Number of Atoms = (Mass in grams / Molar Mass (g/mol)) * 6.022 * 10^23, this grams to atoms converter is a useful tool to calculate grams in atoms.
- Hydrogen: (2 g / 1.008 g/mol) × (6.022 × 10^23 atoms/mol) = 1.194 × 10^24 atoms
- Oxygen: (16 g / 16.00 g/mol) × (6.022 × 10^23 atoms/mol) = 6.022 × 10^23 atoms
- Iron: (55.85 g / 55.85 g/mol) × (6.022 × 10^23 atoms/mol) = 6.022 × 10^23 atoms
- Gold: (100 g / 196.97 g/mol) × (6.022 × 10^23 atoms/mol) = 3.057 × 10^23 atoms
- Uranium: (238 g / 238.03 g/mol) × (6.022 × 10^23 atoms/mol) = 6.022 × 10^23 atoms
Grams to Atoms Calculator
| Element | Molar Mass (g/mol) | 1 gram to Atoms | 10 grams to Atoms | 50 grams to Atoms | 100 grams to Atoms |
|---|---|---|---|---|---|
| Hydrogen (H) | 1.01 | (1/1.01) 6.022 10^23 ≈ 5.94 * 10^24 | (10/1.01) 6.022 10^23 ≈ 5.94 * 10^25 | (50/1.01) 6.022 10^23 ≈ 2.97 * 10^26 | (100/1.01) 6.022 10^23 ≈ 5.94 * 10^26 |
| Carbon (C) | 12.01 | (1/12.01) 6.022 10^23 ≈ 5.01 * 10^22 | (10/12.01) 6.022 10^23 ≈ 5.01 * 10^23 | (50/12.01) 6.022 10^23 ≈ 2.51 * 10^24 | (100/12.01) 6.022 10^23 ≈ 5.01 * 10^24 |
| Oxygen (O) | 16.00 | (1/16.00) 6.022 10^23 ≈ 3.76 * 10^22 | (10/16.00) 6.022 10^23 ≈ 3.76 * 10^23 | (50/16.00) 6.022 10^23 ≈ 1.88 * 10^24 | (100/16.00) 6.022 10^23 ≈ 3.76 * 10^24 |
| Silicon (Si) | 28.09 | (1/28.09) 6.022 10^23 ≈ 2.56 * 10^22 | (10/28.09) 6.022 10^23 ≈ 2.56 * 10^23 | (50/28.09) 6.022 10^23 ≈ 1.28 * 10^24 | (100/28.09) 6.022 10^23 ≈ 2.56 * 10^24 |
| Aluminum (Al) | 26.98 | (1/26.98) 6.022 10^23 ≈ 2.66 * 10^22 | (10/26.98) 6.022 10^23 ≈ 2.66 * 10^23 | (50/26.98) 6.022 10^23 ≈ 1.33 * 10^24 | (100/26.98) 6.022 10^23 ≈ 2.66 * 10^24 |
| Iron (Fe) | 55.85 | (1/55.85) 6.022 10^23 ≈ 1.28 * 10^22 | (10/55.85) 6.022 10^23 ≈ 1.28 * 10^23 | (50/55.85) 6.022 10^23 ≈ 6.40 * 10^23 | (100/55.85) 6.022 10^23 ≈ 1.28 * 10^24 |
| Copper (Cu) | 63.55 | (1/63.55) 6.022 10^23 ≈ 1.13 * 10^22 | (10/63.55) 6.022 10^23 ≈ 1.13 * 10^23 | (50/63.55) 6.022 10^23 ≈ 5.65 * 10^23 | (100/63.55) 6.022 10^23 ≈ 1.13 * 10^24 |
| Silver (Ag) | 107.87 | (1/107.87) 6.022 10^23 ≈ 6.65 * 10^21 | (10/107.87) 6.022 10^23 ≈ 6.65 * 10^22 | (50/107.87) 6.022 10^23 ≈ 3.32 * 10^23 | (100/107.87) 6.022 10^23 ≈ 6.65 * 10^23 |
| Gold (Au) | 196.97 | (1/196.97) 6.022 10^23 ≈ 3.65 * 10^21 | (10/196.97) 6.022 10^23 ≈ 3.65 * 10^22 | (50/196.97) 6.022 10^23 ≈ 1.82 * 10^23 | (100/196.97) 6.022 10^23 ≈ 3.65 * 10^23 |
| Lead (Pb) | 207.20 | (1/207.20) 6.022 10^23 ≈ 3.47 * 10^21 | (10/207.20) 6.022 10^23 ≈ 3.47 * 10^22 | (50/207.20) 6.022 10^23 ≈ 1.73 * 10^23 | (100/207.20) 6.022 10^23 ≈ 3.47 * 10^23 |
Grams to atoms Conversion Formula
Number of atoms = (Mass in grams / Atomic mass) × Avogadro’s constant
Where:
- Mass is measured in grams (g)
- Atomic mass is expressed in grams per mole (g/mol)
- Avogadro’s constant is approximately 6.022 × 10^23 atoms/mol
This formula is based on the relationship between the mole concept and Avogadro’s constant, which represents the number of particles (atoms, molecules, or formula units) in one mole of a substance.
More Calculators:
How do you convert grams to atoms?
To convert grams to atoms, follow these steps:
- Identify the element or compound you’re working with.
- Look up the atomic mass of the element or the molar mass of the compound in a periodic table or reference material.
- Divide the given mass in grams by the atomic (or molar) mass. This gives you the number of moles.
- Multiply the number of moles by Avogadro’s constant to get the number of atoms.
For example, let’s convert 10 grams of carbon to atoms:
- Element: Carbon (C)
- Atomic mass of carbon: 12.01 g/mol
- Number of moles = 10 g / 12.01 g/mol = 0.8326 moles
- Number of atoms = 0.8326 moles × (6.022 × 10^23 atoms/mol) = 5.014 × 10^23 atoms
How many grams are in an atom?
The mass of a single atom is incredibly small and is typically expressed in atomic mass units (amu) rather than grams.
We can calculate the mass of one atom in grams using the following relationship:
Mass of one atom (g) = Atomic mass (g/mol) / Avogadro’s constant (atoms/mol)
For example, the mass of one carbon atom:
- Atomic mass of carbon: 12.01 g/mol
- Mass of one carbon atom = 12.01 g/mol / (6.022 × 10^23 atoms/mol) = 1.994 × 10^-23 g
As you can see, the mass of a single atom is an extremely small number when expressed in grams.
