Let's break down the balanced redox reaction:
\[ \text{Fe}_2\text{O}_3(s) + 2\text{Al}(s) \rightarrow \text{Al}_2\text{O}_3(s) + 2\text{Fe}(l) \]
Now let's answer each of your questions:
l. What is the oxidation state of 2Al(s)?
- The oxidation state of elemental aluminum (Al) in its solid form (Al(s)) is 0. Therefore, for 2Al(s), it is still 0.
m. What is the oxidation state of Fe in Fe2O3(s)?
- In Fe₂O₃, let the oxidation state of Fe be \( x \). We have: \[ 2x + 3(-2) = 0 \implies 2x - 6 = 0 \implies 2x = 6 \implies x = +3 \]
- So, the oxidation state of Fe in Fe₂O₃(s) is +3.
n. What is the oxidation state of O in Fe2O3(s)?
- The oxidation state of oxygen (O) in Fe₂O₃ is typically -2.
o. What is the oxidation state of 2Fe(l)?
- The oxidation state of elemental iron (Fe) in its liquid form (Fe(l)) is 0. Thus, for 2Fe(l), it is 0.
p. What is the oxidation state of Al in Al2O3(s)?
- In Al₂O₃, let the oxidation state of Al be \( y \). We have: \[ 2y + 3(-2) = 0 \implies 2y - 6 = 0 \implies 2y = 6 \implies y = +3 \]
- So, the oxidation state of Al in Al₂O₃(s) is +3.
q. What is the oxidation state of O in Al2O3(s)?
- The oxidation state of oxygen (O) in Al₂O₃ is -2.
r. What is the element that is oxidized?
- Oxidation is the process of losing electrons. In this reaction, aluminum (Al) is oxidized from 0 in Al(s) to +3 in Al₂O₃(s). So, Al is the element that is oxidized.
s. What is the element that is reduced?
- Reduction is the process of gaining electrons. In this reaction, iron (Fe) is reduced from +3 in Fe₂O₃(s) to 0 in Fe(l). So, Fe is the element that is reduced.
t. What is the oxidation agent?
- The substance that causes oxidation (is itself reduced) is the oxidizing agent. Since Fe₂O₃ contains Fe and is being reduced, Fe₂O₃ is the oxidizing agent.
u. What is the reducing agent?
- The substance that causes reduction (is itself oxidized) is the reducing agent. In this case, aluminum (Al) is being oxidized, so Al is the reducing agent.
v. How many electrons are transferred in the reaction as it is balanced?
- For each aluminum (Al) atom, 3 electrons are transferred (from 0 to +3). For 2 aluminum atoms, the total transfer is \( 2 \times 3 = 6 \) electrons. Therefore, 6 electrons are transferred in the reaction.
Summary of Answers:
- 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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