Dear Golizadeh ,

For the accurate determination of the current efficiency during alloy deposition, first you must to determine the mass of the alloy, and composition (EDS, X-ray.) Than from the Faraday law to determine the theoretical mass at given current:

mt = ItMa/(naF)

but where Ma is a molecular weight of alloy given as

sum(Mm*X) where Mm is a molecular weight of single metal in alloy and X is a ratio of metal in alloy. na is the average number of exchanged electrons for alloy, sum(nm*X), where nm is the number of electron for one metal in alloy.

For example for FeCr (from bath containing Fe2+ and Cr3+) with composition 0.3 Fe and 0.7 Cr

Ma = 55.8*0.3 + 52*0.7 = 53.14 g/mol

na = 2*0.3 + 3*0.7 = 2.7 electrons

(Ma/na) is usually called equivalent weight

Dividing experimental mass with theoretical and multiply with 100, you will get current efficiency.

Hello Tahere Golizadeh,

Research Article related to current efficiency of electrodeposited alloy coating be determined.

I hope the information will help you.

With Best Wishes,

Samir G. Pandya

You have to first define your alloy ionic state, for example AB3+ in solution. So for a cathode oxidation, you have 3e- converting to solid AB.

In this example you will mass a sample, plate it with a given amp*s or amp*min and mass the post-plated sample.

Use Faraday's principle to make the final calculation. Cheers!

Dear Golizadeh ,

For the accurate determination of the current efficiency during alloy deposition, first you must to determine the mass of the alloy, and composition (EDS, X-ray.) Than from the Faraday law to determine the theoretical mass at given current:

mt = ItMa/(naF)

but where Ma is a molecular weight of alloy given as

sum(Mm*X) where Mm is a molecular weight of single metal in alloy and X is a ratio of metal in alloy. na is the average number of exchanged electrons for alloy, sum(nm*X), where nm is the number of electron for one metal in alloy.

For example for FeCr (from bath containing Fe2+ and Cr3+) with composition 0.3 Fe and 0.7 Cr

Ma = 55.8*0.3 + 52*0.7 = 53.14 g/mol

na = 2*0.3 + 3*0.7 = 2.7 electrons

(Ma/na) is usually called equivalent weight

Dividing experimental mass with theoretical and multiply with 100, you will get current efficiency.