`H_(2)O_(2)rarrH_(2)O+1/2O_(2)` equivalent mass of `H_(2)O_(2)` is

Options

A. 34 g
B. 46 g
C. 12 g
D. 18 g

Answer

To find the equivalent mass of hydrogen peroxide (H₂O₂) in the given reaction, we can follow these steps:

### Step 1: Write the reaction
The reaction given is:
\[ H_2O_2 \rightarrow H_2O + \frac{1}{2}O_2 \]

### Step 2: Determine the oxidation states
In this reaction, we need to determine the oxidation states of the elements involved:
- In H₂O₂, the oxidation state of oxygen is -1.
- In H₂O, the oxidation state of oxygen is -2.
- In O₂, the oxidation state of oxygen is 0.

### Step 3: Calculate the change in oxidation state
Now, we can calculate the change in oxidation state for oxygen in H₂O₂:
- The change in oxidation state from -1 (in H₂O₂) to -2 (in H₂O) is a reduction of 1.
- The change from -1 (in H₂O₂) to 0 (in O₂) is an oxidation of 1.

### Step 4: Determine the n-factor
The n-factor is defined as the total change in oxidation number per molecule of the substance. In this case, since one molecule of H₂O₂ undergoes both oxidation and reduction, the n-factor can be calculated as:
\[ \text{n-factor} = \text{change in oxidation state for reduction} + \text{change in oxidation state for oxidation} = 1 + 1 = 2 \]

### Step 5: Calculate the molecular weight of H₂O₂
The molecular weight of H₂O₂ can be calculated as follows:
- Hydrogen (H) has an atomic weight of approximately 1 g/mol, and there are 2 hydrogen atoms: \(2 \times 1 = 2\) g/mol.
- Oxygen (O) has an atomic weight of approximately 16 g/mol, and there are 2 oxygen atoms: \(2 \times 16 = 32\) g/mol.
- Therefore, the molecular weight of H₂O₂ is:
\[ 2 + 32 = 34 \text{ g/mol} \]

### Step 6: Calculate the equivalent mass
The equivalent mass can be calculated using the formula:
\[ \text{Equivalent mass} = \frac{\text{Molecular weight}}{\text{n-factor}} \]
Substituting the values we have:
\[ \text{Equivalent mass} = \frac{34 \text{ g/mol}}{2} = 17 \text{ g/equiv} \]

### Final Answer
The equivalent mass of H₂O₂ is 17 g/equiv.

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