Calculate the mass in grams for each of the following: (a) 2.95 ×10^23 atoms of mercury, Hg (b)

step 1 If you have the number of atoms, molecules, or formula units of an element or compound, you shou

Calculate the mass in grams for each of the following: (a)...

Calculate the mass in grams for each of the following:
(a) $2.95 \times 10^{23}$ atoms of mercury, $\mathrm{Hg}$
(b) $1.16 \times 10^{22}$ molecules of nitrogen, $\mathrm{N}_{2}$
(c) $5.05 \times 10^{21}$ formula units of barium chloride, $\mathrm{BaCl}$ ?

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Key Concepts

Molar Mass

Molar Mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It links the microscopic scale (atom/molecule/molecule's mass) to the macroscopic scale used in the laboratory. In calculations, it provides the bridge between the number of moles and the mass in grams.

Avogadro's Number

Avogadro's Number (6.022 x 10^23 mol^-1) is the basic conversion factor that relates the number of particles (atoms, molecules, or formula units) to the amount of substance in moles. It is essential in converting large counts of tiny particles into a more manageable amount expressed in moles, which can then be used with molar masses.

Mole Concept

The Mole Concept is a fundamental principle in chemistry that allows for quantifying a chemical substance by defining one mole as containing Avogadro's Number of particles. This concept is critical in stoichiometry for converting between the number of particles, moles, and mass, enabling the comparison of quantities of different substances based on their chemical formulas.

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