Do For Fe corroding in the aerated solution with the concentration of ferrous ions is equal to $1\mathrm{.}62{10}^{-2}$

$M,$ the anodic dissolution shows the activation polarization. The cathodic polarization curves at

velocity $1($V$1)$ and velocity $2($V$2)$ are shown in the following polarization diagram $($some hints are

included$).$ We have the following data for this corrosion system.

For the anodic process: $b_{a,Fe}=0\mathrm{.}1V,i_{o,a}={10}^{-8}\frac{A}{m^2}$

$($a$)$ Determine the equilibrium potential of the above Fe electrode.

$($b$)$ Sketch the activation polarization curve for anodic reaction on the diagram, and label the curves

completely, including the reactions. $($Use theoretical polarization curve, i$.$e$.,$ ignore the

deviation near the equilibrium potential.$)$

$($c$)$ Is $V1>V2$ or $V1?$

$(d)Is$ corrosion controlled $by$ activation $or$ diffusion $atV1?$

$(e)Is$ corrosion controlled $by$ activation $or$ diffusion $atV2?$

$(f)$ What $is$ the corrosion current density $at$ velocity $2?$

$(g)$ What $is$ the corrosion potential $at$ velocity $2?$

$(h)$ What $is$ the corrosion potential $at$ velocity $2vs.$ SCE?

Do not use ChatGPT or other chegg answers.