Balance the following oxidation-reduction equations. (a) Fe2 S3(s)+H2 O+O2(g) ⟶Fe(OH)3(s)+S(s)

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Balance the following oxidation-reduction equations. (a) ...

Balance the following oxidation-reduction equations. $$\text { (a) } \mathrm{Fe}_{2} \mathrm{S}_{3}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}(\mathrm{g}) \longrightarrow \mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{s})+\mathrm{S}(\mathrm{s})$$ $$\begin{aligned} &\text { (b) } \mathrm{Mn}^{2+}(\mathrm{aq})+\mathrm{S}_{2} \mathrm{O}_{8}^{2-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\\ &&\mathrm{MnO}_{4}^{-}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \end{aligned}$$ $$\begin{aligned} &\text { (c) } \mathrm{Ag}(\mathrm{s})+\mathrm{CN}^{-}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\\ &&\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \end{aligned}$$

Balance the following oxidation-reduction equations.
$$\text { (a) } \mathrm{Fe}_{2} \mathrm{S}_{3}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}(\mathrm{g}) \longrightarrow \mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{s})+\mathrm{S}(\mathrm{s})$$
$$\begin{aligned}
&\text { (b) } \mathrm{Mn}^{2+}(\mathrm{aq})+\mathrm{S}_{2} \mathrm{O}_{8}^{2-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\\
&&\mathrm{MnO}_{4}^{-}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq})
\end{aligned}$$
$$\begin{aligned}
&\text { (c) } \mathrm{Ag}(\mathrm{s})+\mathrm{CN}^{-}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\\
&&\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})
\end{aligned}$$

Key Concepts

Half-Reaction Method

The half-reaction method is a systematic technique used to balance redox reactions by dividing the overall reaction into two parts: one for oxidation and one for reduction. Each half-reaction is balanced separately for atoms and charges, especially focusing on the electrons lost or gained, before combining them to give the balanced overall chemical equation. This method is particularly useful when the reaction occurs in solution and may require additional species like water, hydrogen ions, or hydroxide ions depending on the reaction medium.

Balancing Atoms and Charges

In the context of redox reactions, balancing atoms and charges is crucial to ensure that the law of conservation of mass and the conservation of charge are both satisfied. Techniques such as adding water molecules, hydrogen ions (H+), or hydroxide ions (OH-) are employed based on whether the reaction is in an acidic or basic medium. This step ensures that both the mass and the net charge remain equivalent on both sides of the reaction equation.

Redox Reactions

Redox reactions, or oxidation-reduction reactions, are chemical reactions that involve a transfer of electrons between species. One substance undergoes oxidation (loss of electrons) while another undergoes reduction (gain of electrons). Understanding the underlying electron transfer is crucial for identifying the changes in the oxidation states of elements involved in the reaction, which is fundamental in balancing these types of equations.

Oxidation States

Oxidation states are numerical values assigned to elements in compounds or ions that indicate the degree of oxidation or reduction of an element. These values are essential in redox reactions as they help in identifying which species are oxidized and which are reduced, thereby facilitating the correct balancing of the electron transfer process within the overall reaction.

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