Sure, let's break down each reaction you have provided and categorize the reactants and products.
### 1. Reaction:
[tex]\[
K_2SO_4(aq) + Ba(NO_3)_2(aq) \rightarrow 2KNO_3(aq) + BaSO_4(s)
\][/tex]
In this reaction, we have:
#### Reactants:
- [tex]\( K_2SO_4 \)[/tex] (Potassium sulfate) in aqueous form (aq)
- [tex]\( Ba(NO_3)_2 \)[/tex] (Barium nitrate) in aqueous form (aq)
#### Products:
- [tex]\( 2KNO_3 \)[/tex] (Potassium nitrate) in aqueous form (aq)
- [tex]\( BaSO_4 \)[/tex] (Barium sulfate) in solid form (s)
### 2. Reaction:
[tex]\[
FeCl_2(aq) + Ba_3(PO_4)_2(aq) \rightarrow Fe_3(PO_4)_2(s) + NaCl(aq)
\][/tex]
This reaction has a mistake: the product [tex]\(NaCl\)[/tex] should actually be [tex]\(FeCl_3\)[/tex] to balance the equation correctly. Also, the correct formula for [tex]\(Ba_3(PO_4)_2\)[/tex] should be [tex]\(Fe_3(PO_4)_2\)[/tex].
Considering the corrected reaction:
[tex]\[
3FeCl_2(aq) + 2Ba_3(PO_4)_2(aq) \rightarrow Fe_3(PO_4)_2(s) + 6BaCl_2(aq)
\][/tex]
In this reaction, we have:
#### Reactants:
- [tex]\( 3FeCl_2 \)[/tex] (Iron(II) chloride) in aqueous form (aq)
- [tex]\( 2Ba_3(PO_4)_2 \)[/tex] (Barium phosphate) in aqueous form (aq)
#### Products:
- [tex]\( Fe_3(PO_4)_2 \)[/tex] (Iron(II) phosphate) in solid form (s)
- [tex]\( 6BaCl_2 \)[/tex] (Barium chloride) in aqueous form (aq)
### Tables
#### 1. First Reaction:
[tex]\[
\begin{array}{|c|c|c|}
\hline
\text{Reactants} & \text{Element} & \text{Products} \\
\hline
K_2SO_4(aq) & K & 2KNO_3(aq) \\
Ba(NO_3)_2(aq) & N & BaSO_4(s) \\
& O & \\
& S & \\
& Ba & \\
\hline
\end{array}
\][/tex]
#### 2. Second Reaction:
[tex]\[
\begin{array}{|c|c|c|}
\hline
\text{Reactants} & \text{Element} & \text{Products} \\
\hline
3FeCl_2(aq) & Fe & Fe_3(PO_4)_2(s) \\
2Ba_3(PO_4)_2(aq) & Cl & 6BaCl_2(aq) \\
& P & \\
& O & \\
& Ba & \\
\hline
\end{array}
\][/tex]
These pairwise balanced reactions address both the reactants and products, categorizing them accordingly based on their forms and the elements they contain.
