Equilibrium Test 1 Flashcards
when is a reaction at equilibrium?
when the concentrations or pressures of both the reactants and products don’t change; when the forward and reverse rate of reactions stop changing
what can/can’t be in equilibrium reactions?
solids and liquids are not exchanged between the forward and reverse reactions, so they are not included in our calculations
rate of reaction
= rate constant * [concentration of reactants]^moles
Kc constant
for concentrations,( [product1]^moles * [product2]^moles)/([reactant1]^moles…)
Kp constant
for gas pressures, [Pproduct]^moles/[Preactants]^moles
Kp vs Kc relation
Kp=Kc*(RT)^(moles product- moles reactants)
when K is much greater than one
the equilibrium is towards the right and products are favored
when K is much less than one
the equilibrium is towards the left and reactants are favored
K for forward/reverse reactions
is inverse (1/K)
if you combine multiple equilibrium reactions,
you multiply their Ks
if moles/enthalpy is mulitplied,
you raise the K to the multiplier power
concentration equilibrium graphs
the concentrations level out but the concentrations of products and reactants will not be equal
rate of reaction equilibrium graphs
the rate of reaction for both products and reactants will be equal at equilibrium
Qconstant
measures the same thing the K constant does, but for reactions that are not yet at equilibrium
if K>Q
the reaction is right favored and there are more products
