Answer:
(a) \[\overset{0}{\mathop{{{N}_{2}}}}\,(g)+\overset{0}{\mathop{{{O}_{2}}}}\,(g)\to
\overset{+2-2}{\mathop{2NO}}\,(g)\]
It is a combination (combustion) type of redox reaction.
(b) \[2\overset{+2}{\mathop{Pb}}\,\overset{+5-2}{\mathop{{{(N{{O}_{3}})}_{2}}}}\,(s)\to
\overset{+2-2}{\mathop{2PbO(s)}}\,+2\overset{+4-2}{\mathop{N{{O}_{2}}(g)}}\,+\frac{1}{2}\overset{0}{\mathop{{{O}_{2}}}}\,(g)\]
It is also a redox reaction involving decomposition of lead
nitrate.
(c) \[\overset{+1-1}{\mathop{NaH(s)}}\,+\overset{+1-2}{\mathop{{{H}_{2}}O(l)}}\,\to
\overset{+1-2+1}{\mathop{NaOH}}\,(aq)+\overset{0}{\mathop{{{H}_{2}}}}\,(g)\]
It is a displacement type of redox reaction in which hydrogen
of water is displaced by a hydride ion into dihydrogen gas.
(d)\[2\,\overset{+4}{\mathop{N}}\,{{\overset{-2}{\mathop{O}}\,}_{2}}+2\overset{-2}{\mathop{O}}\,\overset{+1}{\mathop{{{H}^{-}}\to
}}\,\overset{+3}{\mathop{N}}\,\overset{-2}{\mathop{O_{2}^{-}}}\,\,(aq)+\overset{+5}{\mathop{N}}\,\overset{-2}{\mathop{O_{3}^{-}}}\,\,(aq)\]\[+{{H}_{2}}O(l)\]
It is disproportionation in which
the oxidation state of nitrogen changes from +4 to +3 and +5.
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