The volume of `10` volume of `H_2O_2` required to liberate `500mL` of `O_2` at `STP is

Options

A. `25 mL`
B. `50 mL`
C. `100 mL`
D. `125 mL`

Explanation

To solve the problem of determining the volume of 10 volume hydrogen peroxide (H₂O₂) required to liberate 500 mL of oxygen (O₂) at standard temperature and pressure (STP), we can follow these steps:

### Step-by-Step Solution:

1. **Understanding 10 Volume of H₂O₂**:
- The term "10 volume" means that 1 mL of H₂O₂ will liberate 10 mL of O₂ at STP.
- Therefore, for every 1 mL of H₂O₂, we can expect to produce 10 mL of O₂.

2. **Setting Up the Proportion**:
- We need to find out how much H₂O₂ is required to produce 500 mL of O₂.
- Since 1 mL of H₂O₂ produces 10 mL of O₂, we can set up the following relationship:
\[ \text{Volume of H₂O₂ (mL)} = \frac{\text{Volume of O₂ (mL)}}{10} \]

3. **Calculating the Volume of H₂O₂**:
- Plugging in the values we have:
\[ \text{Volume of H₂O₂} = \frac{500 \text{ mL}}{10} = 50 \text{ mL} \]

4. **Conclusion**:
- Therefore, the volume of 10 volume H₂O₂ required to liberate 500 mL of O₂ at STP is **50 mL**.

### Final Answer:
The volume of 10 volume H₂O₂ required to liberate 500 mL of O₂ at STP is **50 mL**.