Randles–Sevcik equation

In electrochemistry, the Randles–Ševčík equation describes the effect of scan rate on the peak current i_p for a cyclic voltammetry experiment. For simple redox events such as the ferrocene/ferrocenium couple, i_p depends not only on the concentration and diffusional properties of the electroactive species but also on scan rate.[1]

${\displaystyle i_{p}=0.4463\ nFAC\left({\frac {nFvD}{RT}}\right)^{\frac {1}{2}}}$

Or if the solution is at 25 °C:[2]

${\displaystyle i_{p}=2.69\times 10^{5}\ n^{3/2}AC{\sqrt {Dv}}}$

• i_p = current maximum in amps
• n = number of electrons transferred in the redox event (usually 1)
• A = electrode area in cm²
• F = Faraday constant in C mol⁻¹
• D = diffusion coefficient in cm²/s
• C = concentration in mol/cm³
• ν = scan rate in V/s
• R = Gas constant in J K⁻¹ mol⁻¹
• T = temperature in K
• The constant with a value of 2.69x10⁵ has units of C mol⁻¹ V^−1/2

For novices in electrochemistry, the predictions of this equation appear counter-intuitive, i.e. that i_p increases at faster voltage scan rates. It is important to remember that current, i, is charge (or electrons passed) per unit time. In cyclic voltammetry, the current passing through the electrode is limited by the diffusion of species to the electrode surface. This diffusion flux is influenced by the concentration gradient near the electrode. The concentration gradient, in turn, is affected by the concentration of species at the electrode, and how fast the species can diffuse through solution. By changing the cell voltage, the concentration of the species at the electrode surface is also changed, as set by the Nernst equation. Therefore, a faster voltage sweep causes a larger concentration gradient near the electrode, resulting in a higher current.