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1.

Select the nature or type of redox change in the following reactions :(a) 2 Cu+ -----> Cu2+ + Cu0 (b) Cl2 ---------> ClO- + Cl- (c) 2KClO3  --------> 2KCl + 3O2 (d) (NH4)2 Cr2O7  -------> N2 + Cr2O3 + 4 H2O(e) 10FeSO4 + 2 KMnO4 + 8H2 SO4 ------> 2MnSO4 + 5 Fe2 (SO4)3 + K2 SO4 + 8H2 O(f) 5H2C2 O4 + 2KMnO4 + 3H2 SO4 ------> K2 SO4 + 2 MnSO4 + 10CO2 + 8H2O

Answer»

(i) (a) and (b) represents auto-redox or disproportionation in which same substance is oxidised and reduced as well.

(ii) (c) and (d) represents intramolecular redox change in which one element of a compound is oxidised and the other element is reduced.

(iii) (e) and (f) represents intermolecular redox in which one of the two reactant is oxidised and other is reduced.
Discussion
2.

Point out the oxidation number of C in the following : CH4, C3H8, C2H6, C4H10, CO, CO2 and HCO3 -, CO32-

Answer»

CH4 : -4 ;   C3H8: -8/3     C2H6:-3;    C4H10: - 10/4

CO : + 2 ;    CO2 : + 4 ;     HCO3- : + 4    CO32- : +4
Discussion