REDOX REACTIONS AND ELECTROCHEMISTRY

1. E_cell = E^o_cell - log
   [Products][Reactant]
   
   - Δ G = nFE_cell ; - Δ G^o = nFE^o_cell
   E^o_cell = 
   2.303 RTn F
    log K_eq = 
   0.591n
    log K_eq [at 25⁰C]
   Δ G^o = - 2.303 RT logK
2. Gibb's Helmholtz Equation
   
3. Faraday's First Law
   w = Z i t , 1 faraday is the quantity of charge carried by 1 mole of electrons.
   Z = 
   equivalent mass96500
    ; Z = weight deposited when 1A passed for 1 sec.
4. Faraday's second Law
   
   m₁m₂
    = 
   E₁E₂
   
   m₁ , m₂ are masses deposited and E₁ and E₂ are their equivalent weights ; for same amount of passed charge .
   %current efficieny = 
   Actual CurrentAmmeter current
    x 100
   Ohm's Law = I = E/R
   Ions are always discharged / produced in equivalent amounts whatever their speeds of deposition are ,
   Specific conductance = κ = 1 / ρ , ρ = specific resistance
   ρ = 
   la
    x C      
   la
    = constant , C = conductance = 
   1R
   
   Conductivity = cell constant x observed conductance
   π_eq = 
   kC_eq
    = 
   K x 1000 cm³ L^-1Normality
5. Equivalent conductance , (Λ)
   Λ = κ x V
   V = volume in mL containing 1g equivalent of the electrolyte.
   Molar conductance (μ) = [Equivalent conductance]
   (μ) = nΛ
   n = 
   Molecular MassEquivalent Mass
   
   μ = κ x V      V(mL) containing 1g mole of an electrolyte.
   At infinite dilution , Λ_o = λ_a + λ_c
   λ_c = ku_c
   λ_a = ku_a
   λ_a and λ_c , ionic conductance of anion and cation
   k = 96500C
   u_a = mobility of anion
   u_a = mobility of cations
   degree of dissociation = Λ / Λ_∞
   α = ( K / C)^1/2 = 
   λ_e^Cλ_e^∞
    = 
   λ_m^Cλ_μ^∞
   
   λ_e^C , λ_m^C = equivalent and molar conductance
6. Ostwald's Equation
   K = 
   C( λ_m^C )²λ_m^∞ (λ_m^∞ - λ_m^C)
7. Cell Notation
   
   Transport Number
   Transport Number = 
   Current carried by ionToatl current carried
   
   n_c + n_a = 1