Indicate the species which are oxidised and reduced in the following reactions:
`CN^(Ө) + OCl^(Ө) rarr N_(2)+HCO_(3)^(Ө) + Cl^(Ө)`

Explanation

To determine which species are oxidized and reduced in the reaction:

\[ \text{CN}^- + \text{OCl}^- \rightarrow \text{N}_2 + \text{HCO}_3^- + \text{Cl}^- \]

we will follow these steps:

### Step 1: Identify the oxidation states of the elements in the reactants.
- In CN\(^-\), the oxidation state of nitrogen (N) is -3.
- In OCl\(^-\), the oxidation state of chlorine (Cl) is +1.

### Step 2: Identify the oxidation states of the elements in the products.
- In N\(_2\), the oxidation state of nitrogen (N) is 0 (since it is in its elemental form).
- In HCO\(_3^-\), the oxidation state of carbon (C) is +4, and the oxidation state of oxygen (O) is -2.
- In Cl\(^-\), the oxidation state of chlorine (Cl) is -1.

### Step 3: Determine the changes in oxidation states.
- For nitrogen (from CN\(^-\) to N\(_2\)):
- Initial oxidation state: -3
- Final oxidation state: 0
- Change: -3 to 0 (increase in oxidation state, indicating oxidation).

- For chlorine (from OCl\(^-\) to Cl\(^-\)):
- Initial oxidation state: +1
- Final oxidation state: -1
- Change: +1 to -1 (decrease in oxidation state, indicating reduction).

### Step 4: Conclude which species are oxidized and reduced.
- The species that is oxidized is CN\(^-\) (as nitrogen goes from -3 to 0).
- The species that is reduced is OCl\(^-\) (as chlorine goes from +1 to -1).

### Final Answer:
- **Oxidized Species:** CN\(^-\)
- **Reduced Species:** OCl\(^-\)

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