Certainly! Let's break down the process to determine how many moles of AgCl are formed during the reaction.
1. Write the balanced chemical equation:
[tex]\[
2 \, \text{AgNO}_3 (aq) + \text{MgCl}_2 (aq) \rightarrow 2 \, \text{AgCl} (s) + \text{Mg(NO}_3\text{)}_2 (aq)
\][/tex]
2. Identify stoichiometry between reactants and products:
According to the balanced equation, 2 moles of AgNO[tex]\(_3\)[/tex] react to produce 2 moles of AgCl. Therefore, the ratio of AgNO[tex]\(_3\)[/tex] to AgCl is 1:1.
3. Given data:
You have already determined that there are 0.0125 moles of AgNO[tex]\(_3\)[/tex] reacting.
4. Determine moles of AgCl formed:
Since the molar ratio of AgNO[tex]\(_3\)[/tex] to AgCl is 1:1, the moles of AgCl formed will be equal to the moles of AgNO[tex]\(_3\)[/tex] reacting.
Therefore, the moles of AgCl produced are:
[tex]\[
0.0125 \, \text{moles}
\][/tex]
So, the number of moles of AgCl formed during the reaction is [tex]\(0.0125 \, \text{moles}\)[/tex].
