AP Chemistry - Moles and Molar Mass 1.1

Why do chemists use moles?

• To count particles directly

• To relate units of mass to the number of particles in a chemical reaction

• To measure the mass of substances

• To calculate the atomic mass of elements

What is the number of particles in a mole?

• 6.02 x 10^23

• 1

• 12.01

• 342.3

What is the mass of one molecule of sucrose?

• 12.01 atomic mass units

• 1.01 atomic mass units

• 16 atomic mass units

• 342.3 atomic mass units

What is the mass of one mole of sucrose molecules?

• 12.01 grams

• 1.01 grams

• 16 grams

• 342.3 grams

What is the molar mass of H2SO4?

• 98.08 grams per mole

• 12.01 grams per mole

• 1.01 grams per mole

• 16 grams per mole

How many atoms are there in one molecule of H2SO4?

• 1

• 2

• 3

• 4

Tags

NGSS.MS-PS1-1

What is the formula mass of Al(NO3)3?

• 196.01 atomic mass units

• 12.01 atomic mass units

• 1.01 atomic mass units

• 16 atomic mass units

What is the molar mass of Al(NO3)3?

• 196.01 grams per mole

• 12.01 grams per mole

• 1.01 grams per mole

• 16 grams per mole

What is the mass of one molecule of Al(NO3)3?

• 196.01 atomic mass units

• 12.01 atomic mass units

• 1.01 atomic mass units

• 16 atomic mass units

How many atoms are there in one molecule of Al(NO3)3?

• 1

• 2

• 3

• 4

Tags

NGSS.MS-PS1-1