TED-Ed: How big is a mole? (Not the animal, the other one.) - Daniel Dulek

The video tutorial introduces the concept of the mole in chemistry, explaining its significance in counting extremely small particles like atoms and molecules. It discusses Avogadro's hypothesis, which laid the foundation for the atomic theory, and introduces Avogadro's number, 6.02 x 10^23, as a way to quantify large numbers of particles. The tutorial uses visual analogies, such as a mole of donuts or basketballs, to help viewers grasp the enormity of a mole. Finally, it explains how chemists use the mole in practical applications, similar to how we use units like pounds or dozens in everyday life.

What was Avogadro's hypothesis about gases?

• Gases at the same temperature and pressure have equal numbers of particles.

• Gases at the same temperature and pressure have different numbers of particles.

• Gases at different temperatures have equal numbers of particles.

• Gases at different pressures have different numbers of particles.

What is Avogadro's number?

• 6.02 x 10^22

• 6.02 x 10^25

• 6.02 x 10^23

• 6.02 x 10^24

How many molecules are in 18.01 grams of water?

• 60.2 sextillion

• 602 sextillion

• 6.02 sextillion

• 6.02 trillion

If you had a mole of basketballs, what could you create?

• A lake the size of the Great Lakes

• A new planet the size of the Earth

• A mountain the size of Everest

• A city the size of New York

How do chemists use the concept of a mole?

• To measure the weight of substances

• To determine the color of substances

• To calculate the speed of reactions

• To count large quantities of small particles