Choose the disproportionation reaction among the following redox reactions.

Options

A. `3 Mg (s) + N_(2)(g)rarrMg_(3)N_(2)(s)`
B. `P_(4)(s)+3NaOH(aq)+3H_(2)O(l)rarrPH_(3)(g)+3NaH_(2)PO_(2)(aq)`
C. `Cl_(2)(g)+2KI(aq)rarr2KCl(Aq)+I_(2)(s)`
D. `Cr_(2)O_(3)(s)+2Al(s)rarrAl_(2)O_(3)(s)+2Cr`

Answer

b

Explanation

In reaction (b) `P_(4)` is both reduced to `PH_(3)` and oxidised to `NaH_(2)PO_(2)` thus it is a disproportion nation reaction but in all other redox reaction different speiced are oxidised / reduced i.e in reactoin(a) Mg is oxidised but `N_(2)` is reduced reaction (c ) `COI_(2)` is reduced AI is oxidised while in reaction (e ) `Na^(+)` is reduced but `H^(-)` oxidised