1 / 3

Understanding Gas Mixtures: Partial Pressures and Mole Fractions

Learn about partial pressures, Dalton’s Law, and collecting wet gases through water vapor. Explore the ideal gas law for gas mixtures, the calculation of total pressure, and the impact of water vapor on gas collections.

tuyet
Download Presentation

Understanding Gas Mixtures: Partial Pressures and Mole Fractions

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. Unit 7.5 Gas Mixtures: Partial Pressures and Mole fractions

  2. VI) (7.5) Gas Mixtures: Partial Pressures and Mole fractions iii) are the pressures of the gases if they were alone. and a) Introduction: i.) The ideal gas law applies to pure gases and gas mixtures ii) For a mixture of two gases (A and B), the total pressure is given by the expression: These are called partial pressures iv) So: Ptot = PA + PB v) This is referred to as Dalton’s Law of partial pressures: The total pressure of a gas mixture is the sum of the partial pressures of the components of the mixture.

  3. VI) (7.5) Gas Mixtures: Partial Pressures and Mole fractions b) Wet Gases; Partial pressure of water: i) When any gas is collected by bubbling through water, it picks up water vapor. ii) Dalton’s law of partial pressures can be applied to the resulting gas mixture: 1) Ptot = Pwater + Pother 2) Pwater is a fixed value at any given temperature. (appendix 1)

More Related