Let's break down the problem step by step to determine the incorrect statements about the given reaction:
[tex]\[ 2PbO(s) + C(s) \rightarrow 2Pb(s) + CO_2(g) \][/tex]
1. Statement (a): Lead is getting reduced
- Reduction is the gain of electrons, often resulting in a decrease in oxidation state.
- Lead in lead oxide ([tex]\(PbO\)[/tex]) has an oxidation state of +2.
- Lead in elemental form ([tex]\(Pb\)[/tex]) has an oxidation state of 0.
- As [tex]\(PbO\)[/tex] is transforming to [tex]\(Pb\)[/tex], the oxidation state decreases from +2 to 0. This indicates that lead is indeed getting reduced.
- Therefore, statement (a) is correct.
2. Statement (b): Carbon dioxide is getting oxidized
- Oxidation is the loss of electrons, often resulting in an increase in oxidation state.
- Carbon dioxide ([tex]\(CO_2\)[/tex]) is a product of the reaction.
- In [tex]\(CO_2\)[/tex], carbon has an oxidation state of +4.
- Since [tex]\(CO_2\)[/tex] is formed as a product, there is no change occurring in [tex]\(CO_2\)[/tex] itself within the context of this reaction.
- Therefore, it is incorrect to say that carbon dioxide is getting oxidized during this reaction.
- Statement (b) is incorrect.
3. Statement (c): Carbon is getting oxidised
- Oxidation is the loss of electrons.
- Carbon in its elemental form ([tex]\(C\)[/tex]) has an oxidation state of 0.
- In [tex]\(CO_2\)[/tex], carbon has an oxidation state of +4.
- As carbon transforms from elemental [tex]\(C\)[/tex] to [tex]\(CO_2\)[/tex], its oxidation state increases from 0 to +4, indicating that carbon is being oxidized.
- Therefore, statement (c) is correct.
4. Statement (d): Lead oxide is getting oxidized
- Lead oxide ([tex]\(PbO\)[/tex]) is being transformed in the reaction.
- Lead in [tex]\(PbO\)[/tex] has an oxidation state of +2.
- Lead in the product lead ([tex]\(Pb\)[/tex]) has an oxidation state of 0.
- Since [tex]\(PbO\)[/tex] is losing oxygen and lead's oxidation state is decreasing from +2 to 0, [tex]\(PbO\)[/tex] is undergoing reduction, not oxidation.
- Therefore, statement (d) is incorrect.
From the analysis above, the incorrect statements are (b) and (d).
Next, consider the second reaction:
[tex]\[ Fe_2O_3 + 2Al \rightarrow Al_2O_3 + 2Fe \][/tex]
This reaction is known as a thermite reaction, where a more reactive metal (aluminum) reduces the oxide of a less reactive metal (iron). The aluminum replaces the iron, forming aluminum oxide and elemental iron. This type of reaction is an example of a redox reaction (reduction-oxidation reaction), where reduction and oxidation occur simultaneously.
In conclusion:
- The incorrect statements about the first reaction are (b) and (d).
- The reaction [tex]\[ Fe_2O_3 + 2Al \rightarrow Al_2O_3 + 2Fe \][/tex] is an example of a redox reaction.
