equilibrium Flashcards
dynamic
constant, active movement
static
without motion, fixed
constant
ultimately not changing visually
rate
typically a ratio in referrence to time
example of rate
speed- distance over time
properties of a system in chemical equilibrium
- closed system
- macroscope properties are constant
- equal rate of forward and reverse
dynamic equilibrium
dynamic- reactions still happening
equilibrium- rate of forward reaction is equal to rate of the reverse reaction
macroscopic properties
color
pressure
concentration
is dynamic equilibrium 50/50
not neccesarily
strong acid willing to give up
hydrogen
quantitative reactions
start out as reactants, go till completion, end up as products
-doesnt apply to all reactions
equilibrium constants
must consider reaction and product concentrations at the time equilibrium is reached
-experimental
Keq or Kc
product of molar concentrations of the product for the chemical reaction
rules of Kc
-concentrations always mol/L
-product concentrations are numerator
-reactant concentrations are placed in the denominator
-powers determinded by balanced equation
what types of states concentrations are included in Kc equations
-only gases and substances in solutions
Kc > 1
more inclined to create product
Kc < 1
reactant favoured
factors that affect equilibrium
- diff chemical reactions of different Kc
- temperature
Kc is ____ specific
temperature
factors that DO NOT affect equilibrium
- adding/removing the reactant or product (just reestablishes equilibrium)
- catalysts (reaches equilibrium faster)
- change in pressure (reestablishes)
using a graph to determine Kc what value do we use
equilibrium concentrations
la chateliers principal
if a stress is applied to a system at equilibrium then the system will chabnge to relieve that stress
energy (la chateliers principal)
energy is same as adding or removing chemical
endothermic energy addition
energy is a reactant
-adding energy pushes the reaction to product/right
