Molar Mass and the Mole Lecture Notes

This set of vocabulary flashcards covers concepts from the August 2026 lecture on the Mole, Molar Mass, Avogadro's constant, and Dimensional Analysis.

$$C_6H_{12}O_6$$

The chemical formula for glucose, which consists of $6$ Carbons, $12$ Hydrogens, and $6$ Oxygens and has a molar mass of $180.18$.

Molar Mass

The total mass of a substance found by adding the total atomic mass of each atom in the chemical formula, expressed in units of $\text{g/mol}$ or $\text{g} \cdot \text{mol}^{-1}$.

$$\text{g/mol}$$

The unit for molar mass, standing for "grams per mole," indicating how many grams of a substance are in $1$ mole of that substance.

Dozen

A counting unit representing $12$ items.

Counting Units

Units used to represent specific quantities, such as Pair ($2$), Score ($20$), Gross ($144$), and Ream ($500$).

Mole ($mol$)

A counting unit used to measure the amount of substance, where $1$ mole contains exactly $6.02 \times 10^{23}$ elementary entities.

Avogadro constant

The number of elementary entities in one mole, equal to $6.02 \times 10^{23}$.

Particles

A collective term for elementary entities including Atoms, Ions, and Compounds (specifically Formula Units and Molecules).

Conversion Factors

Equalities used to change a measurement from one unit to another, such as converting between moles and particles ($1\,\text{mole} = 6.02 \times 10^{23}\,\text{particles}$).

Dimensional Analysis

A method of solving problems by starting with a given quantity and using conversion factors to cancel units until the desired unit is reached.

Potassium Carbonate

A chemical compound with the formula $K_2CO_3$.

Sodium Fluoride

A chemical compound with the formula $NaF$, which has the same number of formula units in $1$ mole as $K_2CO_3$ ($6.02 \times 10^{23}$) but a different mass.

Calcium Nitrate

A chemical compound with the formula $Ca(NO_3)_2$.

Ethanol

A chemical compound with the formula $C_2H_5OH$, often used in mass to molecule conversions.

Atomic Mass of Carbon ($C$)

$$12.01$$

Atomic Mass of Hydrogen ($H$)

$$1.01$$

Atomic Mass of Oxygen ($O$)

$$16.00$$

Atomic Mass of Cobalt ($Co$)

$$58.93\,\text{g/mol}$$

Atomic Mass of Helium ($He$)

$$4.00\,\text{g/mol}$$