1 / 9

Chapter 3 Section 4 Notes

Chapter 3 Section 4 Notes. Using Moles to Count Atoms. What is a mole?. The SI base unit that describes the amount of a substance; a collection of a very large number of particles. What is a mole useful for?. Counting small particles. Avogadro’s Constant.

dee
Télécharger la présentation

Chapter 3 Section 4 Notes

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 3 Section 4 Notes Using Moles to Count Atoms

  2. What is a mole? • The SI base unit that describes the amount of a substance; a collection of a very large number of particles.

  3. What is a mole useful for? • Counting small particles

  4. Avogadro’s Constant • Avogadro’s Constant: the number of particles in 1 mol • Equals 6.022 x 1023 particles/ mol • 602,213,670,000,000,000,000,000 particles • How does Avogadro’s constant relate to a mole of something? • It is the number of particles in one mole of anything.

  5. Moles and Grams are related • Molar Mass: the mass in grams of 1 mol of a substance • How do you find molar mass? • The average atomic mass is equal to molar mass. • Simply look on the Periodic Table!

  6. Practice • Determine the molar mass of the following elements: (Round to the nearest hundredth) • Manganese, Mn • 54.94 g/mol • Cadmium, Cd • 112.41 g/mol • Arsenic, As • 74.92 g/mol • Strontium, Sr • 87.62 g/mol

  7. More Practice • Determine the mass, in grams of each of the following: • 0.48 mol of platinum • 2.50 mol of sulfur 0.48 mol x 195.08 g = 94 g 1 mol 2.50 mol x 32.07 g = 80.2 g 1 mol

  8. Even More Practice • Determine how many moles are present in each of the following: • 620 g of mercury • 11 g of silicon 620 g x 1 mol = 3.09 mol 200.59 g 11 g x 1 mol = 0.39 mol 28.09 g

  9. Compounds also have molar mass • To find the molar mass of a compound, add up the molar masses of all the atoms in a molecule of the compound. • Example: H2O • Molar Mass of Hydrogen: 1.01 x 2 = 2.02 g/mol • Molar Mass of Oxygen: 16 g/mol • Total Mass of H2O: 2.02 g + 16 g = 18.02 g/mol

More Related