One mole of hydrogen peroxide `(H_(2)O_(2))` has a mass same as that of

Options

A. 0.2 mol of sucrose `(C_(12)H_(22)O_(11))`
B. 2.0 mol of ammonia
C. 11.2 L of `SO_(2)` at N.T.P.
D. 0.1 mol of `SO_(3)`

Explanation

To solve the question, we need to determine the mass of one mole of hydrogen peroxide (H₂O₂) and then compare it with the masses of the given options.

### Step-by-Step Solution:

1. **Calculate the Molar Mass of Hydrogen Peroxide (H₂O₂)**:
- Hydrogen (H) has an atomic mass of approximately 1 g/mol.
- Oxygen (O) has an atomic mass of approximately 16 g/mol.
- In H₂O₂, there are 2 hydrogen atoms and 2 oxygen atoms.
- Therefore, the molar mass of H₂O₂ can be calculated as follows:
\[ \text{Molar Mass of H₂O₂} = (2 \times \text{mass of H}) + (2 \times \text{mass of O}) \]
\[ = (2 \times 1) + (2 \times 16) \]
\[ = 2 + 32 = 34 \text{ g/mol} \]

2. **Compare with Given Options**:
- We need to find which of the given options has a mass equal to 34 g.
- Let's analyze each option:
- **Option A**: 0.2 moles of sucrose (C₁₂H₂₂O₁₁)
- Molar mass of sucrose = 342 g/mol.
- Mass of 0.2 moles = \( 342 \times 0.2 = 68.4 \) g (not equal to 34 g).
- **Option B**: 2 moles of ammonia (NH₃)
- Molar mass of ammonia = 17 g/mol.
- Mass of 2 moles = \( 17 \times 2 = 34 \) g (equal to 34 g).
- **Option C**: 11.2 liters of SO₂
- Molar mass of SO₂ = 64 g/mol.
- Mass of 11.2 liters = \( \frac{64}{22.4} \times 11.2 = 32 \) g (not equal to 34 g).
- **Option D**: 0.1 mole of SO₃
- Molar mass of SO₃ = 80 g/mol.
- Mass of 0.1 mole = \( 80 \times 0.1 = 8 \) g (not equal to 34 g).

3. **Conclusion**:
- The only option that matches the mass of 1 mole of hydrogen peroxide (34 g) is **Option B: 2 moles of ammonia**.

### Final Answer:
**One mole of hydrogen peroxide (H₂O₂) has a mass same as that of 2 moles of ammonia (NH₃), which is 34 grams.**