1. What is AMU and g/mol?

The atomic mass unit (AMU) and grams per mole (g/mol) are numerically equivalent units used to express atomic and molecular masses. 1 AMU is defined as 1/12 the mass of a carbon-12 atom.

2. How Does the Conversion Work?

The conversion is straightforward:

Where:

• \( g/mol \) — Grams per mole
• \( AMU \) — Atomic Mass Unit

Explanation: The mole was defined such that the mass of one mole of a substance in grams is numerically equal to its atomic or molecular mass in AMU.

3. Importance of the Conversion

Details: This conversion is fundamental in chemistry for relating microscopic atomic masses to macroscopic measurable quantities.

4. Using the Calculator

Tips: Simply enter the value in g/mol to get the equivalent in AMU. The conversion is exact with no rounding needed.

5. Frequently Asked Questions (FAQ)

Q1: Why are g/mol and AMU numerically equal?
A: The mole was defined to make the numerical values match - 1 mole of carbon-12 atoms weighs exactly 12 grams and each atom weighs exactly 12 AMU.

Q2: Is there any situation where they wouldn't be equal?
A: No, the equality holds for all elements and compounds by definition of the mole.

Q3: What's the difference between AMU and g/mol?
A: AMU is the mass of a single atom/molecule, while g/mol is the mass of Avogadro's number of atoms/molecules. The numbers are equal but the scales differ.

Q4: Why do we need both units?
A: AMU is used for single particles, while g/mol is more practical for laboratory measurements of substances.

Q5: How precise is this conversion?
A: It's exact by definition, not an approximation.