or

or

taken

why

Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account.

Don't know
Know
remaining cards
Save
0:01

 Flashcards Matching Hangman Crossword Type In Quiz Test StudyStack Study Table Bug Match Hungry Bug Unscramble Chopped Targets

Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

Normal Size     Small Size show me how

# Chapter 14

### Chapter 14: The behavior of Gases

Why are gases easier to compress than solids or liquids? because gases are easily compressed due to the space between particles.
What is compressibility? a measure of how much the volume decreases under pressure.
What does Boyle's law state? for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure.
How are the temperature and volume of a gas related? as the temperature of an enclosed gas increases, the volume increased if the pressure is constant.
Charles's Law: the volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant.
Gay-Lussacs' Law: the pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant.
Combined gas law: a law that combines Boyle's, Charles's and Gay-Lussac's laws.
Ideal gas constant (R): has the value 8.31 (L x Pa)(K x mol)
Ideal gas law: P,V,T and n .
Partial pressure: the contribution each gas in a mixture makes to the total pressure.
Dalton's law of partial pressures: at constant volume and temperatures, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.
Diffusion: the tendency of molecules to move towards areas of lower concentration until the concentration is uniform throughout.
Effusion: gas escapes through a tiny hole in its container.
Graham's law of effusion: the rate of effusion of a gas is inversely proportional to the square root of the gas's molar mass.
Created by: jmhschemistry