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Let's take a look at the replacement reaction between silver nitrate ([tex]\( \text{AgNO}_3 \)[/tex]) and potassium sulfate ([tex]\( \text{K}_2\text{SO}_4 \)[/tex]). The balanced chemical equation for this reaction is:
[tex]\[ 2 \text{AgNO}_3 + K_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + 2 \text{KNO}_3 \][/tex]
To determine what else is produced during this reaction, we need to carefully analyze the products formed when the reactants combine.
### 1. Understanding the Reactants and Products:
- Reactants:
- [tex]\( \text{AgNO}_3 \)[/tex]: Silver nitrate
- [tex]\( \text{K}_2\text{SO}_4 \)[/tex]: Potassium sulfate
- Products:
- [tex]\( \text{Ag}_2\text{SO}_4 \)[/tex]: Silver sulfate
- [tex]\( \text{KNO}_3 \)[/tex]: Potassium nitrate (produced in a quantity of 2 moles per reaction unit)
### 2. Balancing the Chemical Equation:
The balanced reaction is given as:
[tex]\[ 2 \text{AgNO}_3 + K_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + 2 \text{KNO}_3 \][/tex]
This means that for every 2 moles of silver nitrate and 1 mole of potassium sulfate, we get 1 mole of silver sulfate and 2 moles of potassium nitrate.
### 3. Identifying the Produced Substances:
From the balanced equation, we can see the substances that are produced on the right-hand side:
1. Silver sulfate ([tex]\(\text{Ag}_2\text{SO}_4\)[/tex]): This is one of the products formed.
2. Potassium nitrate ([tex]\(\text{KNO}_3\)[/tex]): This is another product, and it is produced in double the amount of potassium sulfate (i.e., 2 moles of [tex]\(\text{KNO}_3\)[/tex] for every mole of [tex]\(\text{K}_2\text{SO}_4\)[/tex]). Therefore, we explicitly write it as [tex]\(2 \text{KNO}_3\)[/tex].
### Conclusion:
During the replacement reaction of silver nitrate and potassium sulfate, the substances produced are:
1. Silver sulfate ([tex]\(\text{Ag}_2\text{SO}_4\)[/tex])
2. Potassium nitrate ([tex]\(2 \text{KNO}_3\)[/tex])
Therefore, the products formed are [tex]\(\text{Ag}_2\text{SO}_4\)[/tex] and [tex]\(2 \text{KNO}_3\)[/tex].
[tex]\[ 2 \text{AgNO}_3 + K_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + 2 \text{KNO}_3 \][/tex]
To determine what else is produced during this reaction, we need to carefully analyze the products formed when the reactants combine.
### 1. Understanding the Reactants and Products:
- Reactants:
- [tex]\( \text{AgNO}_3 \)[/tex]: Silver nitrate
- [tex]\( \text{K}_2\text{SO}_4 \)[/tex]: Potassium sulfate
- Products:
- [tex]\( \text{Ag}_2\text{SO}_4 \)[/tex]: Silver sulfate
- [tex]\( \text{KNO}_3 \)[/tex]: Potassium nitrate (produced in a quantity of 2 moles per reaction unit)
### 2. Balancing the Chemical Equation:
The balanced reaction is given as:
[tex]\[ 2 \text{AgNO}_3 + K_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + 2 \text{KNO}_3 \][/tex]
This means that for every 2 moles of silver nitrate and 1 mole of potassium sulfate, we get 1 mole of silver sulfate and 2 moles of potassium nitrate.
### 3. Identifying the Produced Substances:
From the balanced equation, we can see the substances that are produced on the right-hand side:
1. Silver sulfate ([tex]\(\text{Ag}_2\text{SO}_4\)[/tex]): This is one of the products formed.
2. Potassium nitrate ([tex]\(\text{KNO}_3\)[/tex]): This is another product, and it is produced in double the amount of potassium sulfate (i.e., 2 moles of [tex]\(\text{KNO}_3\)[/tex] for every mole of [tex]\(\text{K}_2\text{SO}_4\)[/tex]). Therefore, we explicitly write it as [tex]\(2 \text{KNO}_3\)[/tex].
### Conclusion:
During the replacement reaction of silver nitrate and potassium sulfate, the substances produced are:
1. Silver sulfate ([tex]\(\text{Ag}_2\text{SO}_4\)[/tex])
2. Potassium nitrate ([tex]\(2 \text{KNO}_3\)[/tex])
Therefore, the products formed are [tex]\(\text{Ag}_2\text{SO}_4\)[/tex] and [tex]\(2 \text{KNO}_3\)[/tex].
Answer:
B. \( 2 KNO_3 \)
Explanation:
The balanced chemical equation for the reaction is:
\[ 2 AgNO_3 + K_2SO_4 \rightarrow Ag_2SO_4 + 2 KNO_3 \]
So, \( 2 KNO_3 \) is also produced during the replacement reaction of silver nitrate and potassium sulfate.
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