Chemical Equilibria Flashcards
Main concept of Equilibrium
rates of the FORWARD and REVERSE REACTIONS are equal
Can equilibriuim be reached from either direction?
yes
Forward vs Reverse Reaction
F: Reactants produce more products
R: Products produce more reactants
Symbol for IRREVERSIBLE REACTIONS
2 arrows that are double headed
FORMULAS:
a A + b B -> <- c C + d D
- Kc expression
- Kp expression
- Kp formula using Kc
Kc = ( [C]^c [D]^d ) / ( [A]^a [B]^b )
Kp = ( PC^c PD^d) / ( PA^a PB^b )
Kp = Kc (RT)^(Δn gas)
wherein R = 0.0821 (L-atm)/(mol-K)
and Δn gas = moles of gas in products - moles of gas in reactants
When will Kc = Kp
If Δn gas = 0
Where do you look for the MOLES in a concetrantion
Coefficient
MEANING:
K eq > 1
K eq < 1
K eq = 1
Forward
Reverse
Equilibrium
What do not appear in the K eq expression
solids and liquids
What kind of K eq does (aq) appear in?
Kc or Ksp
*not Kp = only for gases
Homogenous vs Heterogenous Equilibrium
Homo = all reacting species are in the same phase
Hetero = reactants and products are in different phases
What does “Reacting Species” denote?
Both reactants and Products
What is the MOST important rule before writing and Keq Value + using Le Chatelier’s Principle?
BALANCE the equation
What is the….
- K eq of the reverse reaction
- K eq of the new reaction when original is multiplied by n
- 1/K eq of original
- (K original)^n
Reaction Quotient Definition
Ratio that helps determine the direction a rxn must shift to reach equilibrium
denoted by Q
