Commercial 10 volume `H_(2)O_(2)` is a solution with a strength approximately

Options

A. 0.3
B. 0.1
C. 0.03
D. 1 %.

Answer

To find the strength of commercial 10 volume H₂O₂, we can follow these steps:

### Step 1: Understand the meaning of "10 volume"
A "10 volume" solution of H₂O₂ means that 1 liter of this solution will produce 10 liters of oxygen gas (O₂) at standard temperature and pressure (STP).

### Step 2: Write the decomposition reaction of H₂O₂
The decomposition of hydrogen peroxide (H₂O₂) can be represented by the following chemical equation:
\[ 2 \text{H}_2\text{O}_2 \rightarrow 2 \text{H}_2\text{O} + \text{O}_2 \]
From this equation, we see that 2 moles of H₂O₂ produce 1 mole of O₂.

### Step 3: Calculate the volume of O₂ produced from H₂O₂
At STP, 1 mole of any gas occupies 22.4 liters. Therefore, to find out how much H₂O₂ is needed to produce 10 liters of O₂, we can set up the following ratio:
- 1 mole of O₂ (22.4 liters) is produced from 2 moles of H₂O₂.

### Step 4: Calculate the mass of H₂O₂ required
To find out how many grams of H₂O₂ are needed to produce 10 liters of O₂, we can use the following calculations:
- 10 liters of O₂ corresponds to:
\[ \text{Moles of O}_2 = \frac{10 \text{ liters}}{22.4 \text{ liters/mole}} \approx 0.4464 \text{ moles} \]
- Since 2 moles of H₂O₂ produce 1 mole of O₂, we need:
\[ \text{Moles of H}_2\text{O}_2 = 2 \times 0.4464 \approx 0.8928 \text{ moles} \]

### Step 5: Convert moles of H₂O₂ to grams
The molar mass of H₂O₂ is approximately 34 g/mol. Therefore, the mass of H₂O₂ required is:
\[ \text{Mass of H}_2\text{O}_2 = 0.8928 \text{ moles} \times 34 \text{ g/mol} \approx 30.3 \text{ grams} \]

### Step 6: Calculate the strength of the solution
The strength of the solution is defined as the mass of solute (H₂O₂) per liter of solution. Since we have approximately 30 grams of H₂O₂ in 1 liter of solution, the strength is:
\[ \text{Strength} = 30 \text{ g/L} \]

### Step 7: Convert grams to percentage
To convert grams to percentage, we use the formula:
\[ \text{Percentage} = \left( \frac{\text{mass of solute}}{\text{mass of solution}} \right) \times 100 \]
Assuming the density of the solution is similar to water (1 g/mL), 1 liter of solution weighs approximately 1000 grams. Thus:
\[ \text{Strength} = \left( \frac{30 \text{ g}}{1000 \text{ g}} \right) \times 100 = 3\% \]

### Conclusion
The strength of commercial 10 volume H₂O₂ is approximately **3%**.

---