The following reaction is used for the preparation of oxygen gas in the laboratory
`2KClO_(3)(s)underset("Catalyst")overset("Heat")to2KCl(s)+3O_(2)(g)`
Which of the following statement(s) is/are not correct about the reaction?

Options

A. Potassium is undergoing oxidation
B. Chlorine is undergoing oxidation
C. Oxygen is reduced
D. None of the species are undergoing oxidation or reduction

Explanation

To determine which statements are not correct about the given reaction, we need to analyze the oxidation states of the elements involved in the reaction:

**Given Reaction:**
\[ 2 \text{KClO}_3(s) \xrightarrow{\text{Heat, Catalyst}} 2 \text{KCl}(s) + 3 \text{O}_2(g) \]

### Step 1: Assign Oxidation States
1. **Potassium (K)** in KClO3 and KCl:
- K in KClO3: +1
- K in KCl: +1

2. **Chlorine (Cl)** in KClO3 and KCl:
- Let the oxidation state of Cl in KClO3 be \( x \).
- The equation for KClO3 is:
\[ +1 + x + 3(-2) = 0 \]
\[ +1 + x - 6 = 0 \]
\[ x = +5 \]
- Cl in KCl: -1

3. **Oxygen (O)** in KClO3 and O2:
- O in KClO3: -2
- O in O2 (elemental form): 0

### Step 2: Determine Changes in Oxidation States
- **Potassium (K)**: No change (remains +1).
- **Chlorine (Cl)**: Changes from +5 in KClO3 to -1 in KCl. This indicates a gain of electrons (reduction).
- **Oxygen (O)**: Changes from -2 in KClO3 to 0 in O2. This indicates a loss of electrons (oxidation).

### Step 3: Analyze the Statements
1. **Potassium is undergoing oxidation**: Incorrect, as there is no change in the oxidation state of potassium.
2. **Chlorine is undergoing oxidation**: Incorrect, as chlorine is being reduced (gaining electrons).
3. **Oxygen is reduced**: Incorrect, as oxygen is being oxidized (losing electrons).
4. **None of the species are undergoing oxidation or reduction**: Incorrect, as we have identified that chlorine is reduced and oxygen is oxidized.

### Conclusion
All the statements provided are incorrect regarding the reaction.

### Final Answer
All statements (1, 2, 3, and 4) are not correct.

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