When `H_(2)O_(2)` is decomposed to `O_(2)` gas, it `n_("factor")` is_____.

Answer

To find the n-factor of hydrogen peroxide (H₂O₂) when it decomposes to oxygen gas (O₂), we will follow these steps:

### Step 1: Write the decomposition reaction
The decomposition of hydrogen peroxide can be represented by the following unbalanced equation:
\[ \text{H}_2\text{O}_2 \rightarrow \text{O}_2 + \text{H}_2\text{O} \]

### Step 2: Balance the reaction
To balance the reaction, we need to ensure that the number of atoms of each element is the same on both sides. The balanced equation for the decomposition of hydrogen peroxide is:
\[ 2 \text{H}_2\text{O}_2 \rightarrow \text{O}_2 + 2 \text{H}_2\text{O} \]

### Step 3: Identify oxidation and reduction
In this reaction:
- H₂O₂ is oxidized to O₂ (loss of electrons).
- H₂O₂ is also reduced to H₂O (gain of electrons).

### Step 4: Determine the number of electrons transferred
For the oxidation half-reaction:
\[ \text{H}_2\text{O}_2 \rightarrow \text{O}_2 + 2 \text{H}^+ + 2 e^- \]
This shows that 2 electrons are lost.

For the reduction half-reaction:
\[ \text{H}_2\text{O}_2 + 2 e^- + 2 \text{H}^+ \rightarrow 2 \text{H}_2\text{O} \]
This shows that 2 electrons are gained.

### Step 5: Calculate the n-factor
The n-factor is defined as the number of electrons transferred per mole of reactant. In our balanced equation, we have:
- 2 moles of H₂O₂ producing 2 moles of electrons.

Thus, the n-factor of H₂O₂ can be calculated as:
\[ \text{n-factor} = \frac{\text{Total number of electrons transferred}}{\text{Number of moles of H}_2\text{O}_2} = \frac{2 \text{ electrons}}{2 \text{ moles of H}_2\text{O}_2} = 1 \]

### Final Answer
The n-factor of H₂O₂ when decomposed to O₂ gas is **1**.

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