In the reaction `KMnO_(4) + H_(2)SO_(4) + H_(2)C_(2)O_(4) to` products, `Mn^(2+)` ions act as:

Options

A. Positve catalyst
B. Negative catalyst
C. Auto catalyst
D. Enzyme catalyst

Answer

To determine the role of Mn²⁺ ions in the reaction between KMnO₄, H₂SO₄, and H₂C₂O₄, we can follow these steps:

### Step 1: Write the balanced chemical equation
The reaction involves potassium permanganate (KMnO₄), sulfuric acid (H₂SO₄), and oxalic acid (H₂C₂O₄). The balanced equation for the reaction is:

\[ 2 KMnO_4 + 5 H_2C_2O_4 + 3 H_2SO_4 \rightarrow K_2SO_4 + 2 MnSO_4 + 10 CO_2 + 8 H_2O \]

### Step 2: Identify the products
From the balanced equation, we see that the products formed are potassium sulfate (K₂SO₄), manganese(II) sulfate (MnSO₄), carbon dioxide (CO₂), and water (H₂O). The Mn²⁺ ions are produced as a result of the reduction of KMnO₄.

### Step 3: Analyze the role of Mn²⁺ ions
In this reaction, the Mn²⁺ ions are produced as a by-product. These ions can further catalyze the reaction, meaning they can speed up the reaction without being consumed in the process.

### Step 4: Conclusion
Since the Mn²⁺ ions facilitate the reaction by acting as a catalyst, we can conclude that they act as an autocatalyst in this reaction.

### Final Answer:
Mn²⁺ ions act as an autocatalyst.

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