what is a dynamic equilibrium
in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction and the concentrations of reactants and products do not change
how do you write the Kc equation aA + bB —> cC +dD
[C]^c x [D]^d/ [A]^a x [B]^b
if Kc has no units what can you use
equilibrium moles
for Kc if given data in moles and a total volume what do you have to do
convert moles to conc
moles/volume
how do you work out partial pressure
mole fraction x total pressure of gas mixture
how do you work out mole fraction
moles of gas A / total moles of gas
what does increasing the conc of a reactant do to kc
same principle for inverse and conc of products
kc doesnt change
- equilibrium no longer
- for the value of kc to be restored the conc of products must increase and reactants decrease
- position of eq shifts to right until orginal Kc value restored
explanation for increasing the pressure when the products have the least moles of gas
same principle for decreasing pressure for products and reactants and increasing pressure of reactants
- for value of kp to be restored partial pressure of products must increase so eq shifts to the right until kp restored
if the reaction is exothermic then what does increasing the temp do to kc and kp
decreases
if reaction is exothermic then what does decreasing the temperature do
increases kp kc
if the reaction is endothermic what does increasing the temp do t kp and kc
increases
if the reaction is endo thermic what does decreasing the temp do to kp and kc
decreases
how do you work out partial pressure
mole fraction x total pressure
kp equation for aA +bB —–> cC + dD
pC^c x pD^d / pA^a x pB^b
what does it mean when k is greater than 1
reaction favours the products
what does it mean when k is lesser then 1
reaction favours reactants
