Let's solve each question step by step:
### Question 9:
In the reaction:
[tex]\[ \text{TiCl}_4(l) + \text{O}_2(g) \rightarrow \text{TiO}_2(s) + 2 \text{Cl}_2(g) \][/tex]
We need to determine which species is reduced. Reduction involves a decrease in oxidation state.
1. Determine the oxidation states:
- In [tex]\(\text{TiCl}_4\)[/tex]: Ti is +4 (since Cl is -1 and there are 4 Cl atoms, total Cl oxidation state is -4).
- In [tex]\(\text{TiO}_2\)[/tex]: Ti remains +4 (since O is -2, and with 2 O atoms, total O oxidation state is -4).
- In [tex]\(\text{O}_2\)[/tex]: O is 0.
- In [tex]\(\text{Cl}_2\)[/tex]: Cl is 0.
2. Identify changes in oxidation states:
- Cl in [tex]\(\text{TiCl}_4\)[/tex] is -1 and changes to 0 in [tex]\(\text{Cl}_2\)[/tex].
- Ti remains +4.
- O remains 0 in [tex]\(\text{O}_2\)[/tex] and -2 in [tex]\(\text{TiO}_2\)[/tex].
Since reduction involves a decrease in oxidation state, the species reduced is:
- The Cl in [tex]\(\text{TiCl}_4\)[/tex] changes from -1 to 0.
Hence, the correct answer is:
The Cl in [tex]\(\text{TiCl}_4\)[/tex]
### Question 10:
In the reaction:
[tex]\[ 5 \text{Fe}^{2+}(aq) + \text{MnO}_4^-(aq) + 8 \text{H}^+(aq) \rightarrow 5 \text{Fe}^{3+}(aq) + \text{Mn}^{2+}(aq) + 4 \text{H}_2\text{O}(l) \][/tex]
We need to determine the reducing agent. The reducing agent is the species that gets oxidized (loses electrons) in the reaction.
1. Determine the changes in oxidation states:
- Fe in [tex]\(\text{Fe}^{2+}\)[/tex] has an oxidation state of +2 and changes to +3 in [tex]\(\text{Fe}^{3+}\)[/tex].
- Mn in [tex]\(\text{MnO}_4^-\)[/tex] has an oxidation state of +7 (MnO4-: typically Mn is +7, O is -2 each) and changes to +2 in [tex]\(\text{Mn}^{2+}\)[/tex].
2. Identify the oxidized species:
- Fe goes from +2 to +3, indicating it is oxidized.
Therefore, the reducing agent (the one being oxidized) is:
Fe2+
The correct answers to the questions are:
- For Question 9: The Cl in [tex]\(\text{TiCl}_4\)[/tex]
- For Question 10: [tex]\(\text{Fe}^{2+}\)[/tex]
