Comparison of Different Electrochemical Methodologies for Electrode Reactions: A Case Study of Paracetamol

: Understanding electrochemical reactions at the surface of electrodes requires the accurate calculation of key parameters—the transfer coefficient ( α ), diffusion coefficient ( D 0 ), and heterogeneous electron transfer rate constant ( k 0 ). The choice of method to calculate these parameters requires careful consideration based on the nature of the electrochemical reaction. In this study, we conducted the cyclic voltammetry of paracetamol to calculate the values of these parameters using different methods and present a comparative analysis. Our results demonstrate that the E p − E p/ 2 equation for α and the modified Randles–Ševˇc í k equation for D 0 is particularly effective for the calculations of these two parameters. The Kochi and Gileadi methods are reliable alternatives for the calculation of k 0 . Nicholson and Shain’s method using the equation k 0 = Ψ ( π nD 0 F ν / RT ) 1/2 gives the overestimated values of k 0 . However, the value of k 0 calculated using the plot of ν − 1/2 versus Ψ (from the Nicholson and Shain equation, where ν is scan rate) agrees well with the values calculated from the Kochi and Gilaedi methods. This study not only identifies optimal methodologies for quasi-reversible reactions but also contributes to a deeper understanding of electrochemical reactions involving complex electron transfer and coupled chemical reactions, which can be broadly applicable in various electrochemical studies.


Introduction
A deep insight into electrochemical reactions on the surface of electrodes is essential to understanding the processes in catalysis, electrolysis, batteries, sensors, and fuel cells [1][2][3][4][5][6][7][8][9][10][11][12][13][14].Cyclic voltammetry-a simple, easy, and common technique-is a front-line tool to investigate reactions on electrode surfaces.Cyclic voltammetry is generally the first choice to test any material with potential application in these research areas for the determination of redox potentials and rates (for heterogeneous electron transfer and coupled chemical reactions) [15][16][17][18][19][20][21].However, the selection of a feasible method to explore reactions at the electrode surface is essential because of the complex nature of these reactions, i.e., electron transfer with chemically coupled reactions [22,23].No method is universal that works well for all kinds of reactions, hence requiring a careful choice of method depending on the nature of the reaction.
In electrochemical studies, the number of electrons transferred (n), the transfer coefficient (α), diffusion coefficient (D 0 ), and heterogeneous electron transfer rate constant (k 0 ) are essential parameters to explore reactions on the electrode surface.The transfer coefficient is the symmetry factor that affects the activation energy at the electrode surface, hence affecting the direction of the reaction.The diffusion coefficient is a transport parameter that is related to the transport of species toward and away from the surface of

Materials and Methods
LiClO 4 bought from Merck (Darmstadt, Germany) and paracetamol from Glaxo Smith Klein Pharmaceuticals (PVT) Ltd. (Karachi, Pakistan).In total, 10 mL of 1 × 10 −6 M of the paracetamol solution with 0.1 M of LiClO 4 as a supporting electrolyte in deionized water was prepared and used.The working electrode was polished using 0.2 µm of aluminum powder provided by CHI Instruments.All solutions were purged with nitrogen gas for 15 min before running cyclic voltammetry.
Cyclic voltammetry was carried out at room temperature using a CHI 760D Electrochemical Workstation, operated by an Intel Core 2 Quad-Supported IBM computer with a Windows XP operating system.All the electrochemical experiments were performed in a conventional three-electrode cell.The following electrodes were used: glassy carbon (GC) as the working electrode, platinum as the counter electrode, and the saturated calomel electrode (SCE) as the reference electrode.The digital simulation was carried out through DigiSim software built into the CHI 760D electrochemical workstation.The working electrode was polished with aluminum powder before use.The surface area of the working electrode was 0.0706 cm 2 , as provided by CHI Instruments (Austin, TX, USA; Model No. CHI 104).All reported potentials are referenced to the SCE potential.

