Select the nature or type of redox change in the following reactions:
(a) `2Cu^(+)rarrCu^(2+)+Cu^(0)`
(b) `Cl_(2)rarrClO^(-)+Cl^(-)`
(c ) `2KClO_(3)overset(Delta)rarr2KCl+3O_(2)`
(d) `(NH_(4))_(2)Cr_(2)O_(7)rarrN_(2)+Cr_(2)O_(3)+4H_(2)O`
(e ) `10FeSO_(4)+2KMnO_(4)+8H_(2)SO_(4)rarrK_(2)SO_(4)rarr2MnSO_(4)+5Fe_(2)(SO_(4))_(3)+K_(2)SO_(4)+8H_(2)O`
(f) `5H_(2)C_(2)O_(4)+2KMnO_(4)+3H_(2)SO_(4)rarrK_(2)SO_(4)+2MnSO_(4)+10CO_(2)+8H_(2)O`

Explanation

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