Save
Busy. Please wait.
or

show password
Forgot Password?

Don't have an account?  Sign up 
or

Username is available taken
show password

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.
We do not share your email address with others. It is only used to allow you to reset your password. For details read 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
share
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

Gas Laws

gas laws and stoichiometry

TermDefinition
Kinetic Molecular Theory pt. 1 Gas molecules do not attract or repel each other
Kinetic Molecular Theory pt. 2 Gas particles are much smaller than the spaces between them
Kinetic Molecular Theory pt. 3 Gas particles are in constant, random motion
Kinetic Molecular Theory pt. 4 No kinetic energy is lost when gas particles collide with each other or with the walls of their container
Kinetic Molecular Theory pt. 5 All gases have the same kinetic energy at a given temperature
Rate of effusion depends on the mass of the particles
In diffusion, lighter particles diffuse... more rapidly than heavier particles
Graham's Law of Effusion Rate A / Rate B = sqrt(Rate B / Rate A) *compound A has the smallest molar mass
Pressure formula P= force / area
A barometer is used the measure atmospheric pressure
Units of standard pressure 101.3 kPa 1 atm 760 mmHg
Dalton's Law of Partial Pressure The total pressure of a mixture of gases is equal to the sum of the pressures of all the gases in the mixture. Ptotal = Px + Py + Pz
Pressure is measured in these 3 units: mmHg, kPa, atm
Temperature is measure in Kelvin (conversion from Celsius = C + 273)
Volume is measured in Liters
Number of particles is solved by completing gas stoichiometry
Boyle's Law P1V1 = P2V2 inverse relationship
Charles' Law V1 / T1 = V2 / T2 direct
Gay-Lussac's Law P1 / T1 = P2 /V2 direct
Combined Gas Law P1V1 / T1 = P2V2 / T2 direct
Ideal Gas Law PV = nRT p = pressure, v = volume, n = number of moles, R = given constant, T = temperature
How many variations to the Ideal Gas Law? 3
Variables M = Molar mass m = mass D = density (g/L)
Variations M = mRT / PV M = DRT / P D = MP / RT
If GRAMS are given, start with: stoichiometry
If LITERS are given, start with: PV = nRT (or if @ STP, you may use the 22.4/mol conversion)
Created by: mma129
 

 



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