Respuesta :
Explanation:
Reaction for oxidation of gaseous nitric oxide to aqueous nitrous acid is as follows.
[tex]NO(g) \rightarrow HNO_{2}(aq)[/tex]
By adding water, we will balance the oxygen atoms on both the sides as follows.
[tex]NO(g) + H_{2}O(l) \rightarrow HNO_{2}(aq)[/tex]
Now, we will balance the hydrogen atoms by adding [tex]H^{+}[/tex] ions as follows.
[tex]NO(g) + H_{2}O(l) \rightarrow HNO_{2}(aq) + H^{+}(aq)[/tex]
Now, we will add [tex]OH^{-}[/tex] ions on both the sides in order to neutralize [tex]H^{+}[/tex] ions.
[tex]NO(g) + H_{2}O(l) + OH^{-}(aq) \rightarrow HNO_{2}(aq) + H^{+}(aq) + OH^{-}(aq)[/tex] ..... (1)
We will combine the [tex]H^{+}[/tex] and [tex]OH^{-}[/tex] ions in order to form water in equation (1) and cancelling the common terms as follows.
[tex]NO(g) + OH^{-}(aq) \rightarrow HNO_{2}(aq)[/tex]
Now, we will balance the charge on both the sides as follows.
[tex]NO(g) + OH^{-}(aq) \rightarrow HNO_{2}(aq) + 1e^{-}[/tex]
Thus, we can conclude that the balanced half-reaction equation is as follows.
[tex]NO(g) + OH^{-}(aq) \rightarrow HNO_{2}(aq) + 1e^{-}[/tex]
