Suggest a scheme of classification of the following redox reactions:
$(a) N_{2(g)} + O_{2(g)} \rightarrow 2NO_{(g)}$
$(b) 2Pb(NO_3)_{2(s)} \rightarrow 2PbO_{(s)} + 4NO_{2(g)} + O_{2(g)}$
$(c) NaH_{(s)} + H_2O_{(l)} \rightarrow NaOH_{(aq)} + H_{2(g)}$
$(d) 2NO_{2(g)} + 2OH^{-}_{(aq)} \rightarrow NO_2^-(aq) + NO_3^-(aq) + H_2O_{(l)}$
$(a) N_{2(g)} + O_{2(g)} \rightarrow 2NO_{(g)}$
$(b) 2Pb(NO_3)_{2(s)} \rightarrow 2PbO_{(s)} + 4NO_{2(g)} + O_{2(g)}$
$(c) NaH_{(s)} + H_2O_{(l)} \rightarrow NaOH_{(aq)} + H_{2(g)}$
$(d) 2NO_{2(g)} + 2OH^{-}_{(aq)} \rightarrow NO_2^-(aq) + NO_3^-(aq) + H_2O_{(l)}$
(N/A) In reaction $(a)$,the compound nitric oxide is formed by the combination of elemental substances,nitrogen and oxygen; therefore,this is a combination redox reaction.
In reaction $(b)$,lead nitrate breaks down into three components; therefore,this is a decomposition redox reaction.
In reaction $(c)$,the hydrogen of water is displaced by the hydride ion to form dihydrogen gas; therefore,this is a displacement redox reaction.
In reaction $(d)$,$NO_2$ ($+4$ oxidation state) disproportionates into $NO_2^-$ ($+3$ oxidation state) and $NO_3^-$ ($+5$ oxidation state); therefore,this is a disproportionation redox reaction.
In reaction $(b)$,lead nitrate breaks down into three components; therefore,this is a decomposition redox reaction.
In reaction $(c)$,the hydrogen of water is displaced by the hydride ion to form dihydrogen gas; therefore,this is a displacement redox reaction.
In reaction $(d)$,$NO_2$ ($+4$ oxidation state) disproportionates into $NO_2^-$ ($+3$ oxidation state) and $NO_3^-$ ($+5$ oxidation state); therefore,this is a disproportionation redox reaction.
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$(a)$ $6 CO_{2(g)} + 6 H_{2}O_{(l)} \rightarrow C_{6}H_{12}O_{6(aq)} + 6 O_{2(g)}$
$(b)$ $O_{3(g)} + H_{2}O_{2(l)} \rightarrow H_{2}O_{(l)} + 2 O_{2(g)}$
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$(a)$ $6 CO_{2(g)} + 12 H_{2}O_{(l)} \rightarrow C_{6}H_{12}O_{6(aq)} + 6 H_{2}O_{(l)} + 6 O_{2(g)}$
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$(a)$ $6 CO_{2(g)} + 6 H_{2}O_{(l)} \rightarrow C_{6}H_{12}O_{6(aq)} + 6 O_{2(g)}$
$(b)$ $O_{3(g)} + H_{2}O_{2(l)} \rightarrow H_{2}O_{(l)} + 2 O_{2(g)}$
Why is it more appropriate to write these reactions as:
$(a)$ $6 CO_{2(g)} + 12 H_{2}O_{(l)} \rightarrow C_{6}H_{12}O_{6(aq)} + 6 H_{2}O_{(l)} + 6 O_{2(g)}$
$(b)$ $O_{3(g)} + H_{2}O_{2(l)} \rightarrow H_{2}O_{(l)} + O_{2(g)} + O_{2(g)}$
Also,suggest a technique to investigate the path of the above $(a)$ and $(b)$ redox reactions.
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