Mole Conversions: From Moles to Grams and Molecules

Mr. Anderson introduces the concept of moles in chemistry, comparing it to a dozen using eggs as an analogy. He explains how moles are used to measure atoms and molecules, and discusses the relationship between moles and formula mass. The video covers conversions between moles, particles, and grams using the factor label method, and includes example problems to demonstrate these conversions.

Why is the concept of a mole used in chemistry?

• To calculate the speed of reactions

• To determine the color of compounds

• To measure the volume of liquids

• To deal with very small atoms in a usable amount

What is the numerical value of one mole?

• 1.01

• 24

• 6.022 x 10^23

• 12

How many eggs are in a dozen?

• 24

• 12

• 10

• 6

What is the formula mass of H2O?

• 32.06 grams

• 1.01 grams

• 16.00 grams

• 18.02 grams

What is the first step in converting moles to grams?

• Calculate the speed of reaction

• Find the volume of the substance

• Determine the formula mass from the periodic table

• Measure the temperature

What is the formula mass of H2SO4?

• 98.08 grams

• 18.02 grams

• 64.00 grams

• 32.06 grams

How many grams are in 0.200 moles of H2SO4?

• 32.06 grams

• 0.200 grams

• 98.08 grams

• 19.616 grams

What is the next step after converting grams to moles in the factor-label method?

• Convert moles to volume

• Convert moles to particles

• Convert moles to temperature

• Convert moles to speed

How many molecules are in 102.8 grams of H2O?

• 6.022 x 10^23

• 18.02 x 10^23

• 3.435 x 10^24

• 1.01 x 10^23

What is Avogadro's number?

• 1.01

• 32.06

• 18.02

• 6.022 x 10^23