Fluorine reacts with ice and results in the change:
`H_(2)O(s)+F_(2)(g) rarr HF(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)rarroverset(+1)Hoverset(-1)F+overset(+1)Hoverset(-2)Ooverset(+1)F`
In this case, `F_2` is reduced to HF and oxidised to HOF. Therefore , it redox reaction , HOF is unstable and decomposes to from `O_2` and HF.
`2overset(+1)(H)overset(-2)Ooverset(+1)Frarr2overset(+1)H" "overset(-1)F+overset0O`
In this reaction, F of HOF is reduced while O of HOF is oxidised . Therefore , it is a redox reaction but not a disproportionation reaction . If oxygen of HOF disproportionate then oxygen must show three oxidation states . If we assume that oxidation state of O is zero in HOF, the its oxidation state decreases to -2 . HOF is reduced to `H_2O` and increases to +2 if if HOF gets oxidised to `OF_2` .
Therefore , the possible reaction is
`2overset(+1)(H)overset(0)Ooverset(-1)Frarroverset(+1)(H_2)overset(-2)O+overset(+2)Ooverset(-1)(F_2)`