Final answer:
The molar mass of nitrogen (N) for 6.022 x 10²³ particles, which is one mole of diatomic nitrogen (N₂), is 28.0134 grams per mole.
Step-by-step explanation:
The question asks for the molar mass of 6.022 x 10²³ particles of nitrogen (N). To find the molar mass of nitrogen, we must use the molecular mass of diatomic nitrogen (N₂) since nitrogen typically exists in this form. From the periodic table, the atomic mass of nitrogen is approximately 14.0067 amu. Since there are two nitrogen atoms in a molecule of diatomic nitrogen, we multiply this value by 2.
Molar mass of N₂ = 2 x 14.0067 g/mol = 28.0134 g/mol.
Since one mole of any substance contains Avogadro's number of particles or molecules, which is 6.022 x 10²³, the molar mass applies to this many particles. We have thus determined the molar mass of one mole of nitrogen molecules, which contains 6.022 x 10²³ individual nitrogen molecules.