chemical equilibrium Flashcards
forward reaction
initial reactants are used up quickly but slow down as the concentration drops
backward reaction
initially reactants are reformed slowly but speed up as the concentration of products increases
le chatiliers principle
if a reaction is at equilibrium is subjected to a change in pressure or temperature or conc
portion of equilibrium will move to counteract the change
eq shift left
make more reactants
eq shift right
make more products
change of concentration
3h2 + n2 → 2nh3
increased concentration of reactant or product
Equilibrium shifts to reduce the concentration
3h2 + n2 → 2nh3
increase in h3 conc equilibrium will shift right to use it up and reduce the concentration and more nh3 is produced
increase in the nh3 concentration equilibrium shifts left to use it up and reduce the concentration so more h2 and n2 produced
changing temperature
3h2 + n2 → 2nh3
3h2 + n2 → 2nh3
increase temperature equilibrium will shift to reduce the temp in the endothermic direction so more n2 or h2 produced
decrease in temp equilibrium shifts in exothermic direction increasing the temp and more nh3 produced
catalysts
no effect on equilibrium
speeds up forward and backward reaction equally so no effect on yield
making ethanol
c2h4 + h2o→ c2h5oh
pressure 60
temp 300
phosphoric acid catalyst
forward reaction is exothermic so decreases temp equilibrium shifts right producing more ethanol
low temp
lower rate of a reaction
300 is a compromise between yield and rate
pressure
high pressure means equilibrium shifts right producing more ethanol
less moles of gas on right so equilibrium shits right to reduce pressure
high pressure increases rate
hp environment expensive due to thick and robust vessels and pipes needed
compromise between yield speed and cost
temp effect on KC
only valid for one temp
change in temp = change in equilibrium concentration so kc changes too
if temp change causes equilibrium to shift right ks increases
if temp change causes equilibrium to shift left kc decreases