1 / 7

The Mole – Volume Relationship

The Mole – Volume Relationship. Avogadro’s Hypothesis. equal volumes of gases at the same temperature and pressure contain the equal number of particles. Number of moles to volume(L) and volume(L) to moles.

ferdinand
Download Presentation

The Mole – Volume Relationship

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 – Volume Relationship

  2. Avogadro’s Hypothesis • equal volumes of gases at the same temperature and pressure contain the equal number of particles.

  3. Number of moles to volume(L) and volume(L) to moles • at standard temperature (0°C) and pressure (1 atmosphere), one mole of any gas has a volume of 22.4 L • this is called the molar volume of a gas

  4. Find the volume (in liters) of .60 moles of SO2 gas. .60 mol SO2 x 22.4 L SO2 1 1 mol SO2 = 13.0 L SO2 • Find the number of moles in 0.200 L of H2 gas. • 0.200 L H2 x 1 mole H2__ • 1 22.4 L H2 = 8.93 x 10-3 mol H2

  5. Volume to number of particles… and so on • Find the number of particles in 3.5 L of chlorine gas (Cl2). • 3.5 L Cl2x 1 mole Cl2_ x _6.02 X 1023 particles Cl2 • 1 22.4 L Cl21 mole = 9.41 X 1022 molecules Cl2 • Find the volume of 51.2 g of chlorine gas (Cl2). • 51.2 g Cl2x 1 mole Cl2_ x _22.4 L Cl2 • 1 71.0 g Cl2 1 mole = 16.2 L Cl2

More Related