Interfacial charge-transfer reactions in electrochemical systems often involve multiple reaction steps . For multi-step reactions, the experimentally measured (i.e., apparent) α value is understood to be a compound parameter, which can be different than the α values of each elementary reaction step . The mechanisms of multi-step electron-transfer reactions can often be understood through analysis of the apparent α value, for example, by the quasi-equilibrium method . However, it must be reiterated that the equations developed in this work are related purely to the experimental measurement of the apparent α value, and should not be construed to imply any mechanistic conclusions about the apparent α value. It must also be recognized that the empirical models derived so far, which assume one-step symmetric BV kinetics, may not provide a sufficiently accurate description of the interfacial kinetics for multi-step reactions. For the sake of mathematical simplicity, we assume that the interfacial kinetics can be fully described by the BV equation, but this assumption is understood not to be universally valid for real electrochemical systems. For example, there are many reported cases of elementary steps in multi-step reactions (e.g., coupled chemical reactions) which do not follow the BV equation; this can, but does not necessarily, cause the measured interfacial kinetics to deviate from the BV equation . If the measured kinetics of at least one reaction step is to deviate from the BV equation, this deviation would manifest as a quantitative disagreement between the experimental data and the mathematical models developed herein, in which case alternative models would be needed to fit the empirical data. However, no such disagreement is observed in the present work.