Save
Busy. Please wait.
Log in with Clever
or
show password
Forgot Password?
Don't have an account?  Sign up 
Sign up using Clever
or
Username is available taken
show password


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. Your email address is only used to allow you to reset your password. See our Privacy Policy and Terms of Service.

Already a StudyStack user? Log In

Reset Password
Enter the associated with your account, and we'll email you a link to reset your password.
focusNode
Didn't know it?
click below
 
Knew it?
click below
Don't Know
Remaining cards (0)
Know
0:00
edit
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

Chemistry: Chapter 9

Kinetic Molecular Theory, Ideal & Real Gas Properties, Gas Laws, Mole Fraction

QuestionAnswer
properties of gasses 1. no definite shape or volume 2. exert pressure on surroundings 3. volumes change with temperature and pressure 4. gases mix completely with other gases 5. much less dense then solids or liquids
pressure P
volume V
temperature T
number of moles n
gas constant R
Boltzmann's constant k - 1.381x10^-23
Dalton's: partial pressure P
Dalton's: total pressure P (sub) tot
Dalton's: moles of component A n (sub) a
Dalton's: moles n
Dalton's: total moles n (sub) tot
Dalton's: speed (rate) u (sub) rms
Dalton's: attractive forces a
Dalton's: molecule size b
Maxwell-Blotzmann Distrtribution a distribution of molecular speeds; depends on the absolute temperature of the gas; as temperature increases, the distribution broadens, and the maximum shifts to higher speeds
3 different speeds average speed, root mean square speed, and most probable speed
average speed the average of the speeds of all the molecules
root mean square speed the speed of a molecule that has the average kinetic energy
most probable speed the speed of the largest number of molecules and the maximum in the Maxwell-Boltzmann distribution
pressure force per unit area
atmospheric pressure exerted due to gravity acting on air above Earth's surface
Boyle's Law the volume of a sample of gas at a constant temperature is inversely proportional to its pressure
Charle's Law the volume occupied by a sample of gas at constant pressure is directly proportional to the absolute temperature
Avogardro's Law equal volume of any two gasses at the same temperature and pressure contain the same number of moles; volume = moles at a constant temp and pressure
molar volume the volume occupied by one mole of gas at a particular temperature or pressure
Combined Gas Law combines all gas laws into one formula
Ideal Gas Law pressure, universal gas constant, volume, moles, temperature; PV=nRT; most gasses obey the ideal gas law; deviations occur at severe temp decreases and pressures increases
universal gas constant value of the universal gas constant depends on the units; volume and pressure
standard temperature and pressure (STP) P=1 atm; T=0C
molar volume for one mol of an ideal gas at STP
densities of gasses can be calculated from molar mass (M) and molar volume (V/n); depends on molar masses & temperature; density decreases as temp increases
gas mixtures in a mixture of gasses, each gas behaves independently of each other; exerts a pressure as if it were the only gas there; equals to the partial pressure of the gas combination
Dalton's Law of Partial Pressure the pressure exerted by a particular gas in a mixture is the partial pressure pf that gas; the sum of partial pressures = the total pressure; individual partial pressures obey the ideal gas law
mole fraction the fraction of the molecules of that component of the mixture
thermal pollution the decrease in solubility as temp increases due to factories or power plants; solubility increases as pressure increases; solubility decreases as temperature increases
Henry's Law the higher partial pressure of the gas above a liquid, the more soluable
diffusion the process by which molecules of one substance spread out through a medium to occupy a space uniformly; depend upon the speed at which the molecules are moving
effusion the process by which molecules of a gas flow through a small hole in a container; depends upon the speed at which the molecules are moving
Graham's Law under conditions of constant temp and pressure, the rates of diffusion and effusion of a gas are inversely proportional to the square root of its molecular weight; compares to different gasses at constant temp and pressure
real gasses as pressure increases, and/or temperature decreases; deviations from ideal gas behavior
Van Der Waals Equation resembles the ideal gas equation, but includes a pressure correction to account for the IMFs between molecules and a volume correction to account for the volume of individual molecules; a and b constants; constants are larger in molecules with larger IMFs
Created by: livabirch4
Popular Chemistry sets

 

 



Voices

Use these flashcards to help memorize information. Look at the large card and try to recall what is on the other side. Then click the card to flip it. If you knew the answer, click the green Know box. Otherwise, click the red Don't know box.

When you've placed seven or more cards in the Don't know box, click "retry" to try those cards again.

If you've accidentally put the card in the wrong box, just click on the card to take it out of the box.

You can also use your keyboard to move the cards as follows:

If you are logged in to your account, this website will remember which cards you know and don't know so that they are in the same box the next time you log in.

When you need a break, try one of the other activities listed below the flashcards like Matching, Snowman, or Hungry Bug. Although it may feel like you're playing a game, your brain is still making more connections with the information to help you out.

To see how well you know the information, try the Quiz or Test activity.

Pass complete!
"Know" box contains:
Time elapsed:
Retries:
restart all cards