Question
Iron(III) Chloride reacts with Lead(II) Sulfate to undergo a double replacement reaction. Which of the following represents the correct chemical equation?
Group of answer choices
FeCl3 + PbSO4 ---> Fe2(SO4)3 + PbCl3
FeCl3 + PbSO4 ---> Fe(SO4)3 + PbCl2
FeCl3 + PbSO4 ---> FeSO4 + PbCl2
FeCl3 + PbSO4 ---> Fe2(SO4)3 + PbCl2
Group of answer choices
FeCl3 + PbSO4 ---> Fe2(SO4)3 + PbCl3
FeCl3 + PbSO4 ---> Fe(SO4)3 + PbCl2
FeCl3 + PbSO4 ---> FeSO4 + PbCl2
FeCl3 + PbSO4 ---> Fe2(SO4)3 + PbCl2
Answers
GPT-4o mini
To determine the correct chemical equation for the double replacement reaction between Iron(III) Chloride \( \text{FeCl}_3 \) and Lead(II) Sulfate \( \text{PbSO}_4 \), we must first identify the products of the reaction.
In a double replacement reaction, the cations and anions exchange partners. Here, the cation \( \text{Fe}^{3+} \) from \( \text{FeCl}_3 \) will pair with the anion \( \text{SO}_4^{2-} \) from \( \text{PbSO}_4 \) to potentially form Iron(III) Sulfate \( \text{Fe}_2(\text{SO}_4)_3 \), while Lead(II) \( \text{Pb}^{2+} \) will pair with Chloride \( \text{Cl}^- \) to potentially form Lead(II) Chloride \( \text{PbCl}_2 \).
Now, let's balance the equation:
1. \( \text{FeCl}_3 \) contains \( 1 \) iron and \( 3 \) chloride ions.
2. \( \text{PbSO}_4 \) contains \( 1 \) lead and \( 1 \) sulfate ion.
3. Iron(III) Sulfate \( \text{Fe}_2(\text{SO}_4)_3 \) requires \( 2 \) iron and \( 3 \) sulfate ions, meaning we need \( 2 \) moles of \( \text{FeCl}_3 \) to get \( 2 \) iron ions and \( 3 \) sulfate ions.
4. Therefore, we need \( 3 \) moles of \( \text{PbSO}_4 \) to provide the \( 3 \) sulfate ions.
The balanced equation would thus be:
\[
2 \text{FeCl}_3 + 3 \text{PbSO}_4 \rightarrow 1 \text{Fe}_2(\text{SO}_4)_3 + 3 \text{PbCl}_2
\]
Looking at your provided choices, the closest reaction template matching is:
\[
\text{FeCl}_3 + \text{PbSO}_4 \rightarrow \text{Fe}_2(\text{SO}_4)_3 + \text{PbCl}_2
\]
However, it should be noted that this reaction is not balanced as presented. None of the options provided are correctly balanced, but **the closest one** with correct formula standards for products formed would be:
**FeCl3 + PbSO4 ---> Fe2(SO4)3 + PbCl2.**
So, despite the imbalance, it's the only formula that reflects the formed products accurately.
In a double replacement reaction, the cations and anions exchange partners. Here, the cation \( \text{Fe}^{3+} \) from \( \text{FeCl}_3 \) will pair with the anion \( \text{SO}_4^{2-} \) from \( \text{PbSO}_4 \) to potentially form Iron(III) Sulfate \( \text{Fe}_2(\text{SO}_4)_3 \), while Lead(II) \( \text{Pb}^{2+} \) will pair with Chloride \( \text{Cl}^- \) to potentially form Lead(II) Chloride \( \text{PbCl}_2 \).
Now, let's balance the equation:
1. \( \text{FeCl}_3 \) contains \( 1 \) iron and \( 3 \) chloride ions.
2. \( \text{PbSO}_4 \) contains \( 1 \) lead and \( 1 \) sulfate ion.
3. Iron(III) Sulfate \( \text{Fe}_2(\text{SO}_4)_3 \) requires \( 2 \) iron and \( 3 \) sulfate ions, meaning we need \( 2 \) moles of \( \text{FeCl}_3 \) to get \( 2 \) iron ions and \( 3 \) sulfate ions.
4. Therefore, we need \( 3 \) moles of \( \text{PbSO}_4 \) to provide the \( 3 \) sulfate ions.
The balanced equation would thus be:
\[
2 \text{FeCl}_3 + 3 \text{PbSO}_4 \rightarrow 1 \text{Fe}_2(\text{SO}_4)_3 + 3 \text{PbCl}_2
\]
Looking at your provided choices, the closest reaction template matching is:
\[
\text{FeCl}_3 + \text{PbSO}_4 \rightarrow \text{Fe}_2(\text{SO}_4)_3 + \text{PbCl}_2
\]
However, it should be noted that this reaction is not balanced as presented. None of the options provided are correctly balanced, but **the closest one** with correct formula standards for products formed would be:
**FeCl3 + PbSO4 ---> Fe2(SO4)3 + PbCl2.**
So, despite the imbalance, it's the only formula that reflects the formed products accurately.