The number of electrons involved when 1 mole of `H_(2)O_(2)` decomposes as
`H_(2)O_(2) rarr H_(2)O +O_(2)`, is

Options

A. 1
B. 8
C. 6
D. 4

Answer

To determine the number of electrons involved when 1 mole of \( H_2O_2 \) decomposes according to the reaction:

\[ H_2O_2 \rightarrow H_2O + O_2 \]

we will analyze the oxidation states of the elements involved in the reaction.

### Step 1: Identify the oxidation states
- In hydrogen peroxide (\( H_2O_2 \)), the oxidation state of oxygen is \(-1\).
- In water (\( H_2O \)), the oxidation state of oxygen is \(-2\).
- In molecular oxygen (\( O_2 \)), the oxidation state of oxygen is \(0\).

### Step 2: Determine the changes in oxidation states
- The oxygen in \( H_2O_2 \) changes from \(-1\) to \(-2\) in \( H_2O\) (this is a reduction).
- The other oxygen in \( H_2O_2 \) changes from \(-1\) to \(0\) in \( O_2\) (this is an oxidation).

### Step 3: Calculate the number of electrons transferred
- For the oxygen that is reduced (from \(-1\) to \(-2\)), it gains 1 electron.
- For the oxygen that is oxidized (from \(-1\) to \(0\)), it loses 1 electron.

### Step 4: Conclusion
Since one mole of \( H_2O_2 \) produces one mole of \( H_2O \) and half a mole of \( O_2 \), the total number of electrons involved in the reaction is:

\[ 1 \text{ (for reduction)} + 1 \text{ (for oxidation)} = 1 \text{ electron} \]

Thus, the total number of electrons involved when 1 mole of \( H_2O_2 \) decomposes is **1**.

### Final Answer:
The number of electrons involved when 1 mole of \( H_2O_2 \) decomposes is **1**.

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