When we make calculations of the corrosion rates of Mg alloys, we often need to perform some simple conversions. The results are included in essentially any research paper in the field, while the logics of the development often remains obscured. For that reason I found useful to show the development here.
Faraday's law: m = (M / (nF))⋅it
since m = ρV, where ρ is the density and V is the volume of the corrosion layer and V = hA, where A is the area and h is the height (assuming pacing corrosion), h = m / (ρA)
=> h,cm / t,s = (M,g/mol / (nF)⋅A,cm2⋅ρ,g/cm3)⋅i,A
after the substitution of the corresponding values:
Rate,mm/y = (3.154⋅108s⋅24g/mol)/(2⋅11.1cm2⋅1.8 g/cm3⋅96500C/mol)⋅i(A)
Finally, Rate (mm/y)=1.981· 104·i(A)
This conversion is based on the Faraday's laws of Electrolysis and some basic conversions of units (centimeters to millimeters and seconds to years). The final formula was developed for the particular case when M = 24 g/mol, n = 2, ρ= 1.8 g/cm3 (Mg) and the area of a standard specimen A = 1.1 cm2. This values should, of course, be changed if necessary.
This only includes the conversion of units: days to years, centimeters to millimeters. The density is taken ρ= 1.8 g/cm3 (and should be adjusted if necessary) and the surface area is variable (A, cm2).
m(Mg) = n(mol) ·24 g/mol
n(Mg)=n(H2) = pV / RT = (1.013⋅105Pa⋅10-6⋅V(H2)mL)/(8.314J/mol−K⋅298K) = 4.09⋅10−5⋅VmL
m(Mg), g = 9.8· 10-4 V(H2), mL
PH = (2.03⋅103⋅9.8⋅104⋅V(H2),mL) / (A,cm2⋅t,days)
PH,mm/y = (1.99⋅V(H2),mL) / (A,cm2⋅t,days)
A bit more assumptions have been made here. First, the gas is assumed to be hydrogen formed in the simplified reaction: