• 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

Card Range To Study



Play button


Play button




Click to flip

Use LEFT and RIGHT arrow keys to navigate between flashcards;

Use UP and DOWN arrow keys to flip the card;

H to show hint;

A reads text to speech;

14 Cards in this Set

  • Front
  • Back
Dynamic Equilibrium

- involved with reversible reactions which contain forward and reverse reactions

- forward and reverse reactions are going at the same rate


- measure of distribution of energy throughout a system or between a system and its environment

Law of mass action

- if the systm is at a constant temp, the following ratio is constant

Keq = [C]^c[D]^d/[A]^a[B]^b

Equilibrium Constant

- For the F and R rxn of 2A--> B+C

- Kc = Keq = [B][C]/[A]^2

Reaction Quotient

- how to measure the concentrations of all the reactants and products

- concentrations of the products and reactants are not constant

Relationships btwn Q and Keq

- Q< Keq --> forward rxn has not yet reached equilibrium, greater concen of reactants

- Q = Keq, rxn is in dynamic equilibrium

-Q> Keq --> forward rxn has exceeded equilibrium, greater concen of products

Properties of the law of mass action

- concentrations of pure solids and liquids do not appear in equil. constant eqns

-Keq = temperature dependent

- Larger the Keq = equilibrium is further to the right

- equil constant for forward rxn = Keq, reverse rxn = 1/Keq

Le Chatliers Principle

- if stress is applied to a system, the system shifts to relieve that applied stress
Ideal Gas Law

-if the pressure increases, it will respond by decrease the amount of moles, therefore decreasing the pressure back to equilibrium
Volume and Pressure

- volume increases, pressure decreases

- system will react by increasing the number of gas moles to restore pressure

Changes in temperature (Le Chatliers principle)

endothermic: heat = reactant (H>0)

exothermic: heat = product (H<0)

Kinetic Product

-formed at lower temperatures with smaller heat transfer

- "fast" products: require a lower free energy to form

Thermodynamic product

- higher temperature with a larger heat transfer

- free energy of the product is lower therefore more stable