Which of the following has maximum mass ?

Options

A. 1.0 mole of `H_(2)` gas
B. 0.5 mole of sucrose `(C_(12)H_(22)O_(11))`
C. 1.2 mole of `N_(2)` at N.T.P.
D. 22.4 L of `N_(2)` at N.T.P.

Answer

To determine which of the given options has the maximum mass, we will calculate the mass for each option based on the number of moles and the molecular weight of the substances involved.

### Step-by-Step Solution:

1. **Calculate the mass of 1 mole of S2:**
- Molecular weight of S2 = 2 × Atomic weight of Sulfur (S)
- Atomic weight of Sulfur (S) = 32 g/mol
- Therefore, Molecular weight of S2 = 2 × 32 = 64 g/mol
- Mass = Number of moles × Molecular weight = 1 × 64 = **64 grams**

2. **Calculate the mass of 0.5 moles of sucrose (C12H22O11):**
- Molecular weight of C12H22O11 = (12 × Atomic weight of C) + (22 × Atomic weight of H) + (11 × Atomic weight of O)
- Atomic weight of Carbon (C) = 12 g/mol, Hydrogen (H) = 1 g/mol, Oxygen (O) = 16 g/mol
- Molecular weight = (12 × 12) + (22 × 1) + (11 × 16)
- = 144 + 22 + 176 = **342 g/mol**
- Mass = Number of moles × Molecular weight = 0.5 × 342 = **171 grams**

3. **Calculate the mass of 1.2 moles of N2:**
- Molecular weight of N2 = 2 × Atomic weight of Nitrogen (N)
- Atomic weight of Nitrogen (N) = 14 g/mol
- Therefore, Molecular weight of N2 = 2 × 14 = 28 g/mol
- Mass = Number of moles × Molecular weight = 1.2 × 28 = **33.6 grams**

4. **Calculate the mass of 22.4 liters of N2 at NTP:**
- At NTP, 22.4 liters of any gas corresponds to 1 mole.
- Therefore, mass of 1 mole of N2 = 28 grams (as calculated above).
- Mass = 1 × 28 = **28 grams**

### Summary of Masses:
- Mass of S2 = 64 grams
- Mass of sucrose (C12H22O11) = 171 grams
- Mass of N2 (1.2 moles) = 33.6 grams
- Mass of N2 (22.4 liters) = 28 grams

### Conclusion:
The maximum mass is from the second option, which is **171 grams** of sucrose (C12H22O11).