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Elements of Groups 16, 17 and 18 — Chemistry STD 12 Science — Question

Maharashtra BoardEnglish MediumSTD 12 ScienceChemistryElements of Groups 16, 17 and 183 Marks
Question
Ozone acts as an oxidising agent and a reducing agent. Explain with examples.
✓

Answer

$(A)$ Ozone as an oxidising agent : Since ozone decomposes to liberate nascent oxygen, it is a powerful oxidising agent next to fluorine.
$O _{3( g )} \rightarrow O _{2( g )}+ O$
For example :
It oxidises lead sulphide $(PbS)$ to lead sulphate $(PbSO_4)$ changing the oxidation state of $S$ from $-2$ to $+6$
$ PbS _{( s )}+4 O _{3( g )} \rightarrow PbSO _{( s )}+4 O _{2( g )}$
Potassium iodide, $KI$ is oxidised to iodine, $I_3$ in the solution.
$2 KI _{( aq )}+ H _3 O _{(1)}+ O _{3( g )} \rightarrow 2 KOH _{( aq )}+ I _{2( s )}+ O _{2( g )}$
Ozone oxidises nitrogen oxide to nitrogen dioxide.
$NO _{( g )}+ O _{3( g )} \rightarrow NO _{2( g )}+ O _{2( g )}$
$(B)$ Ozone as a reducing agent : Ozone reduces peroxides $(O^{1-})$ to oxides $(O^{2-}).$
Ozone reduces barium peroxide, $BaO_2$ to barium oxide, $BaO.$
$BaO_2 + O_3 \rightarrow BaO + 2O_2$
Ozone reduces hydrogen peroxide, $H_2O_2$ to water, $H_2O.$
$H_2O_2 + O_3 \rightarrow H_2O + 2O_2$

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