To solve this question, let's analyze the given balanced chemical equation for the reaction between silver nitrate (AgNO[tex]\(_3\)[/tex]) and potassium sulfate (K[tex]\(_2\)[/tex]SO[tex]\(_4\)[/tex]):
[tex]\[
2 \, \text{AgNO}_3 + \text{K}_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + 2 \, \text{KNO}_3
\][/tex]
Steps of Analysis:
1. Identify the reactants and products:
- Reactants: Silver nitrate (AgNO[tex]\(_3\)[/tex]) and potassium sulfate (K[tex]\(_2\)[/tex]SO[tex]\(_4\)[/tex]).
- Products: Silver sulfate (Ag[tex]\(_2\)[/tex]SO[tex]\(_4\)[/tex]) and potassium nitrate (KNO[tex]\(_3\)[/tex]).
2. Examine the stoichiometry of the reaction:
- From the equation, you can see that 2 moles of AgNO[tex]\(_3\)[/tex] react with 1 mole of K[tex]\(_2\)[/tex]SO[tex]\(_4\)[/tex]).
- This forms 1 mole of Ag[tex]\(_2\)[/tex]SO[tex]\(_4\)[/tex] and 2 moles of KNO[tex]\(_3\)[/tex]).
3. Determine the additional product besides Ag[tex]\(_2\)[/tex]SO[tex]\(_4\)[/tex]:
- According to the balanced equation, besides forming Ag[tex]\(_2\)[/tex]SO[tex]\(_4\)[/tex], the reaction also produces 2 moles of potassium nitrate (KNO[tex]\(_3\)[/tex]).
Thus, the other product formed in the reaction is 2 moles of potassium nitrate (KNO[tex]\(_3\)[/tex]). Therefore, the correct choice is:
[tex]\[
\boxed{2 \, \text{KNO}_3}
\][/tex]
