NEETChemistryRedox Reactions
In the reaction given below: (A) ( H ₂ ~S _ (a) + Cl _ 2(a) 2 HCl _ (a) + S _ (a) ) (B) (3 Fe ₃ O _ 4(5) +8 Al _ (6) 9 Fe _ (4) +4 Al ₂ O _ 3(6) ) The related statements are: Statement-I : In (A) ( H ₂ ~S ) is oxidised because a more electronegative element ( Cl ₂ ) is added to hydrogen. Statement-II : In (B) Aluminium is oxidised because oxygen is added to it. Statement-III : In (B) Ferrous ferric oxide is reduced.
Options
- AStatement-I, II, III and IV are correct
- BStatement-I, II are correct but III and IV are incorrect
- CStatement-I, II, III and IV are incorrect
- DStatement-II, IV are incorrect but I and III are correct
Correct answer
D. Statement-II, IV are incorrect but I and III are correct
Step-by-step solution
- Statement I: Incorrect. ( H ₂ ~S ) is oxidized, but not because ( Cl ₂ ) is more electronegative. It's due to sulfur's oxidation state change. - Statement II: Incorrect. Aluminium is oxidized, but the reasoning is wrong. It's oxidized because it loses electrons, not just due to oxygen addition. - Statement III: Correct. ( Fe ₃ O ₄ ) (ferrous ferric oxide) is reduced to Fe. - Statement IV: Correct. Redox reactions involve both oxidation and reduction together. Individual redox reactions don't happen in isolation.