Exam 3 Flashcards
(22 cards)
ΔG < 0
spontaneous
ΔG > 0
nonspontaneous
ΔG = 0
at equilibrium
Exothermic reactions
ΔG = (-)
ΔH = (-)
ΔS = (+)
Always spontaneous except at high temps
Endothermic
ΔG = (+)
ΔH = (+)
ΔS = (-)
Never spontaneous except at high temps
K < 1
more reactants at equilibrium
K > 1
more products at equilibrium
K = 1
Products = reactants at equilibrium
K < Q
more products than needed
shift left
K > Q
more reactants than needed
shift right
K = Q
system is at equilibrium
Relate Gibbs free energy and equilibrium
when ΔG = 0 the system is at equilibrium
Brongsten Lowry Acid
Compound donates proton to another proton
Brongsten lowry base
compound accept proton
Acids (Arrhenian)
dissolves to yield H30+ and donates H+
Bases (Arrhenian)
dissolves to yield OH- and accepts proton
Bases have
1 less H+ than conjugate acids
acids have
1 more H+ than conjugate base
Explain the relationship in an acid-base conjugate pair
When an acid donates H+, what remains is called the conjugate base of the acid because it reacts as a proton acceptor in the reverse reaction. Like, when a base accepts H+, it is converted to its conjugate acid.
Relate the Ph scale to acidity/basicity
the lower the pH, the more acidic it is and the higher the pH, the more basic it is
recognize & describe the conditions that lead to a solution acting as a buffer
- an acid to consume any OH- that is added
- a base to consume any H3O+ that is added
- the acid and base dont react with each other
demonstrate an understanding of the construction & operation of electrochemical cells
a device that makes electrical energy from chemical rxns. and can also work in reverse
