Relative Atomic Mass Formula:
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Definition: Relative Atomic Mass of an Element is defined as the ratio of the average mass of atom of specific composition to the 1/12th of the mass of atom of nuclide C-12.
Purpose: It provides a standardized way to compare atomic masses across different elements.
The calculator uses the formula:
Where:
Explanation: The mass of the element's atom is compared to 1/12th the mass of a Carbon-12 atom, which serves as the standard reference.
Details: This measurement is fundamental in chemistry for stoichiometric calculations, determining molecular formulas, and understanding chemical reactions.
Tips: Enter the mass of the atom in kilograms and the mass of Carbon-12 atom (default 0.0120116 kg). All values must be > 0.
Q1: Why is Carbon-12 used as the standard?
A: Carbon-12 was chosen as the standard because it's a stable isotope with a well-defined mass and is easy to work with experimentally.
Q2: What's the typical mass of a Carbon-12 atom?
A: The exact mass is 1.992646547 × 10⁻²⁶ kg, but for practical calculations, 0.0120116 kg per mole is often used.
Q3: How precise should my measurements be?
A: For accurate results, measurements should be as precise as possible, ideally using mass spectrometry data.
Q4: Can I use atomic mass units (u) instead of kilograms?
A: Yes, but the calculator would need to be modified since it currently expects kilogram inputs.
Q5: How does this relate to molar mass?
A: The relative atomic mass in grams becomes the molar mass of the element (grams per mole).