To analyze the balanced redox reaction \( \text{Fe}_2\text{O}_3(s) + 2\text{Al}(s) \rightarrow \text{Al}_2\text{O}_3(s) + 2\text{Fe}(l) \), let's address each question one by one:
l. What is the oxidation state of 2Al(s)?
- The oxidation state of pure elemental aluminum (Al) is 0. Therefore, for \( 2\text{Al}(s) \), it remains 0.
m. What is the oxidation state of Fe in Fe2O3(s)?
- In \( \text{Fe}_2\text{O}_3 \), there are two iron (Fe) atoms. Let the oxidation state of iron be \( x \). The oxidation state of oxygen is usually -2. The equation can be set up as follows: \[ 2x + 3(-2) = 0 \implies 2x - 6 = 0 \implies 2x = 6 \implies x = +3 \]
- Therefore, the oxidation state of Fe in \( \text{Fe}_2\text{O}_3 \) is +3.
n. What is the oxidation state of O in Fe2O3(s)?
- As established previously, the oxidation state of oxygen (O) in \( \text{Fe}_2\text{O}_3 \) is -2.
o. What is the oxidation state of 2Fe(l)?
- The oxidation state of elemental iron (Fe) in its liquid state is also 0. Therefore, for \( 2\text{Fe}(l) \), it remains 0.
p. What is the oxidation state of Al in Al2O3(s)?
- In \( \text{Al}_2\text{O}_3 \), let the oxidation state of aluminum (Al) be \( y \). The equation can be set up as follows: \[ 2y + 3(-2) = 0 \implies 2y - 6 = 0 \implies 2y = 6 \implies y = +3 \]
- Therefore, the oxidation state of Al in \( \text{Al}_2\text{O}_3 \) is +3.
q. What is the oxidation state of O in Al2O3(s)?
- As in \( \text{Fe}_2\text{O}_3 \), the oxidation state of oxygen (O) in \( \text{Al}_2\text{O}_3 \) is -2.
r. What is the element that is oxidized?
- Oxidation is the loss of electrons. In this reaction, aluminum (Al) is oxidized from an oxidation state of 0 to +3. Al is the element that is oxidized.
s. What is the element that is reduced?
- Reduction is the gain of electrons. In this reaction, iron (Fe) is reduced from an oxidation state of +3 in \( \text{Fe}_2\text{O}_3 \) to 0 in elemental \( \text{Fe} \). Fe is the element that is reduced.
t. What is the oxidizing agent?
- The oxidizing agent is the species that is reduced. In this reaction, the oxidizing agent is Fe2O3.
u. What is the reducing agent?
- The reducing agent is the species that is oxidized. In this reaction, the reducing agent is Al.
v. How many electrons are transferred in the reaction as it is balanced?
- Each aluminum atom loses 3 electrons (oxidation from 0 to +3), and since there are 2 aluminum atoms, the total number of electrons lost is: \[ 2 \times 3 = 6 \text{ electrons} \]
- Therefore, 6 electrons are transferred in the reaction.
In summary:
- l: 0
- m: +3
- n: -2
- o: 0
- p: +3
- q: -2
- r: Al
- s: Fe
- t: Fe2O3
- u: Al
- v: 6 electrons
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