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 $\mathrm{H}_{2}$ b. $1.5 \times 10^{14}$ atoms of $\mathrm{He}$ c. $7.7 \times 10^{12}$ molecules of $\mathrm{N}_{2} \mathrm{O}$ d. $3.0 \times 10^{12}$ molecules of $\mathrm{CO}$

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 $\mathrm{H}_{2}$
b. $1.5 \times 10^{14}$ atoms of $\mathrm{He}$
c. $7.7 \times 10^{12}$ molecules of $\mathrm{N}_{2} \mathrm{O}$
d. $3.0 \times 10^{12}$ molecules of $\mathrm{CO}$

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Key Concepts

Conversion Between Particle Count and Moles

This concept involves calculating the number of moles from a given number of atoms or molecules by using Avogadro's Number as the conversion factor. By dividing the number of particles by Avogadro's Number, one can determine the corresponding amount in moles, facilitating quantitative analysis in chemical reactions and processes.

Avogadro's Number

Avogadro's Number (approximately 6.02 x 10^23) is the number of particles in one mole of a substance. It is a cornerstone constant in chemistry that enables the conversion from a count of atoms or molecules to the amount in moles. This constant is used universally when relating quantities at the molecular or atomic level to amounts that can be measured and manipulated in the laboratory.

Mole Concept

The mole is a fundamental unit in chemistry that represents a specific number of particles, typically atoms, molecules, or ions. It provides a bridge between the atomic scale and everyday amounts of material, allowing chemists to count particles by weighing macroscopic samples. This concept is essential for converting between mass, number of particles, and moles in chemical calculations.

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