Important equations Flashcards
Molar concentration=
moles/volume (dm^3)
Moles=
mass/molar mass
Energy=
Plank’s constant x frequency
Percentage yield=
(actual yield/theoretical yield) x 100
Mass concentration=
mass (g)/volume (dm^3)
Rate of reaction for an Sn1 reaction=
k[haloalkane]
Rate of reaction for an Sn2 reaction=
k[haloalkane][nucleophile]
Specific rotation=
(Observed rotation (degrees))/(length (dm) x concentration (g/ml))
ΔU =
U(products) – U(reactants)
Rate of reaction for an E1 reaction=
k[haloalkane]
Rate of reaction for an E2 reaction=
k[haloalkane][base]
pH=
-log([H3O+])
pOH=
-log([OH-])
pH + pOH=
pKw = 14.00 (at 25°C)
pV=
pressure (Pa) x volume (m^3) =
nRT
moles x gas constant (8.314) x temperature (K)
Ka=
([H3O+][A-])/[HA]
Acid dissociation constant
pKa=
-log(Ka)
Kb=
([HB+][OH-])/B
Base dissociation constant
pKb=
-log(Kb)
Kc=
(([C]^c)([D]^d])/(([A]^a)([B]^b))
Equilibrium constant
What is Kp?
The equilibrium constant expressed in terms of partial pressures
Kw=
[H+][OH-]
At 25 °C and zero ionic strength, Kw is equal to 1.0×10−14
pKw=
-log(Kw)
