1. What is AMU?

The atomic mass unit (AMU) is a standard unit of mass that quantifies mass on an atomic or molecular scale. 1 AMU is defined as one twelfth of the mass of an unbound neutral atom of carbon-12 in its nuclear and electronic ground state.

2. How Does the Conversion Work?

The conversion between grams per mole (g/mol) and atomic mass units (AMU) is:

Where:

• \( \text{g/mol} \) — Grams per mole (molar mass)
• \( \text{AMU} \) — Atomic Mass Unit (unified atomic mass unit)

Explanation: The molar mass of a substance in grams per mole is numerically equal to the average mass of one molecule of that substance in atomic mass units.

3. Importance of AMU Calculation

Details: Understanding the relationship between g/mol and AMU is fundamental in chemistry for calculating molecular weights, stoichiometric calculations, and understanding atomic-scale masses.

4. Using the Calculator

Tips: Simply enter the value in grams per mole (g/mol) and the calculator will provide the equivalent value in atomic mass units (AMU).

5. Frequently Asked Questions (FAQ)

Q1: Why are g/mol and AMU numerically equivalent?
A: This is by definition - the mole was defined such that the molar mass of carbon-12 is exactly 12 g/mol, and carbon-12 has a mass of exactly 12 AMU.

Q2: What's the difference between AMU and g/mol?
A: They represent the same numerical value but different units - AMU is the mass of a single atom/molecule, while g/mol is the mass of one mole (6.022×10²³) of atoms/molecules.

Q3: Is this conversion exact?
A: Yes, the conversion is exact by definition in the modern system of units.

Q4: Does this work for all elements and compounds?
A: Yes, the relationship holds for the molar mass of any element or compound.

Q5: What about Dalton (Da) units?
A: 1 Dalton (Da) = 1 AMU, so the same conversion applies.