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.

Remove ads
Don't know
Know
remaining cards
Save
0:01
To flip the current card, click it or press the Spacebar key.  To move the current card to one of the three colored boxes, click on the box.  You may also press the UP ARROW key to move the card to the "Know" box, the DOWN ARROW key to move the card to the "Don't know" box, or the RIGHT ARROW key to move the card to the Remaining box.  You may also click on the card displayed in any of the three boxes to bring that card back to the center.

Pass complete!

"Know" box contains:
Time elapsed:
Retries:
restart all cards




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

Graham's Law

cava s2d12 303 1.13 Graham's law of effusion

QuestionAnswer
[...]: movement of gas molecules from areas of high concentration to areas of low concentration diffusion: movement of gas molecules from areas of high concentration to areas of low concentration
[...]: movement of gases through a tiny pore or opening effusion: movement of gases through a tiny pore or opening
HS Chemistry courses love the word effusion, but it really just means diffusing [...]. HS Chemistry courses love the word effusion, but it really just means diffusing out of an opening.
Graham's law of effusion: The rate of effusion is [-ly] proportional to the square root of the molar mass of the gas particles. Graham's law of effusion: The rate of effusion is inversely proportional to the square root of the molar mass of the gas particles.
Graham's law math: [...] Graham's law math: Rate gas1 / Rate gas2 = Sqrt{ mass gas 2 } / sqrt{ mass gas1 }
Notice that in Graham's law, gas 1 is on top on the left, but on [...] on the right. Notice that in Graham's law, gas 1 is on top on the left, but on bottom on the right.
Although Graham's law describes *effusion* rates, it can also be used to describe *[...] rates* and sometimes test-writers throw *[...] rate* questions at you and expect you to know that Graham's law relates to both. Although Graham's law describes *effusion* rates, it can also be used to describe *diffusion rates* and sometimes test-writers throw *diffusion rate* questions at you and expect you to know that Graham's law relates to both.
Graham's law is used for BOTH effusion and [...] rate problems, even though his law is called Graham's law of *effusion*. Graham's law is used for BOTH effusion and diffusion rate problems, even though his law is called Graham's law of *effusion*.
Graham's law of effusion: The rate of effusion is inversely proportional to the [...] of the molar mass of the gas particles. Graham's law of effusion: The rate of effusion is inversely proportional to the square root of the molar mass of the gas particles.
Graham's law of effusion: The rate of effusion is inversely proportional to the square root of the [...] of the gas particles. Graham's law of effusion: The rate of effusion is inversely proportional to the square root of the molar mass of the gas particles.
Created by: mr.shapard