Let's take a closer look at the given chemical reaction and determine the correct products [tex]\( X \)[/tex] and [tex]\( Y \)[/tex].
The given reaction is:
[tex]\[ 2 \text{Al(OH)}_3 + 3 \text{H}_2\text{SO}_4 \rightarrow X + 6Y \][/tex]
We start by identifying the reactants and attempting to balance the reaction:
1. Reactants:
- Aluminum hydroxide ([tex]\(\text{Al(OH)}_3\)[/tex])
- Sulfuric acid ([tex]\(\text{H}_2\text{SO}_4\)[/tex])
2. Products: We need to determine [tex]\( X \)[/tex] and [tex]\( Y \)[/tex].
When aluminum hydroxide reacts with sulfuric acid, it forms aluminum sulfate and water. Let's outline the possible products:
- Aluminum sulfate: This compound is typically represented as [tex]\(\text{Al}_2(\text{SO}_4)_3\)[/tex].
- Water: Represented as [tex]\(\text{H}_2\text{O}\)[/tex].
3. Balancing the Reaction:
- We start with the balanced version of the aluminum sulfate formation:
[tex]\[ 2 \text{Al(OH)}_3 + 3 \text{H}_2\text{SO}_4 \rightarrow \text{Al}_2(\text{SO}_4)_3 + 6 \text{H}_2\text{O} \][/tex]
From the balanced reaction, we can see:
- [tex]\( X \)[/tex] should be [tex]\(\text{Al}_2(\text{SO}_4)_3\)[/tex] (aluminum sulfate), and
- [tex]\( Y \)[/tex] should be [tex]\(\text{H}_2\text{O}\)[/tex] (water).
Thus, the correct products are:
- [tex]\( X = \text{Al}_2(\text{SO}_4)_3 \)[/tex]
- [tex]\( Y = \text{H}_2\text{O} \)[/tex]
So, the correct option is:
[tex]\[ \boxed{X= \text{Al}_2\left( \text{SO}_4 \right)_3; Y= \text{H}_2\text{O}} \][/tex]
