What is the mass in grams of each of the following? a. 6.02 ×10^24 atoms Bi b. 1.00 ×10^24 atoms

step 1 In this problem, we have five substances given in subpart A, B, C, D and E. For each one of thes

What is the mass in grams of each of the following? a. 6.02...

What is the mass in grams of each of the following?
a. $6.02 \times 10^{24}$ atoms $\mathrm{Bi}$
b. $1.00 \times 10^{24}$ atoms $\mathrm{Mn}$
c. $3.40 \times 10^{22}$ atoms He
d. $1.50 \times 10^{15}$ atoms $\mathrm{N}$
e. $1.50 \times 10^{15}$ atoms $\mathrm{U}$

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Key Concepts

Molar Mass

Molar mass is the mass in grams of one mole of a substance. It directly relates the mass of a sample to the number of moles present, allowing conversions from moles to grams using the substance’s atomic or molecular weight.

Avogadro's Number

Avogadro's Number is a fundamental constant, approximately 6.02 x 10^23, representing the number of atoms or molecules in one mole of a substance. It is crucial for converting between the number of individual particles and the amount in moles.

Mole Concept

The mole is a basic chemical unit that gives a measure for the amount of substance. It allows chemists to count atoms, molecules, or other particles by relating them to a standard unit based on Avogadro's Number, bridging the microscopic and macroscopic scales.

Atom-to-Mole Conversion

This conversion involves dividing the number of atoms by Avogadro's Number to calculate the number of moles, which is then multiplied by the molar mass to obtain the mass in grams. It is a fundamental calculation in stoichiometry for relating microscopic particle counts to measurable masses.

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