Write a balanced half-reaction for the oxidation of liquid water to gaseous oxygen in basic aqueous solution. be sure to add physical state symbols where appropriate.

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25-08-2022
Chemistry

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Write a balanced half-reaction for the oxidation of liquid water to gaseous oxygen in basic aqueous solution. be sure to add physical state symbols where appropriate.

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smecloudbird18 smecloudbird18 · Answer 1 · 2022-09-02T10:59:47-04:00

The balanced half-reaction for the oxidation of liquid water to gaseous oxygen in basic aqueous solution is given as ,

[tex]4OH^{-}[/tex](aq) ⟶ [tex]O_{2} (g)[/tex] + [tex]2H_{2}O[/tex](l) + [tex]4e^{-}[/tex]

Steps involved :

The oxidation of liquid water to gaseous oxygen can be represented as

[tex]H_{2} O(l)[/tex] ⟶ [tex]O_{2} (g)[/tex]

To balance this, we will first balance the number of oxygen atoms.

[tex]2H_{2} O(l)[/tex] ⟶ [tex]O_{2} (g)[/tex]

Now we have to balance the hydrogen atoms. Since the reaction takes place in an basic aqueous medium, hydroxide will be present in the form of its ions, dissolved in the aqueous medium.

[tex]2H_{2} O(l)[/tex] + [tex]4OH^{-}[/tex]⟶ [tex]O_{2} (g)[/tex] + [tex]4H^{+}[/tex]+ [tex]4OH^{-}[/tex]

Now the atoms on either side are balanced, but the charges are not. The reactant have a charge of +4 whereas the product is neutral. So, to balance the charge, we will add electrons to the products side, which was expected since, in an oxidation reaction, electrons are released.

[tex]2H_{2} O(l)[/tex] + [tex]4OH^{-}[/tex]⟶ [tex]O_{2} (g)[/tex] + [tex]4H_{2}O[/tex] + [tex]4e^{-}[/tex]

[tex]4OH^{-}[/tex](aq) ⟶ [tex]O_{2} (g)[/tex] + [tex]2H_{2}O[/tex](l) + [tex]4e^{-}[/tex]

This is the required balanced half-reaction.

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