Fluorine reacts with ice and results in the change :
`H_(2)O_((s))+F_(2(g))toHF_((g))+HOF_((g))`
Justify that this reaction is a redox reaction.

Explanation

`overset(+1)(H_(2))overset(-2)(O_((s)))+overset(0)(F_(2(g)))tooverset(+1)(H)overset(-1)(F_((g)))+overset(+1)(H)overset(-2)(O)overset(+1)(F_((g)))`
Oxidation number of F in `F_(2)` reduces from 0 to -1 and in HOF is +1. Therefore F gets reduced as well as oxidized.
Therefore it is disproportionate redox reactions.