Calculation of Silver Chloride (AgCl) Formation from Silver Nitrate (AgNO3) and Aluminum Chloride (AlCl3)

When dealing with chemical reactions involving solid reactants, it is crucial to ensure proper stoichiometry and consider reactant solubility. This article explains the process of determining the mass of silver chloride (AgCl) formed in a reaction where 3.74 moles of silver nitrate (AgNO3) react with aluminum chloride (AlCl3). This calculation involves several key steps, including writing the balanced chemical equation, calculating the mole ratio, and determining the mass of the product.

Step 1: Balanced Chemical Equation

The balanced chemical equation for the reaction between silver nitrate and aluminum chloride is as follows:

3 AgNO3 AlCl3 → 3 AgCl Al(NO3)3

Step 2: Stoichiometry and Mole Ratio

From the balanced equation, we observe that 3 moles of AgNO3 react to produce 3 moles of AgCl. This indicates a 1:1 molar ratio between AgNO3 and AgCl. Given that we have 3.74 moles of AgNO3, the molar amount of AgCl formed will also be 3.74 moles.

Step 3: Calculation of Mass of AgCl

To find the mass of AgCl, we need to calculate its molar mass:

AgCl 107.87 g/mol (atomic mass of Ag) 35.45 g/mol (atomic mass of Cl) 143.32 g/mol

Using the number of moles of AgCl formed:

Mass of AgCl moles of AgCl × molar mass of AgCl

Mass of AgCl 3.74 moles × 143.32 g/mol ≈ 536.43 g

Thus, the mass of AgCl formed is approximately 536.43 grams.

Considerations for the Reaction

The given reaction traditionally occurs in a solvent, such as water, to dissolve the reactants and facilitate the chemical interaction. However, when dealing with solids, careful consideration must be given to the net reactant and the potential for a violent reaction between aluminum chloride (AlCl3) and water due to the formation of hydrogen chloride (HCl).

AlCl3 in Water

Aluminum chloride reacts aggressively with water, leading to the formation of aluminum hydroxide (Al(OH)3) and hydrogen chloride (HCl). The reaction can be represented as:

AlCl3(s) 6H2O(l) → [Al(H2O)6]3 (aq) 3 Cl-(aq)

Under these circumstances, the addition of AlCl3 to the solution should be done slowly to manage the exothermic reaction and the release of corrosive gases. Once the AlCl3 is dissolved, the remaining reaction (AgNO3 AlCl3 → AgCl Al(NO3)3) will proceed efficiently.

Conclusion

The balanced chemical equation is the cornerstone in chemical calculations. For the given problem, 3.74 moles of AgNO3 reacting with AlCl3 will produce 3.74 moles of AgCl, which corresponds to a mass of approximately 536.43 grams. Understanding the reaction dynamics and possible hazards is essential for practical applications, especially when dealing with reagents that react violently with water.