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.
Didn't know it?
click below
Knew it?
click below
Don't know
Remaining cards (0)
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

CHEM 126 Chapter 6

CHEM 126 Final

heat energy transferred between system & surroundings due to difference in temp (thermal) - thermal energy of molecule motion - Q
work - energy transferred when object is moved by force - W
relationship between change in energy, heat, work - ∆E = q + w
- Q > 0 - E increases
heat FROM system TO surroundings - q < 0 - E decreases
work done ON system BY surroundings - w > 0 - E increases
work done BY system ON surroundings - w < 0 - E decreases
E increases when.. - Q > 0 - W > 0
E decreases when... - Q < 0 - W < 0
P-V work - W = -P * ∆V - use when rxn occurs that changes V of system - undergoes V change by pushing against surroundings -> do work
units of energy - E = (1/2)M*V^2 * mass = kg & volume = m/s - 1 joule = 1 kg*m^2/s^2 - 1 caolire = 4.184 J
state function - values depeond only on the state that the system is in, not path it took to get there - EX: altitude, energy, enthalpy, pressure, volume, temp
change of enthalpy in terms of change of internal energy/heat ∆E = q - P∆V - at constant P (qp) = ∆E + P∆V ***** ∆H = ∆E + P∆V = qp (P∆V is usually 0)
endothermic vs. exothermic ∆H > 0: endothermic - absorb heat ∆H < 0: exothermic - release heat
specific heat capacity - amount of heat required to change the temp of 1 gram of a material by 1 degree Kalvin - Q = C * M * ∆T - C = J/(g*K), M = grams, T = Kelvin, Q = Joules
constant pressure - coffee cup calorimeter - qp = ∆H
constant volume - bomb calorimeter - qv = ∆E (used for combustion)
constant pressure calometry equation -T final water = T final solid - q H20 = - q solid - C H20 * M H20 * ∆T H20 = -(C solid * M solid * ∆T solid)
Hess's law - ∆H rxn = sum of the enthalpy changes for the individual steps ** make sure excess elements cross off, moles match up, reverse sign if rxn needs to be reveresed
stand heats of rxn & standard heats of formation - ∆H rxn° = ∆H rxn under standard conditions - ∆H f° = enthalpy change for the formation of 1 mol of substance from its elements in their standard state
hess's law + heat of formation ∑(number of mols * heat of rxn(products)) - ∑(number of mols*heat of reaction(reactants))
Created by: ccottrel



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:
restart all cards