If the atomic weight of an element is x, what is the mass in grams of 6.02 x 10^23 atoms of the element? How does your answer compare numerically with the atomic weight of element x?

Verified step by step guidance

1. Step 1: Understand that 6.02 x 10^23 atoms is Avogadro's number, which represents one mole of atoms.
2. Step 2: Recognize that the atomic weight of an element in atomic mass units (amu) is numerically equal to the mass of one mole of that element in grams.
3. Step 3: Since the atomic weight of the element is given as x, the mass of one mole (6.02 x 10^23 atoms) of the element is x grams.
4. Step 4: Conclude that the mass in grams of 6.02 x 10^23 atoms of the element is x grams.
5. Step 5: Note that the mass in grams of 6.02 x 10^23 atoms is numerically equal to the atomic weight of the element, which is x.

Key Concepts

Atomic Weight

Atomic weight, often expressed in atomic mass units (amu), is the weighted average mass of an element's isotopes relative to 1/12th the mass of a carbon-12 atom. It reflects the mass of a single atom of the element and is crucial for converting between moles and grams in chemical calculations.

Avogadro's Number

Avogadro's number, approximately 6.02 x 10^23, is the number of atoms, ions, or molecules in one mole of a substance. This constant allows chemists to relate the macroscopic scale of substances (grams) to the microscopic scale (individual atoms or molecules), facilitating calculations involving moles.

Molar Mass Calculation

The molar mass of an element is numerically equal to its atomic weight in grams per mole. To find the mass of a specific number of atoms, one can use the formula: mass = (number of atoms / Avogadro's number) x molar mass. This relationship helps compare the mass of a given number of atoms to the atomic weight.