Equilibrium Flashcards
Kc =
[products]^mol / [reactants]^mol
Kc value is constant. Only dependent on
Temperature
Kc units
Kc = [mol dm-3]^∆n
Kp = (in terms of Kc Kx and Kn)
Kp = Kc (RT)^∆n
Kp = Kx (RT/V)^∆n
Kp = Kn (P/N)^∆n
If ∆n = 0 then
Kp = Kc
Kp = Kx
Kp = Kn
If n prod > n reactant (pos) then
Kp > Kc
Kp > Kx
Kp > Kn
When n prod < n reactant
Kp < Kc
Kp < Kx
Kp < Kn
If Kc large it means
If Kc small it means
Large Kc means more products (forward reaction favored)
Small Kc means more reactants (forward reaction not favored)
If Kc > Qc then
Forward reaction
Qc =
Qc = Pc / Rc
(Quotient = Product / Reactant)
Pressure effect
Inc in pressure means equilibrium shifts to side with less moles
Ice <—> Liquid when pressure increases
Ice to liquid (forward) preferred
Ice has more volume and liquid has less volume
Ef > Er =
Ef < Er =
Ef > Er = endo
Ef < Er = exo (Rexo)
Ksp =
[cation] [anion]
Ksp is proportional to
Temperature and solubility
General formula for Ksp
[cation^+y]^x [anion^-x]^y
Saturated salt
Ionic Prod = Ksp (no ppt)
Unsaturated salt
Ionic Character < Ksp (no ppt)
Super saturated salt
Ionic character > Ksp (ppt present)
(ppt when ionic prod more)
Zinc displaces copper from its solution because
Zinc has a smaller reduction potential than copper
Temp needed for ammonia production (Haber process)
400º - 450ºC
Haber process
N2 + 3H2 —> 2NH3
400º - 450º heat
150-200 atm pressure
Iron catalyst
∆H = 92 kJ/mol
Exothermic
pH = pKa + ?
pH = pKa + log [salt]/[acid]
pH > pKa means
[salt] > [acid]
pH = pKa + 1
pH < pKa means
[salt] < [acid]
pH = pKa - 1
