Chem 223 Midterm 1 Flashcards
key idea about equilibrium
RATIO
what is k
equilibrium constant
what is the k equation
k = prod/reac
what is q
reaction quotient
when does q=k
at equilibrium
when do we use q and when do we use k
k at equilibrium, q when not at equilibrium
Q<K
shifts to form products, progresses to the right
Q>K
shifts to form reactants, progresses to the left
reference state
implied, standard state
what are the states we don’t care about
liquid and solid
if solid or liquid states are in a reaction, what do we plug into the k equation in their place
1 ([CO2]/1)
what happens to the size of Q with an increase in product
larger Q
what happens to the size of Q was an increase in reactant
smaller Q
5% rule
for assumption to be valid, x must be <5% of the number
summary of LeChatlier’s principle
when a chemical system at equilibrium is disturbed, either the products or reactants side will shift their values to account for the change and get back to equilibrium
how does the reaction shift if addition is added to the reactants
shift to the right
how does the reaction shift if addition is added to the products
shift to the left
how does the reaction shift if reactant side is subtracted
shift to the left
how does the reaction shift if the product side is subtracted
shift to the right
pressure eqaution
force/area
exothermic reaction and shift
releases heat, increasing the temperature shifts equilibrium to the left; decreasing the temperature shifts equilibrium to the right
endothermic reaction and shift
absorbs heat, increasing the temperature shifts equilibrium to the right; decreasing the temperature shifts equilibrium to the left
three different acid base definitions
Arrhenius, Bronstead-Lowry (not dependent on water), Lewis
Arrhenius acid definition
contains H+ and generates H+ in water
