later developments in chemistry . Infact , this was the result of exact measurement of masses of reactants and products, and carefully planned experiments performed by Lavoisier.
What weight of silver nitrate will react with 0.585 g NaCl to produce 1.435 g AgCl and 0.85 g `NaNO_(3)`

Answer

To solve the problem, we need to apply the law of conservation of mass, which states that the mass of reactants must equal the mass of products in a chemical reaction.

### Step-by-Step Solution:

1. **Identify the Reaction**:
The reaction between silver nitrate (AgNO₃) and sodium chloride (NaCl) can be written as:
\[ \text{AgNO}_3 + \text{NaCl} \rightarrow \text{AgCl} + \text{NaNO}_3 \]

2. **List the Given Masses**:
- Mass of NaCl = 0.585 g
- Mass of AgCl = 1.435 g
- Mass of NaNO₃ = 0.85 g
- Let the mass of AgNO₃ be \( x \) grams.

3. **Apply the Law of Conservation of Mass**:
According to the law, the mass of reactants equals the mass of products:
\[ \text{Mass of Reactants} = \text{Mass of Products} \]
This can be expressed as:
\[ x + \text{mass of NaCl} = \text{mass of AgCl} + \text{mass of NaNO}_3 \]

4. **Substitute the Known Values**:
Substitute the known masses into the equation:
\[ x + 0.585 = 1.435 + 0.85 \]

5. **Calculate the Right Side**:
First, calculate the total mass of the products:
\[ 1.435 + 0.85 = 2.285 \text{ g} \]

6. **Set Up the Equation**:
Now, we can set up the equation:
\[ x + 0.585 = 2.285 \]

7. **Solve for \( x \)**:
To find \( x \), subtract 0.585 from both sides:
\[ x = 2.285 - 0.585 \]
\[ x = 1.7 \text{ g} \]

8. **Conclusion**:
The mass of silver nitrate (AgNO₃) that will react with 0.585 g of NaCl is **1.7 g**.