`Cr_(2)O_(7)^(2-)+H^(+)+SO_(3)^(2-) to Cr^(3+)(aq.)+SO_(4)^(2-)`

Options

A. For disproportionation reaction.
B. For comproportionation reaction.
C. For either intermolecular redox reaction or displacement reaction
D. For either thermal combination redox reaction or thermal decomposition redox reaction.

Answer

To solve the given reaction:

**Step 1: Write the balanced chemical equation.**
The reaction is:
\[ \text{Cr}_2\text{O}_7^{2-} + \text{H}^+ + \text{SO}_3^{2-} \rightarrow \text{Cr}^{3+} + \text{SO}_4^{2-} \]

**Step 2: Assign oxidation states to each element.**
- In \(\text{Cr}_2\text{O}_7^{2-}\), the oxidation state of Cr is +6.
- In \(\text{H}^+\), the oxidation state of H is +1.
- In \(\text{SO}_3^{2-}\), the oxidation state of S is +4.
- In \(\text{Cr}^{3+}\), the oxidation state of Cr is +3.
- In \(\text{SO}_4^{2-}\), the oxidation state of S is +6.

**Step 3: Identify changes in oxidation states.**
- Chromium (Cr) goes from +6 in \(\text{Cr}_2\text{O}_7^{2-}\) to +3 in \(\text{Cr}^{3+}\) (reduction).
- Sulfur (S) goes from +4 in \(\text{SO}_3^{2-}\) to +6 in \(\text{SO}_4^{2-}\) (oxidation).

**Step 4: Determine the type of reaction.**
Since one species is being reduced (Cr) and another is being oxidized (S), this is a redox reaction. Specifically, it is an intermolecular redox reaction because it involves the transfer of electrons between two different molecules.

**Step 5: Conclusion.**
The type of reaction is an intermolecular redox reaction.

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