The following reaction is an example of a:4 N | vedclass

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(B) $1$. Analyze the oxidation states of the elements in the reaction:- In $NH_{3}$,the oxidation state of $N$ is $-3$ and $H$ is $+1$.- In $O_{2}$,th

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$(i)$ and $(iii)$

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(B) $1$. Analyze the oxidation states of the elements in the reaction:- In $NH_{3}$,the oxidation state of $N$ is $-3$ and $H$ is $+1$.- In $O_{2}$,the oxidation state of $O$ is $0$.- In $NO$,the oxidation state of $N$ is $+2$ and $O$ is $-2$.- In $H_{2}O$,the oxidation state of $H$ is $+1$ and $O$ is $-2$.$2$. Observe the changes:- Nitrogen $(N)$ changes from $-3$ to $+2$ (oxidation).- Oxygen $(O)$ changes from $0$ to $-2$ (reduction).Since both oxidation and reduction occur,it is a redox reaction $(iii)$.$3$. Identify the reaction type:- This is a displacement reaction because $O_{2}$ displaces $H$ from $NH_{3}$ to form $NO$ and $H_{2}O$,which is a type of oxidation-reduction displacement $(i)$.Therefore,the reaction is both a displacement reaction and a redox reaction.

The following reaction is an example of a:
$4 NH_{3}(g) + 5 O_{2}(g) \rightarrow 4 NO(g) + 6 H_{2}O(g)$
$(i)$ Displacement reaction
$(ii)$ Combination reaction
$(iii)$ Redox reaction
$(iv)$ Neutralisation reaction

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The following reaction is an example of a:$4 NH_{3}(g) + 5 O_{2}(g) \rightarrow 4 NO(g) + 6 H_{2}O(g)$$(i)$ Displacement reaction$(ii)$ Combination reaction$(iii)$ Redox reaction$(iv)$ Neutralisation reaction