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Consider the redox reaction below:

[tex]\[ \text{Mg}_{(s)} + \text{Fe}^{2+}_{(aq)} \longrightarrow \text{Mg}^{2+}_{(aq)} + \text{Fe}_{(s)} \][/tex]

Which equation is a half reaction that describes the reduction that is taking place?

A. [tex]\[ \text{Fe}^{2+}_{(aq)} + 2e^{-} \longrightarrow \text{Fe}_{(s)} \][/tex]

B. [tex]\[ \text{Mg}_{(s)} \longrightarrow \text{Mg}^{2+}_{(aq)} + 2e^{-} \][/tex]

C. [tex]\[ \text{Fe}^{2+}_{(aq)} \longrightarrow \text{Fe}_{(s)} + 2e^{-} \][/tex]

D. [tex]\[ \text{Mg}_{(s)} + 2e^{-} \longrightarrow \text{Mg}^{2+}_{(aq)} \][/tex]



Answer :

GinnyAnswer
In the given redox reaction:

[tex]\[ Mg\ (s) + Fe^{2+}\ (aq) \longrightarrow Mg^{2+}\ (aq) + Fe\ (s) \][/tex]

we need to identify the half-reaction that describes the reduction process.

Step-by-Step Solution:

1. Identify the Oxidation States:
- Magnesium (Mg) starts as a solid with an oxidation state of [tex]\(0\)[/tex] and becomes [tex]\(Mg^{2+}\ (aq)\)[/tex], which means it loses 2 electrons ([tex]\(e^-)\)[/tex]. Hence, it is oxidized.
- Iron ([tex]\(Fe^{2+}\)[/tex]) in aqueous state starts with an oxidation state of [tex]\(+2\)[/tex] and becomes solid iron (Fe) with an oxidation state of [tex]\(0\)[/tex], which means it gains 2 electrons. Hence, it is reduced.

2. Write the Reduction Half-Reaction:
- The reduction process involves gaining electrons. Here, iron is being reduced from a [tex]\(+2\)[/tex] state to [tex]\(0\)[/tex].
- The balanced half-reaction for the reduction process can be written as:
[tex]\[ Fe^{2+}\ (aq) + 2e^- \longrightarrow Fe\ (s) \][/tex]

Among the given options, the correct half-reaction describing the reduction process is:
[tex]\[ Fe^{2+}\ (aq) + 2e^- \longrightarrow Fe\ (s) \][/tex]

Thus, the correct equation is:
[tex]\[ Fe^{2+}\ (aq) + 2e^- \longrightarrow Fe\ (s) \][/tex]

This matches the answer option:
[tex]\[ Fe^{2+}\ (aq) + 2e^- \longrightarrow Fe\ (s) \][/tex]

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