$1\cdot7\text{ g}$ of silver nitrate is dissolved in $100\text{ g}$ of water, and $0\cdot585\text{ g}$ of sodium chloride is dissolved in $100\text{ g}$ of water. Both are mixed and a chemical reaction occurs. $1\cdot435\text{ g}$ of silver chloride and $0\cdot85\text{ g}$ of sodium nitrate are formed. Which law of chemical combination is shown by the above reaction?

Question

Prepp Team · Accepted Answer

Understanding the Chemical Reaction Data

This question asks to identify the law of chemical combination demonstrated by the reaction between silver nitrate and sodium chloride, based on the given masses of reactants and products.

Calculating Total Reactant Mass

First, calculate the total mass of the reactants used in the reaction.

Mass of Silver Nitrate ($\text{AgNO}_3$) = $1.7\text{ g}$
Mass of Sodium Chloride ($\text{NaCl}$) = $0.585\text{ g}$

Total Reactant Mass = Mass of $\text{AgNO}_3$ + Mass of $\text{NaCl}$

$ \text{Total Reactant Mass} = 1.7\text{ g} + 0.585\text{ g} = 2.285\text{ g} $

Calculating Total Product Mass

Next, calculate the total mass of the products formed.

Mass of Silver Chloride ($\text{AgCl}$) = $1.435\text{ g}$
Mass of Sodium Nitrate ($\text{NaNO}_3$) = $0.85\text{ g}$

Total Product Mass = Mass of $\text{AgCl}$ + Mass of $\text{NaNO}_3$

$ \text{Total Product Mass} = 1.435\text{ g} + 0.85\text{ g} = 2.285\text{ g} $

Analyzing Mass Conservation

Compare the total mass of reactants and products.

Total Reactant Mass = $2.285\text{ g}$
Total Product Mass = $2.285\text{ g}$

Since the total mass of reactants is equal to the total mass of products ($2.285\text{ g} = 2.285\text{ g}$), the reaction demonstrates the Law of Conservation of Mass. This law states that mass is neither created nor destroyed during a chemical reaction.