The following quantities of trace gases were found in a 1.0...

The following quantities of trace gases were found in a 1.0 mL sample of air. Calculate the number of moles of each compound in the sample. a. $1.4 \times 10^{13}$ molecules of $\mathrm{H}_{2}(g)$ b. $1.5 \times 10^{14}$ atoms of $\mathrm{He}(g)$ c. $7.7 \times 10^{12}$ molecules of $\mathrm{N}_{2} \mathrm{O}(g)$ d. $3.0 \times 10^{12}$ molecules of $\mathrm{CO}(g)$

The following quantities of trace gases were found in a 1.0 mL sample of air. Calculate the number of moles of each compound in the sample.
a. $1.4 \times 10^{13}$ molecules of $\mathrm{H}_{2}(g)$
b. $1.5 \times 10^{14}$ atoms of $\mathrm{He}(g)$
c. $7.7 \times 10^{12}$ molecules of $\mathrm{N}_{2} \mathrm{O}(g)$
d. $3.0 \times 10^{12}$ molecules of $\mathrm{CO}(g)$

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Key Concepts

Avogadro's Number

Avogadro's number, approximately 6.022 × 10^23, is the number of atoms, molecules, or other particles in one mole of a substance. It serves as a conversion factor between the mass of a substance and the number of individual particles, allowing for quantitative comparisons in chemical reactions and processes.

Conversion of Particles to Moles

Converting a given number of particles to moles involves dividing the number of particles by Avogadro's number. This process is essential for bridging the gap between the microscopic world of atoms and molecules and the macroscopic amounts measured in the laboratory. Understanding this conversion is crucial in stoichiometry and in the analysis of gas samples or mixtures.

Mole Concept

The mole is a fundamental unit in chemistry used for quantifying the amount of a substance. It is defined as the amount of any substance that contains as many elementary entities (atoms, molecules, ions, etc.) as there are atoms in 12 grams of carbon-12. This concept allows chemists to count particles by weighing a substance and makes it possible to convert between the mass of a substance and the number of entities it contains.

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