Calculate the number of atoms in each sample. a. 5.18 g P

Verified step by step guidance

Determine the molar mass of phosphorus (P) from the periodic table.

Use the formula: number of moles = mass (g) / molar mass (g/mol) to calculate the moles of phosphorus.

Use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles of phosphorus to atoms.

Multiply the number of moles by Avogadro's number to find the total number of atoms.

Ensure all units cancel appropriately, leaving you with the number of atoms as the final unit.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For phosphorus (P), the molar mass is approximately 30.97 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 sample based on its mass.

Recommended video:

Guided course