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Question
Identify the redox reactions out of the following reactions and identify the oxidising and reducing agents in them.
\[\ce{4NH3 (g) + 3O2 (g) -> 2N2 (g) + 6H2O (g)}\]
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Solution
\[\ce{\overset{-3}{4N}\overset{+1}{H3} (g) + 3\overset{0}{O2} (g) -> 2\overset{0}{N}2 (g) + 6\overset{+1}{H2}\overset{-2}{O} (g)}\]
Here. O.N. of N increases from -3 (in \[\ce{NH3}\]) to 0 in \[\ce{(N2)}\] and therefore, \[\ce{NH3}\] acts as a reducing agent. O.N. of \[\ce{O}\] decreases from 0 (in \[\ce{O2}\]) to –2 (in \[\ce{H, O}\]), and therefore, \[\ce{O2}\] acts as an oxidizing agent.
Thus, reaction is a redox reaction.
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