The volume strength (at STP) of 100 ml `H_2O_2` solution which
produce 5.6 litre of oxygen gas at 1 atm and `273K` is :

Answer

To find the volume strength of the hydrogen peroxide (H₂O₂) solution, we can follow these steps:

### Step 1: Understand the Reaction
The decomposition of hydrogen peroxide can be represented by the equation:
\[ 2 H_2O_2 \rightarrow 2 H_2O + O_2 \]
From this reaction, we can see that 2 moles of H₂O₂ produce 1 mole of O₂.

### Step 2: Convert Volume of Oxygen to Milliliters
The problem states that 5.6 liters of oxygen gas is produced. We need to convert this volume into milliliters:
\[ 5.6 \, \text{liters} = 5.6 \times 1000 \, \text{ml} = 5600 \, \text{ml} \]

### Step 3: Use the Volume Strength Formula
The volume strength (VS) of a solution is defined as the volume of gas produced at STP (Standard Temperature and Pressure) by 1 volume of the solution. The formula can be expressed as:
\[ \text{Volume of O}_2 = \text{Volume Strength} \times \text{Volume of H}_2O_2 \]

### Step 4: Substitute the Known Values
We know the volume of oxygen produced (5600 ml) and the volume of the H₂O₂ solution (100 ml). We can substitute these values into the equation:
\[ 5600 \, \text{ml} = \text{Volume Strength} \times 100 \, \text{ml} \]

### Step 5: Solve for Volume Strength
Now, we can solve for the volume strength:
\[ \text{Volume Strength} = \frac{5600 \, \text{ml}}{100 \, \text{ml}} = 56 \]

### Final Answer
The volume strength of the 100 ml H₂O₂ solution is **56**.

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