1 / 7

The Mole

The Mole. Chapter 11 Chemistry. The Mole. The mole ( mol ) is the SI unit used to measure the amount of a substance. A mole of anything contains 6.02 x10 23 particles. This number is also known as Avogadro’s number. A mole is also equal to the atomic mass of an element in grams.

rooney-watts
Télécharger la présentation

The Mole

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. The Mole Chapter 11 Chemistry

  2. The Mole • The mole (mol) is the SI unit used to measure the amount of a substance. • A mole of anything contains 6.02 x1023 particles. This number is also known as Avogadro’s number. • A mole is also equal to the atomic mass of an element in grams. • 1.0 mol of carbon is 12.0 g. • 1.0 mol of oxygen gas is 32.0 g.

  3. Converting Moles to Particles • The conversion factor is 1 mol = 6.02 x1023 particles (molecules, atoms, etc.) • Practice Problems • Determine the number of atoms in 2.50 mol of zinc. • Calculate the number of water molecules in 11.5 moles of water. • Convert the number of atoms of the following to moles: a. 5.75 x1024 atoms Al b. 3.75 x1024 molecules CO2 c. 3.58 x 1023 molecules ZnCl2

  4. Mass and the Mole • The mass in grams of one mole of any pure substance is called the molar mass. • The molar mass of any element is numerically equal to its atomic mass and has the units g/mol. • Molar mass is used as a conversion to convert mass of a substance to its molar quantity and its molar quantity to its molar mass.

  5. Practice Problems • Determine the mass in grams of each of the following: • 3.57 mol Al • 42.6 mol Si • 3.45 mol Co • 2.45 mol Zn • Determine the number of moles in each of the following: • 25.5 g Ag • 300.0 g S • 125 g Zn • 1.00 kg Fe

  6. Conversions from Mass to Atoms • When given the mass of a substance to convert to number of atoms use the following steps: • Convert from mass to moles using molar mass. • Convert from moles to number of atoms using 6.02 x1023.

  7. Practice Problems • How many atoms are in each of the following samples: • 55.2 g Li • 0.230 g Pb • 11.5 g Hg • 45.6 g Si • 0.120 g Ti • What is the mass in grams of each of the following: • 6.02 x1024 atoms Bi • 1.00 x 1024 atoms Mn • 3.40 x 1022 atoms He • 1.50 x 1015 atoms N • 5.00 x 1020atoms U

More Related