Which of the following have maximum mass?

Options

A. 1 g iron
B. `10^(20)` molecdules of `CO_(2)`
C. `0.1` mole of `NH_(3)`
D. `10^(22)` atoms of carbon

Explanation

To determine which of the given substances has the maximum mass, we will calculate the mass of each substance based on the information provided in the video transcript.

### Step-by-Step Solution:

1. **Calculate the mass of 1 gram of Iron (Fe)**:
- Molar mass of Iron (Fe) = 56 g/mol.
- For 1 gram of Iron, the number of moles = mass / molar mass = 1 g / 56 g/mol = 1/56 moles.

2. **Calculate the mass of 10^20 molecules of Carbon Dioxide (CO2)**:
- Molar mass of CO2 = 44 g/mol.
- 1 mole of any substance contains Avogadro's number of molecules, which is approximately 6.022 x 10^23.
- Therefore, the mass of 10^20 molecules of CO2 = (44 g/mol) * (10^20 molecules / 6.022 x 10^23 molecules) = 44 / (6.022 x 10^3) g = 7.3 x 10^-3 g.

3. **Calculate the mass of 0.1 mole of Ammonia (NH3)**:
- Molar mass of Ammonia (NH3) = 17 g/mol.
- Mass of 0.1 mole of NH3 = 0.1 moles * 17 g/mol = 1.7 g.

4. **Calculate the mass of 10^22 atoms of Carbon (C)**:
- Molar mass of Carbon (C) = 12 g/mol.
- The mass of 10^22 atoms of Carbon = (12 g/mol) * (10^22 atoms / 6.022 x 10^23 atoms) = 12 / (6.022 x 10^1) g = 1.99 x 10^-1 g.

5. **Compare the calculated masses**:
- Mass of Iron = 1 g.
- Mass of 10^20 molecules of CO2 = 7.3 x 10^-3 g.
- Mass of 0.1 mole of NH3 = 1.7 g.
- Mass of 10^22 atoms of Carbon = 1.99 x 10^-1 g.

### Conclusion:
The maximum mass among the given substances is that of **1 gram of Iron (Fe)**, which is greater than the masses of CO2, NH3, and Carbon.