Chapter 5 Key Terms Flashcards
Atmosphere (atm)
A unit of pressure based on the average pressure of air at sea level.
Avogadro’s Law
The law that state the volume of a gas is directly proportional to its amount in moles. V/n=V/n
Barometer
An instrument used to measure atmospheric pressure
Boyles Law
V1/P1=V2/P2
Charles’s Law
V1/T1=V2/T2
Dalton’s Law of Partial Pressures
The sum of the partial pressures of the components in a gas mixture is the total pressure
Diffusion
The process of a gas spreading through a space
Effusion
The process where a gas escapes into a vacuum through a small opening
Hypoxia
When you’re running out of oxygen and start feeling symptoms
Ideal Gas Constant (R)
R=.08206 Latm/molK
Ideal Gas Law
PV=nRT
Kinetic Molecular Theory
A model of an ideal gas as a collection of particles in constant motion with many collisions
Manometer
Instrument used to measure pressure (u-shaped)
Mean Free Path
Average distance a molecule travels between collision
mmHg
Unit of pressure referring to amount needed to raise 1 mmHg
Molar Volume
Volume of 1 mol of a gas. At STP, it is 22.4L
Mole Fraction
Number of moles of a component in a mixture divided by total moles of that mixture
Nitrogen narcosis
If there’s too much nitrogen you act drunk
Oxygen toxicity
If there’s too much oxygen, you twitch and seize
Partial Pressure
Pressure of one gas in a mixture as compared to the whole
Pascal (Pa)
SI unit of pressure. 1 N/M^2
Pressure
Force exerted per unit area
STP, Standard Temperature and Pressure
T= 0*C P= 1 atm
