Consider the chemical equation given below and answer the questions that follow:
`CuO+H_2 overset("Heat")to Cu+H_2O`
Name the oxidizing and the reducing agent.

Explanation

To determine the oxidizing and reducing agents in the given chemical equation \( \text{CuO} + \text{H}_2 \overset{\text{Heat}}{\rightarrow} \text{Cu} + \text{H}_2\text{O} \), we can follow these steps:

### Step 1: Identify the oxidation states of the elements involved.
- In \( \text{CuO} \), copper (Cu) has an oxidation state of +2 and oxygen (O) has an oxidation state of -2.
- In \( \text{Cu} \), copper is in its elemental form, so its oxidation state is 0.
- In \( \text{H}_2 \), hydrogen (H) is also in its elemental form, so its oxidation state is 0.
- In \( \text{H}_2\text{O} \), hydrogen has an oxidation state of +1 and oxygen has an oxidation state of -2.

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