Chemistry Flashcards
Formal Charge
VE - ½ BE - LPE
VE - valence electrons
BE - bonding electrons (in pairs)
LPE - lone pair electrons
Percent yield
actual mass of desired product/
theoretical mass of desired product
x 100%
Kelvin Temperature
K = C + 273.15
Heat
Q = mcΔT
Q - heat
m - mass
c - specific heat
ΔT - change in temperature
Enthalpy of the reaction
ΔH rxn = ΔHbonds broken - ΔHbonds formed
Gibbs Free Energy
ΔG = ΔH - TΔS
ΔG - change in Gibbs free energy
ΔH - change in enthalpy
T - temperature
ΔS - change in entropy
Gibbs Free energy of a reaction
ΔGo rxn = ΔGo products - ΔGo reactants
Gibbs free energy of reaction - ideal gas
ΔG rxn = ΔGo rxn + RTlnQ
ΔG rxn - Gibbs free energy of the reaction
ΔG° rxn - Gibbs free energy of the reaction under
standard conditions
R - ideal gas constant
T - temperature
Q - Reaction quotient
Gibbs Free energy of a reaction at equilibrium
ΔGo rxn = -RTlnKeq
ΔG° rxn - Gibbs free energy of the reaction under
standard conditions
R - ideal gas constant
T - temperature
Keq - equilibrium constant
van der Waals equation
(P + an^2/V^2 )(V - nb) = nRT
P - pressure
V - Volume
n - moles of gas
R - ideal gas constant
T - Temperature
a - the attractive forces factor
b - the volume factor
Daltons Law of partial pressure
Pgas = Xgas (Ptotal)
Boyles Law
Pressure/Volume = constant
Charles Law
Volume/Temp
Gay-Lussac’s Law
Pressure/Temp = constant
Molality
m = moles of solute/ kilograms of solvent = mol/kg
Molarity
M = moles of solute/liters of solution = mol/L
Raoults Law
vapor pressure of solution = mole fraction of solvent/vapor pressure of pure solvent
Boiling point elevation
ΔTb = iKbm
ΔTb - magnitude of boiling point elevation
i - van ‘t Hoff factor
Kb - boiling point elevation constant
m - molality
Freezing point depression
ΔTf = iKfm
ΔTf - magnitude of freezing point depression
i - van ‘t Hoff factor
Kf - freezing point depression constant
m - molality
Osmotic pressure
Π = iMRT
Π - osmotic pressure
i - van ‘t Hoff factor
M - molarity
R - ideal gas constant
T - temperature
Reaction rate
rate = k[A]^x[B]^y
rate - reaction rate
k - rate constant
[A] and [B] - concentration of reactants
x and y - order of reaction with respect to each
reactant
pH
-log[H3O+]
Henderson-Hasselbalch equation
pH = pKa + log [A-]/
[HA]
pH - pH of the solution
pKa - pKa
of acid
[HA] - concentration of acid
[A-] - concentration of conjugate base
