Formulas Used in Chemistry
Part of the Atom Mass Charge
Electrons 9.1956 x 10 ^-31 Kg -1
Protons 1.67262 x 10 ^-27 Kg +1
Neutrons 1.67493 x 10 ^-27 Kg neutral
Number of Moles
n= m
MW
n=# of moles
m= mass in grams
MW= molecular weight in moles per gram
Avogadro's Constant= 6.02 x 10^23
Equilibrium
k= [OH-][H+]
k= the equilibrium constant = 1.0 x 10 -14
= KaKb
pH= pKa + log [OH- (base)] / [H+ (acid)]
Thermodynamics/ Kinetic Energy
Gibb's Free Energy
ΔG= ΔH - TΔS
ΔG= Gibb's Free Energy
ΔH= Heat capacity or enthalpy
ΔS= Entropy= disorder
ΔG= ΔH - TΔS
= -RT ln K R= Gas Constant= 8.314 J/mol•K
= -nF E°
F= Faraday's constant= 9.65 x 10 ^-1 C/moles of electrons
ln [A]1= -kt ( 1/[A]1 - 1/[A]0])
[A]0
ln k= -E/R (1/T) + ln A
ln P= -ΔH/RT + C
ln P2 = -ΔH/R (1/T2 - 1/T1)
P1
Heat
q= mcΔT
q= heat
m= mass in grams
c= speed of light= 3.00 x 10 ^8 m/s2
ΔT= temperature in Kelvin
Specific Heat Capacity
Cp= ΔH / ΔT
Cp = specific heat capacity
ΔH= total heat/enthalpy
ΔT = temperature in Kelvin
Ideal Gas Law
PV= nRT
P= Pressure in atm (1 atm= 760 torr= 760mm Hg)
V= Volume in litres (L)
n= # of moles
R= 8.314 Js
T= temperature in Kelvin (K= C + 273)
Electro-chemistry
E°cell = E - RT ln Q
nF
= E - 0.0592 ln Q
n
E°= kinetic energy of the cell
R= 8.314 Js
T= temperature in Kelvin
Q= equilibrium constant
Atomic Structure
En= -2.178 x 10 ^-18 J
n
λ= h
m ѵ
λ= wavelength
h= Plank's Constant= 6.63 x 10 ^-34 J•s
m= mass
ѵ = frequency
Part of the Atom Mass Charge
Electrons 9.1956 x 10 ^-31 Kg -1
Protons 1.67262 x 10 ^-27 Kg +1
Neutrons 1.67493 x 10 ^-27 Kg neutral
Number of Moles
n= m
MW
n=# of moles
m= mass in grams
MW= molecular weight in moles per gram
Avogadro's Constant= 6.02 x 10^23
Equilibrium
k= [OH-][H+]
k= the equilibrium constant = 1.0 x 10 -14
= KaKb
pH= pKa + log [OH- (base)] / [H+ (acid)]
Thermodynamics/ Kinetic Energy
Gibb's Free Energy
ΔG= ΔH - TΔS
ΔG= Gibb's Free Energy
ΔH= Heat capacity or enthalpy
ΔS= Entropy= disorder
ΔG= ΔH - TΔS
= -RT ln K R= Gas Constant= 8.314 J/mol•K
= -nF E°
F= Faraday's constant= 9.65 x 10 ^-1 C/moles of electrons
ln [A]1= -kt ( 1/[A]1 - 1/[A]0])
[A]0
ln k= -E/R (1/T) + ln A
ln P= -ΔH/RT + C
ln P2 = -ΔH/R (1/T2 - 1/T1)
P1
Heat
q= mcΔT
q= heat
m= mass in grams
c= speed of light= 3.00 x 10 ^8 m/s2
ΔT= temperature in Kelvin
Specific Heat Capacity
Cp= ΔH / ΔT
Cp = specific heat capacity
ΔH= total heat/enthalpy
ΔT = temperature in Kelvin
Ideal Gas Law
PV= nRT
P= Pressure in atm (1 atm= 760 torr= 760mm Hg)
V= Volume in litres (L)
n= # of moles
R= 8.314 Js
T= temperature in Kelvin (K= C + 273)
Electro-chemistry
E°cell = E - RT ln Q
nF
= E - 0.0592 ln Q
n
E°= kinetic energy of the cell
R= 8.314 Js
T= temperature in Kelvin
Q= equilibrium constant
Atomic Structure
En= -2.178 x 10 ^-18 J
n
λ= h
m ѵ
λ= wavelength
h= Plank's Constant= 6.63 x 10 ^-34 J•s
m= mass
ѵ = frequency