In the reaction
`K+O_(2)rarrKO_(2)`

Options

A. `O_(2)` acts as an oxidising agent
B. Both `K` and `O_(2)` are oxidised
C. `O_(2)` is oxidised while `K` is reduced
D. `K` acts as an oxidising agent

Explanation

To analyze the reaction \( K + O_2 \rightarrow KO_2 \) in terms of redox processes, we will break it down into half-reactions and identify the oxidation and reduction components.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
- The reactants are potassium (K) and oxygen (O2).
- The product is potassium superoxide (KO2).

2. **Determine the Oxidation States**:
- In elemental form, potassium (K) has an oxidation state of 0.
- In \( O_2 \), the oxidation state of oxygen is also 0.
- In \( KO_2 \), potassium (K) has an oxidation state of +1, and each oxygen in \( O_2^{2-} \) has an oxidation state of -1.

3. **Write the Half-Reactions**:
- For potassium (K):
\[ K \rightarrow K^+ + e^- \]
This half-reaction shows that potassium is oxidized (loses an electron).

- For oxygen (O2):
\[ O_2 + 4e^- \rightarrow 2O^{2-} \]
This half-reaction shows that oxygen is reduced (gains electrons).

4. **Identify Oxidation and Reduction**:
- **Oxidation**: The process where potassium (K) loses an electron and is oxidized to \( K^+ \).
- **Reduction**: The process where oxygen (O2) gains electrons to form \( O^{2-} \).

5. **Identify the Reducing and Oxidizing Agents**:
- The reducing agent is the species that gets oxidized. In this case, potassium (K) is the reducing agent.
- The oxidizing agent is the species that gets reduced. Here, oxygen (O2) is the oxidizing agent.

6. **Conclusion**:
- In the reaction \( K + O_2 \rightarrow KO_2 \), potassium is oxidized and acts as the reducing agent, while oxygen is reduced and acts as the oxidizing agent.

### Final Answer:
- Potassium (K) is the reducing agent, and oxygen (O2) is the oxidizing agent in the reaction.