{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Chapter 6 M

# Chapter 6 M - CHAPTER 6 GASES CHM 25/Spring 2009 Prof R.S...

This preview shows pages 1–12. Sign up to view the full content.

CHAPTER 6 – GASES CHM 25/Spring 2009 Prof. R.S. Miller

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
Composition of Earth’s Atmosphere Compound %(Volume) Mole Fraction a Nitrogen 78.08 0.7808 Oxygen 20.95 0.2095 Argon 0.934 0.00934 C b di id 0 033 0 00033 Carbon dioxide 0.033 0.00033 Methane 2 x 10 -4 2 x 10 -6 Hydrogen 5 x 10 -5 5 x 10 -7 5 7 a. mole fraction = mol component/total mol in mixture.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
Properties of Gases Gases are highly compressible and occupy the full volume of their containers. When a gas is subjected to pressure, its volume decreases. Gases always form homogeneous mixtures with h other gases. Gases only occupy about 0.1 % of the volume of their containers their containers.
Measurement of Pressure

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
Elevation and Atmospheric Pressure
Units for Expressing Pressure Unit Value Atmosphere 1 atm Pascal (Pa) 1 atm = 1.01325 x 10 5 Pa Kilopascal (kPa) 1 atm = 101.325 kPa mmHg 1 atm = 760 mmHg Torr 1 atm = 760 torr Bar 1 atm = 1 01325 bar 1 atm 1.01325 bar mbar 1 atm = 1013.25 mbar psi 1 atm = 14 7 psi 1 atm = 14.7 psi

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
Manometer
Boyle’s Law (1627-1691) Boyle’s Law: the volume of a fixed quantity of gas is inversely Boyle s Law: the volume of a fixed quantity of gas is inversely proportional to its pressure. Boyle (1627-1691) used a manometer to carry out the experiment.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document