BLOCK 5 Chemical Equilibrium Flashcards
equilibrium constant calculations
[products]/[reactants]
equilibrium constant calculations units
[mol/dm^3]
define dynamic equilibrium
forward reaction = reverse reaction (in a closed system)
define Le Chatelier’s Principle
if a reaction is at equilibrium and subjected to a change in: temp, pressure, conc,
position of equilibrium will shift to minimize that change
Haber process conditions:
temp = 400 celsius
pressure = 200atm
catalyst = iron
Effect of position of equilibrium:
Decrease temp
(to minimize change,) equilibrium shifts to favour exothermic reaction
yield: up
rate: down
Effect of position of equilibrium:
Increase temp
(to minimize change,) equilibrium shifts to favour endothermic reaction
yield: down
rate: up
Effect of position of equilibrium:
decrease pressure
(to minimize change,) equilibrium shifts to side with most gaseous moles
yield: down
Effect of position of equilibrium:
increase pressure
(to minimize change,) equilibrium shifts to side with lease gaseous moles
yield: up
why not increase pressure if it increases yield?
expensive
Effect of position of equilibrium:
remove catalyst
no effect. however system will take longer to get to equilibrium without a catalyst
endothermic =
ΔH
exothermic =
-ΔH
