1 ml of `H_(2)O_(2)` solution given 10 ml of `O_(2)` at NTP. It is :

Options

A. `10 vol H_(2)O_(2)`
B. 20 vol `H_(2)O_(2)`
C. 30 vol `H_(2)O_(2)`
D. 40 vol `H_(2)O_(2)`

Answer

To solve the problem, we need to determine the volume strength of the hydrogen peroxide (H₂O₂) solution based on the amount of oxygen gas (O₂) produced during its decomposition. Here’s a step-by-step solution:

### Step 1: Understand the decomposition of hydrogen peroxide
The decomposition reaction of hydrogen peroxide is given by:
\[ 2 \, H_2O_2 \, \rightarrow \, 2 \, H_2O + O_2 \]

From this reaction, we can see that 2 moles of hydrogen peroxide produce 1 mole of oxygen gas.

### Step 2: Relate the volume of oxygen produced to the volume strength
The volume strength of hydrogen peroxide is defined as the volume of oxygen gas liberated by 1 liter of hydrogen peroxide solution.

### Step 3: Analyze the given data
We are given that 1 ml of H₂O₂ solution produces 10 ml of O₂ gas at NTP (Normal Temperature and Pressure).

### Step 4: Scale up to 1 liter
Since 1 liter is equal to 1000 ml, we can scale the volume of oxygen produced:
- If 1 ml of H₂O₂ produces 10 ml of O₂, then:
\[ 1000 \, ml \, H_2O_2 \, \text{produces} \, 1000 \times 10 \, ml \, O_2 = 10000 \, ml \, O_2 \]

### Step 5: Calculate the volume strength
The volume strength of the hydrogen peroxide solution is therefore:
- Volume strength = Volume of O₂ produced by 1 liter of H₂O₂ solution = 10000 ml = 10 liters.

### Step 6: Convert to volume strength units
Since volume strength is often expressed in terms of "volume," we can express this as:
- Volume strength = 10 V (volume).

### Conclusion
Thus, the volume strength of the hydrogen peroxide solution is 10 V.

The correct option from the given choices is:
- **Option 1: 10 volume hydrogen peroxide.**

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