`NaNO_(3)+FeSO_(4)+H_(2)SO_(4) to underset(("Ring complex"))([Fe(H_(2)O)_(5)NO]SO_(4))`

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 analyze the reaction \( \text{NaNO}_3 + \text{FeSO}_4 + \text{H}_2\text{SO}_4 \rightarrow [\text{Fe(H}_2\text{O)}_5\text{NO}] \text{SO}_4 \), we need to determine the type of reaction taking place. Let's break it down step by step:

### Step 1: Identify the Reactants and Products
The reactants are sodium nitrate (\( \text{NaNO}_3 \)), iron(II) sulfate (\( \text{FeSO}_4 \)), and sulfuric acid (\( \text{H}_2\text{SO}_4 \)). The product is a complex ion, specifically a ring complex, represented as \( [\text{Fe(H}_2\text{O)}_5\text{NO}] \text{SO}_4 \).

**Hint:** Always start by identifying what substances are involved in the reaction.

### Step 2: Determine the Oxidation States
Next, we need to calculate the oxidation states of the relevant elements in the reactants and products:

- In \( \text{NaNO}_3 \):
- Sodium (\( \text{Na} \)) has an oxidation state of +1.
- Oxygen (\( \text{O} \)) has an oxidation state of -2.
- Let \( x \) be the oxidation state of nitrogen (\( \text{N} \)):
\[ +1 + x + 3(-2) = 0 \implies x = +5 \]

- In \( \text{FeSO}_4 \):
- Iron (\( \text{Fe} \)) has an oxidation state of +2.

- In the product \( [\text{Fe(H}_2\text{O)}_5\text{NO}] \text{SO}_4 \):
- The nitrogen in the nitrosyl (\( \text{NO} \)) has an oxidation state of +3.
- The iron in the complex has an oxidation state of +3.

**Hint:** Calculating oxidation states helps to understand how elements are changing in the reaction.

### Step 3: Analyze the Changes in Oxidation States
Now, let's analyze the changes in oxidation states:
- Iron changes from +2 in \( \text{FeSO}_4 \) to +3 in the product.
- Nitrogen changes from +5 in \( \text{NaNO}_3 \) to +3 in the product.

This indicates that:
- Iron is oxidized (increasing oxidation state from +2 to +3).
- Nitrogen is reduced (decreasing oxidation state from +5 to +3).

**Hint:** Identifying oxidation and reduction processes is key to classifying the reaction type.

### Step 4: Classify the Reaction
Since we have one species being oxidized and another being reduced, this is characteristic of a redox reaction. Specifically, because both oxidation and reduction occur simultaneously, we can classify this as an **intermolecular redox reaction**.

**Hint:** Look for changes in oxidation states to determine if a reaction is redox and how to classify it.

### Conclusion
The reaction \( \text{NaNO}_3 + \text{FeSO}_4 + \text{H}_2\text{SO}_4 \rightarrow [\text{Fe(H}_2\text{O)}_5\text{NO}] \text{SO}_4 \) is classified as an **intermolecular redox reaction**.