Suppose that the atomic mass of C-12 is taken to be 5.000 amu and that a mole is defined as the

step 1 So we're going to define a mole as a number of atoms in 5 ,000 grams, that's 5 kilograms, of car

Suppose that the atomic mass of C-12 is taken to be 5.000...

Suppose that the atomic mass of $\mathrm{C}-12$ is taken to be 5.000 amu and that a mole is defined as the number of atoms in $5.000 \mathrm{~kg}$ of carbon-12. How many atoms would there be in one mole under these conditions? (Hint: There are $6.022 \times 10^{23} \mathrm{C}$ atoms in $12.00 \mathrm{~g}$ of $\left.\mathrm{C}-12 .\right)$

Key Concepts

Atomic Mass Unit

The atomic mass unit (amu) is a unit of mass used to express atomic and molecular weights. It is defined such that one twelfth of the mass of a carbon-12 atom is exactly one atomic mass unit. This concept provides a scale for comparing the masses of different atoms on a relative basis.

Molar Mass

Molar mass links the mass of a substance to the number of atoms or molecules it contains. In chemistry, the mass of one mole of a substance (often given in grams per mole) is numerically equal to the average mass of one atom or molecule in atomic mass units. This allows for conversion between mass and moles using the concept of atomic mass units.

Mole

A mole is a unit used in chemistry to quantify the number of particles in a sample, whether they are atoms, molecules, ions, etc. It is historically defined based on the number of atoms in 12.00 g of carbon-12, which is approximately 6.022×10^23. When the definition of a mole is adjusted (such as by changing the reference mass), the number of particles corresponding to that mole changes accordingly.

Avogadro's Number

Avogadro's number (approximately 6.022×10^23) is the fundamental constant that denotes the number of particles in one mole of a substance, based on the conventional definition. It serves as the bridge between the atomic scale and the macroscopic scale, allowing chemists to count atoms by weighing a substance.

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