Study your flashcards anywhere!

Download the official Cram app for free >

  • Shuffle
    Toggle On
    Toggle Off
  • Alphabetize
    Toggle On
    Toggle Off
  • Front First
    Toggle On
    Toggle Off
  • Both Sides
    Toggle On
    Toggle Off
  • Read
    Toggle On
    Toggle Off

How to study your flashcards.

Right/Left arrow keys: Navigate between flashcards.right arrow keyleft arrow key

Up/Down arrow keys: Flip the card between the front and back.down keyup key

H key: Show hint (3rd side).h key

A key: Read text to speech.a key


Play button


Play button




Click to flip

32 Cards in this Set

  • Front
  • Back
-Defined as the force per unit area on a surface

-caused by collisions
-defined as the pressure exerted by a force of one newton acting on an area of one square meter
the force that will increase the speed of a one kilogram mass by one meter per second each second it's applied
millimeter of mercury
-unit of pressure

-symbolized mm Hg
-device used to measure atmospheric pressure
atmosphere of pressure
(atm) defined as being exactly quivalent to 760mm Hg
ideal gas
an imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory
kinetic-molecular theory (4 constants)
-based on the idea that pa rticles of matter are always in motion
1) gases consist of large #s of tiny particles that are far apart
2) elastic collisions
3) constant, rapid, random motion
4) no forces of attraction or repulision (weak dispersion forces)
real gas
a gas that does not behave completely according to the assumptions of the kinetic-molecular theory
-gas particles glide easily past one another

-liquids and gases that flow
elastic collision
- collisions between gas particles and between particles and container walls are elastic collisions

- no net loss of kinetic energy
a process by which gas particles under pressure pass through a tiny opening
ideal gas constant
R= 0.0821 (L X atm / mol X k)

the constant R
spontaneous mixing of the particles of two substances caused by their random motion
ideal gas law

R= 0.0821 L atm/ mol K

the mathematical relationship of P,V,T and mols
standard molar volume of a gas
the volume ocupied by one mole of a gas at STP

found to be 22.4 L
Avogadro's Law
states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
Guy-Lussac's law of combining volumes of gases
states that at cosntant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers
Graham's law of effusion
R1 radical MW2
R2= radical MW1
Boyle's law

Charle's law
the process by which a liquid or solid changes to a gas
process of diffusion to where a gas fills its container
mm --> atm
divide by 760
C --> K
+ 273
standard temperature and pressure
scientists have agreed on standard conditions of 1 atm pressure and 0 degrees C

absolute zero
- 273. 15 degrees C

given a value of zero on the kelvin scale
gas laws
simple mathematical relationships between the volume, temperature, pressure, and quantity of a gas
partial pressure
preesure of each gas in a mixture
Guy- Lussac's law
Dalton's law of partial pressures
Pt= p1 + p2 +p3
combined gas law