Prior to electrochemical reaction the cyclic voltammetry behaviour of piperine was measured We have previously shown the voltammetric behaviour of a drug molecule is inversely correlated to it in situ metabolic half-life. Using ferrocene (Fc/Fc + ) as an internal standard for the pseudo Ag/AgCl wire reference electrode and a glassy carbon electrode (GCE) as the working electrode and a platinum wire as the counter electrode (CE), the cyclic voltammetry behaviour of piperine was explored (Figures Figure shows that the peak current (ip) of piperine increases with increasing analyte concentration because there are more redox-active species available to undergo oxidation at the electrode surface, and with increasing the scan rate (Figure ), the electrode potential changes more rapidly, and the rate of electron transfer reactions increases, leading to a larger peak current. These are consistent with the Randles-Sevcik equation and indicate the diffusion-controlled redox process. In this Randles-Sevcik equation at 25 °C , (ip= k n 3/2 A √𝐷𝑣 C), ip is the peak current, k is a constant of 2.69 x 10 5 C/ mol√𝑣, n is the number of electrons, A is the electrode area (cm 2 ), D is the analytes diffusion coefficient (cm 2 /s), ν is the rate at which the potential is swept (V/s), and C is concentration. The peak potential (Ep) depends on the scan rate or concentration if the oxidation peak potential shifts to more positive potentials, and the non-scan rate is dependent if the Ep remains relatively constant as the scan rate and concentration increase. This study showed that piperine's electrochemical reaction is not concentration-dependent (range concentration 0.0025-0.0040 M). However, the Ep slightly changed to a more positive potential at C = 0.0045 M, which means the reaction becomes unstable at higher concentrations. In the differential scan rate analyses (Figure ), it showed that the reaction slightly changed and was not significant. Proving that changing the scan rate does not affect the electrochemical reactions. Changing to the multiple scanning of potential waveforms provides several pieces of information, including reversibility or irreversibility of an electrochemical reaction. Figure depicts the multiple features of piperine CVs when using different applied potentials, and the apparent reversibility of some oxidation waves depends on the reversibility of later oxidation waves. Specifically, if the oxidation process generates an unstable species that degrades, all subsequent processes will be affected. For example, when scanning positively with applied potential, piperine will have four oxidation events with two return-reduction waves observed. For the next scanning, the reduction of X/X -means the process generates a new product (X -/X -2 ) that does not appear in the first scanning and increases for the subsequent scanning. However, if the X -3 or X -4 are unstable in the solution, there will not be much X -2 left for a return scan. In other words, X -2 /X -3 & X -3 /X -4 undergo an irreversible oxidation process or decomposition. and mixed diffusion-adsorption process (slope between 0.5 and 1.0). The positive slope of log10ip vs scan rate indicates a linear relationship that suggests the reactions process is electrochemically consistent with the Randles-Sevcik equation. The coefficient determination (R² value) indicates the correlation between the Ep/ip and scan rate. The closer to 0.0, the weaker correlation between the values, and the closer to 1.0, the stronger correlation the value is. In the case of piperine, log10 of peak potential (Ep) vs log10of scan rate (mVs -1 ) gave y = 0.0539x + 2.7743 and R² = 0.9503 shows that the redox process is diffusion-controlled (slope: 0.0539) and log10 of peak current (ip) log10 of scan rate (mVs -1 ) gave y = 0.5111x + 0.8329 and R² = 0.9503 meaning the electrochemical process is consistent with the Randles-Sevcik equation.