Question

10) Which of the statements about the reaction below are incorrect?
Fe2O3(5) + 3 CO(g) → 2Fe(s) + 3C02(8)
a) Iron is getting reduced
c) Carbon monoxide is getting oxidized.
b) Carbon dioxide is getting oxidized
d) Iron oxide is getting reduced.
i) a &b ii) a & C iii) c & d iv) all​

Answer 1

Answer:

The wrong statements are

a) Iron is getting reduced

b) Carbon dioxide is getting oxidized

Explanation:

Oxidation is defined as the loss of electrons by any species.

The gain of electrons by any species is called reduction.

The species that gain electron is called the oxidising agent and the one that loses or donate the electrons to the interacting element is called the reducing agent.

The oxidation state of Fe in Fe₂O₃ is +3. In the given reaction, Fe is undergoing reduction, i.e there is a decrease in positive charge (+3 state to 0 state). In CO, the carbon is in a +2 state, whereas in CO2 it is in a +4 state. Thus, there is an increase in positive charge. CO undergoes oxidation.

Since the oxidation number of Fe decreases from +3 to 0 but of C increases from +2 to +4, thus, here Fe₂O₃ is reduced whereas CO is oxidised.

Answer 2

Solution:

The wrong statements are a & b i.e.

1. Iron is getting reduced
2. carbon dioxide is getting oxidized.

Explanation:

1. Given reaction is a redox reaction.
2. Redox reactions are those in which both oxidation and reduction takes place.
3. Oxidation is defined as the loss of electrons by any species.
4. The gain of electrons by any species is called reduction.
5. The oxidation state of Fe in Fe₂O₃ is +3. In the given reaction, Fe is undergoing reduction, i.e. there is a decrease in positive charge (+3 state to 0 state).
6. In CO, the carbon is in a +2 state, whereas in CO2 it is in a +4 state. Thus, there is an increase in positive charge. CO undergoes oxidation.
7. Since the oxidation number of Fe decreases from +3 to 0 but of C increases from +2 to +4, thus, here Fe₂O₃ is reduced whereas CO is oxidized.