Calculate the number of atoms in each sample. a. 14.955 g Cr

Verified step by step guidance

1. Identify the molar mass of chromium (Cr) from the periodic table, which is approximately 51.9961 g/mol.
2. Use the formula to convert grams to moles: \( \text{moles of Cr} = \frac{\text{mass of Cr in grams}}{\text{molar mass of Cr}} \).
3. Substitute the given mass of chromium (14.955 g) and its molar mass into the formula to find the moles of Cr.
4. Use Avogadro's number, \( 6.022 \times 10^{23} \text{ atoms/mol} \), to convert moles of Cr to atoms: \( \text{atoms of Cr} = \text{moles of Cr} \times 6.022 \times 10^{23} \text{ atoms/mol} \).
5. Perform the multiplication to find the total number of atoms in the sample.

Key Concepts

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For chromium (Cr), the molar mass is approximately 51.996 g/mol. This value is essential for converting grams of a substance to moles, which is a necessary step in determining the number of atoms in a sample.

Avogadro's Number

Avogadro's number, approximately 6.022 x 10²³, 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). It is crucial for calculating the total number of atoms in a given mass of an element.

Conversion from Grams to Atoms

To find the number of atoms in a sample, one must first convert the mass of the sample to moles using the molar mass, and then multiply the number of moles by Avogadro's number. This two-step conversion is fundamental in stoichiometry, allowing for the quantification of particles in a chemical context.