Study your flashcards anywhere!

Download the official Cram app for free >

  • Shuffle
    Toggle On
    Toggle Off
  • Alphabetize
    Toggle On
    Toggle Off
  • Front First
    Toggle On
    Toggle Off
  • Both Sides
    Toggle On
    Toggle Off
  • Read
    Toggle On
    Toggle Off
Reading...
Front

How to study your flashcards.

Right/Left arrow keys: Navigate between flashcards.right arrow keyleft arrow key

Up/Down arrow keys: Flip the card between the front and back.down keyup key

H key: Show hint (3rd side).h key

A key: Read text to speech.a key

image

Play button

image

Play button

image

Progress

1/27

Click to flip

27 Cards in this Set

  • Front
  • Back
1st law of Thermodynamics
Energy of the universe is constant;
Energy can never be created or destroyed
2nd law of Thermodynamics
System spontaneously move toward disorder(high entropy)
ΔE:?
ΔE= q + E
w= -pΔV
+w = V is -
-w = V is +
Locked piston
ΔE = q
Unlocked piston: When heat piston
Volume increases
Work is -
PE increases so ΔE decreases
" Expanding gases cool"
Unlocked piston: Put weight on piston
Work is +
Temp increases
"compressed gases warm"
Isobaric
Pressure constant
area= work done by gas
Isochoric
Volume constant
Area= 0 so work= 0
Isothermal
Temp constant
ΔE=0 so q=-w
Adiabatic
no heat transfer
q=0 ΔE=w
"perfectly insulated system"
Entropy
Amount of disorder
Increasing entropy means:
1) Phase change
2) Increasing # of moles of gas dissolved; the side with the more mol of gas has more entropy
Enthalpy
amount of heat gained or lost when bonds are formed or broken
Bond breaking
requires energy
Bond forming
releases energy
(-)ΔH
exothermic
heat is product
product have stronger bond that the reactant
(+)ΔH
endothermic
heat is reactant
reactant have stronger bonds
Hf=0 when?
when elements are in their natural state
ΔG
Gibbs free energy
Energy evolved or absorbed as the rxn goes from rxn to product
(-)ΔG
product have less energy
more stable
spontaneous
exergonic(energy is given off)
(+)ΔG
Product have more energy
less stable
nonspontaneous
endergonic
ΔG=0
prod and reac have same energy
rxn is @ equilibrium
Low temperature
ΔH dominated
if ΔH and ΔS are both (-):spon
High temperature
ΔS dominates
Kinetics
rates, activation Energy, catalyst, temp
Thermodynamics
ΔG, H, S, Equilibrium, Temperature