In the table, weight gain$-$time data for the oxidation of nickel at an elevated temperature are tabulated.

$($a$)$ Determine whether the oxidation kinetics obey a linear, parabolic, or logarithmic rate expression.

$($b$)$ Now compute $W$ after a time of $1000$min.

$m\frac{g}{c}{m}^2$Nickel experiences corrosion in an acid solution according to the reaction

$Ni+2H^{+}N{i}^{2+}+H_2$

The rates of both oxidation and reduction half$-$reactions are controlled by activation polarization.

For Nickel

$V_{(N\frac{i}{N}i2+)}=-0\mathrm{.}25V$

$i_0={10}^{-8}\frac{A}{c}{m}^2$

$=0\mathrm{.}11$

For Hydrogen

$V_{(H\frac{+}{H}2)}=0V$

$i_0=6{10}^{-7}\frac{A}{c}{m}^2$

$=-0\mathrm{.}10$

$($a$)$ Compute the rate of oxidation of $Ni$ given the following activation polarization data above.

$mo\frac{l}{c{m}^2-s}$

$($b$)$ Compute the value of the corrosion potential.

V