Questions: Study this chemical reaction: Pt + O2 -> PtO2 Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction. oxidation: reduction:

Study this chemical reaction: Pt + O2 -> PtO2 Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction. oxidation: reduction:
Transcript text: Study this chemical reaction: \[ \mathrm{Pt}+\mathrm{O}_{2} \rightarrow \mathrm{PtO}_{2} \] Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction. oxidation: reduction:
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Solution

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Solution Steps

Step 1: Identify the Oxidation and Reduction Processes

In a redox reaction, oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. In the given reaction:

\[ \mathrm{Pt} + \mathrm{O}_{2} \rightarrow \mathrm{PtO}_{2} \]

Platinum (Pt) is being oxidized as it combines with oxygen to form platinum(IV) oxide (\(\mathrm{PtO}_{2}\)). Oxygen (\(\mathrm{O}_{2}\)) is being reduced as it gains electrons to form oxide ions in \(\mathrm{PtO}_{2}\).

Step 2: Write the Oxidation Half-Reaction

The oxidation half-reaction involves the conversion of platinum (Pt) to platinum(IV) oxide (\(\mathrm{PtO}_{2}\)). In this process, platinum loses electrons. The balanced oxidation half-reaction is:

\[ \mathrm{Pt} \rightarrow \mathrm{Pt}^{4+} + 4e^- \]

Step 3: Write the Reduction Half-Reaction

The reduction half-reaction involves the conversion of molecular oxygen (\(\mathrm{O}_{2}\)) to oxide ions. Oxygen gains electrons in this process. The balanced reduction half-reaction is:

\[ \mathrm{O}_{2} + 4e^- \rightarrow 2\mathrm{O}^{2-} \]

Final Answer

  • Oxidation half-reaction: \(\boxed{\mathrm{Pt} \rightarrow \mathrm{Pt}^{4+} + 4e^-}\)
  • Reduction half-reaction: \(\boxed{\mathrm{O}_{2} + 4e^- \rightarrow 2\mathrm{O}^{2-}}\)
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