factors affecting equilibrium Flashcards
what happens if you increase the concentration of reactants? why?
- equilibrium shifts to the right
- favouring the forwards reaction
- in order to decrease the concentration of this added reactant
what happens if you increase the concentration of products? why?
- equilibrium shifts to the left
- favouring the backwards reaction
- in order to decrease the concentration of this added product
which direction is endothermic?
backwards - breaking bonds
which direction is exothermic?
forwards - making bonds
when will pressure change affect equilibrium?
if there are more gaseous molecules on one side of the equation
if pressure increases, which direction will equilibrium shift in?
the side with fewer molecules
what effect do catalysts have on equilibrium?
increases the rate at which equilibrium is established
if pressure decreases, which direction will equilibrium shift in?
the side with more molecules
what happens to equilibrium position if you increase the temperature of a reaction?
shifts in endothermic direction
what happens to equilibrium position if you decrease the temperature of a reaction?
shifts in exothermic direction
how do you know if a reaction is exo / endothermic?
- delta H = exothermic
+ delta H = endothermic
what conditions will give the maximum yield in an exothermic reaction where there are less moles on the products side?
low temperature = equilibrium shifts in exothermic direction towards products
high pressure = equilibrium shifts towards fewer gas molecules towards products
what is the disadvantage of using a high pressure?
- expensive (requires a lot of energy)
how is high pressure and high temperature a compromise for an exothermic reaction with more moles on the products side?
high temp = increases rate of reaction but reduces potential yield
high pressure = increases rate of reaction and also increases yield
- product can form quickly
- compromise between rate and yield
