Consider a Reaction Given By
-In the Above Reaction, the Rate Constants Are Given

Consider a reaction given by $\begin{array} { l } M \underset { k _ { - 1 } } { \stackrel { k _ { 1 } } { \rightleftarrows } } M _ { a ds } ^ { + } + e ^ { - } \\M _ { a d s } ^ { + }\underset { k _ { - 2 } } { \stackrel { k _ { 2 } } { \rightleftarrows } } M _ { sol } ^ { + }\end{array}$ .
-In the above reaction, the rate constants are given by
$$k _ { i } = k _ { i 0 } e ^ { b ^ { \prime } E }$$
where E is measured wrt equilibrium potential. Given that k₁₀ = 10^-7 mol cm^-2 s^-1, b₁ = 20 V^-1, b_-1 = -18 V^-1 , k₂ = 10^-5 mol cm^-2 s^-1, k_-2 = 10⁰ cm s^-1 and the concentration of
$$M _ { s o l } ^ { 2 + }$$
as 25 mM, determine (i) k_-10 = ___________ mol cm^-2 s^-1 . At E = 0.3 V vs. "Equilibrium. potential", (ii) value of k_1dc = ___________mol cm^-2 s^-1, (iii) k_-1dc = ___________mol cm^-2 s^-1, (iv) steady state fractional surface coverage of the intermediate is _______
Remember that 1 M = 1 mol/lit = 10^-3 mol/ cm³.