Busy. Please wait.

show password
Forgot Password?

Don't have an account?  Sign up 

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.
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.
Don't know
remaining cards
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:
restart all cards
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

inorganic chem DAT

DAT flashcards

1 atm = ? 760 mm Hg = 760 torr
standard temp. and pressure 273.15 K and 1 atm (used with problems involving pressure)
standard conditions 0 C, 298 K (used in problems involving enthalpy, entropy, gibbs free energy)
Boyle's gas Law PV = k; P1V1= P2V2 at const. temp., the volume of gas is inversely proportional to its temp.
Law of Charles and Gay-Lussac V/T = k; V1/T1 = V2/T2 at const. pressure, volume of a gas is directly proportional to its absolute temp.
K --> Celsius conversion T(K) = T(C) + 273.15
Avogadro's Principle at const. temp. and pressure, the volume of the gas will be directly proportional to the number of moles of gas present n/V = K; n1/V1 = n2/V2
Ideal Gas Law PV = nRT
Gas constant R = ? 8.21 x 10^-2 (L*atm)/mol*K)
volume of 1 mol of gas at STP 22.4 L
determining partial pressure of a gas Pa = Pt Xa where Xa = n(a)/n(t) (moles of A/total moles)
Assumptions of the Kinetic Molecular Theory gas particles... 1. vol.'s are negligible 2. exhibit no intermolecular interactions 3. are in continuous, random motion, undergoing collisions with other particles and container walls 4. collisions are elastic 5. KE proportional to temp.
fusion transition from solid to liquid
alpha particle helium nucleus
beta decay beta particle = e conversion of neutron to proton Z increases by 1 in daughter cell Z decreases by 1 in positron decay
Created by: bestein