# The weight loss of an aluminum (Al) alloy corroding in HCI acid was observed to be 0.250 g/cm2 after

3 answers

###### Question:

The weight loss of an aluminum (Al) alloy corroding in HCI acid was observed to be 0.250 g/cm2 after an 8 h immersion period. What is the corresponding corrosion current density in mA/em2, assuming that all the corrosion is due to the reaction: Al → Al3+ + 3e

The atomic weight of Al is 26.98 g/mol.

The atomic weight of Al is 26.98 g/mol.

## Answers

I = 0.0931 A/cm^2 or 93.1 mA/cm^2

Explanation:

The computation of the corresponding corrosion is shown below:

As we know that

The mathematical form is

[tex]m=\frac{Q}{F} \frac{M}{z}[/tex]

where,

m = substance mass

Q= total electric charge

F= Faradays constant i.e. = 96,500 C/mol

M = Substance molar mass

z = number of electrons transferred

Now

Q = It

where

I = current

And t = time

[tex]m=\frac{Q}{F} \frac{M}{z}[/tex]

So,

[tex]I = \frac{mFz}{tM}[/tex]

Now it is mentioned that

z=3, M=26.98 g/mol, m=0.25 g/cm2

So,

[tex]I= \frac{0.25 g/cm^2 \times 96,500 C/mol \times 3}{((8\times60\times60 s)} \times 26.98 g/mol)[/tex]

Hence,

I = 0.0931 A/cm^2 or 93.1 mA/cm^2

A.

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