Answer:
(i) Let us
consider reaction between carbon and oxygen. Reducing Agent + Oxidising Agent
\[\underset{(Excess)}{\mathop{C(s)}}\,+\frac{1}{2}{{O}_{2}}(g)\to
\overset{+2}{\mathop{C}}\,\overset{-2}{\mathop{O}}\,\]
Lower state
of carbon
\[C(s)+\underset{(Excess)}{\mathop{{{O}_{2}}(g)}}\,\to
\overset{+4}{\mathop{C}}\,{{\overset{-4}{\mathop{O}}\,}_{2}}\]
Higher state of carbon
(ii) Let us consider the reaction between white phosphorous
(\[{{P}_{4}}\]) and\[C{{l}_{2}}(g)\].
Reducing agent + Oxidising agent
\[\underset{(Excess)}{\mathop{{{P}_{4}}(s)}}\,+3C{{l}_{2}}(g)\to
4\overset{+3-3}{\mathop{PC{{l}_{3}}}}\,\]
Lower oxidation state of phosphorous
\[{{P}_{4}}(s)+\underset{(Excess)}{\mathop{10C{{l}_{2}}(g)}}\,\to
4\overset{+5-5}{\mathop{PC{{l}_{5}}(g)}}\,\]
Higher oxidation of phosphorous
(iii) Let us consider the reaction between sulphur and oxygen.
Reducing agent + Oxidising agent
\[\underset{(Excess)}{\mathop{S}}\,+{{O}_{2}}\to
\overset{+4-4}{\mathop{S{{O}_{2}}}}\,\]
Lower oxidation state of sulphur
\[2S+3{{O}_{2}}\to
2\overset{+6-6}{\mathop{S{{O}_{3}}}}\,\]
Higher oxidation state of sulphur
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