Cyclic Voltammetry of Paracetamol
Before starting with the results, it is essential to understand the basic parameters that can be directly obtained from a cyclic voltammogram.These basic parameters include the peak potentials for anodic (E pa ) and cathodic (E pc ) reactions, as well as the corresponding peak currents for anodic (I pa ) and cathodic (I pc ) processes.From these four foundational parameters, several kinetic and thermodynamic parameters are derived.(1) Formal potential (E 1/2 ) is calculated as the absolute difference between E pc and E pa , divided by two (E 1/2 = |E pc − E pa |/2).The formal potential is also called standard reduction potential.(2) Peak separation (∆E p ), defined as the absolute difference between E pc and E pa (∆E p = |E pc − E pa |), is a parameter that is an immediate measure and shows the nature of the electron transfer process, distinguishing between reversible, quasi-reversible, or irreversible reactions.(3) The ratio of peak currents (I pc /I pa ), the ratio between the anodic and cathodic peak currents that provide insights into chemically coupled reactions, is also an important criterion to evaluate the nature of electron transfer.A value near unity indicates that reduced/oxidized species are stable and there are no chemically coupled reactions.In contrast, a value less than unity indicates the presence of chemically coupled reactions, resulting in the consumption of reduced/oxidized species.Utilizing E pa , E pc , I pa , I pc , and E 1/2 , one can calculate the transfer coefficient and the diffusion coefficient.These coefficients are instrumental in determining the heterogeneous electron transfer rate constants.Such calculations are pivotal in understanding the electron transfer kinetics and the overall electrochemical behavior of the analyte under study.
Cyclic voltammograms of the paracetamol solution were taken at the scan rate of 0.025 V/s to 0.300 V/s with an incremental change of 0.025 V/s and are presented in Figure 1.The scan rate, E pa , E pc , I pa , I pc , ∆E p , E 1/2 , and (I pc /I pa ), is presented in Table S1 of the Supplementary Information.The E pa was observed at 0.705 V at 0.025 V/s, which was shifted to 0.750 V at 0.300 V/s.The E pc shifted from 0.577 V to 0.564 V with the increase in the scan rate.The ∆E p increased from 0.128 V to 0.186 V as the scan rate was increased from 0.025 V/s to 0.300 V/s.An increase in ∆E p and a shift in peak potentials indicated the quasi-reversible nature of the electron transfer or higher uncompensated IR resistance.To check whether quasi-reversibility is attributed to slow electron transfer and not from higher uncompensated IR resistance, we plotted ∆E p vs. the sq.root of the scan rate as presented in Figure S1 of the Supplementary Information.A good regression with a linear trend indicates that ohmic resistance is negligible, and slow electron transfer is responsible for the quasi-reversibility of this process.Additionally, ∆E p is significantly higher than the peak separation of the reversible peak, i.e., 0.029 V for n = 2, (n = number of electron(s)), which shows the quasi-reversible nature of processes.Furthermore, Figure 1 clearly shows that the reverse peak is smaller than the forward peak.The ratio of I pc /I pa remains almost constant at 0.59 ± 0.03.The ratio of I pc /I pa has less than unity and a smaller reverse peak, both indicating the presence of chemically coupled reactions followed by the first electron transfer [32,33].
Electrochem 2024, 5, FOR PEER REVIEW 3 Epa|), is a parameter that is an immediate measure and shows the nature of the electron transfer process, distinguishing between reversible, quasi-reversible, or irreversible reactions.(3) The ratio of peak currents (Ipc/Ipa), the ratio between the anodic and cathodic peak currents that provide insights into chemically coupled reactions, is also an important criterion to evaluate the nature of electron transfer.A value near unity indicates that reduced/oxidized species are stable and there are no chemically coupled reactions.In contrast, a value less than unity indicates the presence of chemically coupled reactions, resulting in the consumption of reduced/oxidized species.Utilizing Epa, Epc, Ipa, Ipc, and E1/2, one can calculate the transfer coefficient and the diffusion coefficient.These coefficients are instrumental in determining the heterogeneous electron transfer rate constants.Such calculations are pivotal in understanding the electron transfer kinetics and the overall electrochemical behavior of the analyte under study.Cyclic voltammograms of the paracetamol solution were taken at the scan rate of 0.025 V/s to 0.300 V/s with an incremental change of 0.025 V/s and are presented in Figure 1.The scan rate, Epa, Epc, Ipa, Ipc, ΔEp, E1/2, and (Ipc/Ipa), is presented in Table S1 of the Supplementary Information.The Epa was observed at 0.705 V at 0.025 V/s, which was shifted to 0.750 V at 0.300 V/s.The Epc shifted from 0.577 V to 0.564 V with the increase in the scan rate.The ΔEp increased from 0.128 V to 0.186 V as the scan rate was increased from 0.025 V/s to 0.300 V/s.An increase in ΔEp and a shift in peak potentials indicated the quasireversible nature of the electron transfer or higher uncompensated IR resistance.To check whether quasi-reversibility is attributed to slow electron transfer and not from higher uncompensated IR resistance, we plotted ΔEp vs. the sq.root of the scan rate as presented in Figure S1 of the Supplementary Information.A good regression with a linear trend indicates that ohmic resistance is negligible, and slow electron transfer is responsible for the quasi-reversibility of this process.Additionally, ΔEp is significantly higher than the peak separation of the reversible peak, i.e., 0.029 V for n = 2, (n = number of electron(s)), which shows the quasi-reversible nature of processes.Furthermore, Figure 1 clearly shows that the reverse peak is smaller than the forward peak.The ratio of Ipc/Ipa remains almost constant at 0.59 ± 0.03.The ratio of Ipc/Ipa has less than unity and a smaller reverse peak, both indicating the presence of chemically coupled reactions followed by the first electron transfer [32,33].The first criterion we need to know is whether the reaction is adsorption-controlled or diffusion-controlled because both processes require different forms of electrochemistry.
Generally, I p correlates with the scan rate raised to some power, which is supposedly b here.If the reaction is adsorption-controlled, the I p vs. scan rate is linear (b = 1); if diffusion-controlled, the I p vs. sq.root of the scan rate is linear (b = 0.5).We plotted I p vs. the scan rate and I p vs. the sq.root of the scan rate in Figure 2a,b, respectively.Comparatively, the best fit for I p vs. the sq.root of the scan rate (Figure 2b) shows that the process is diffusion-controlled.However, R 2 for Figure 2a is 0.984 and 0.964, and Figure 2b is 0.997 (for both lines), indicating a very small difference in the values of R 2 .We adapted an alternate approach to confirm the nature of processes in which the log of the scan rate vs. the log of the peak current is plotted.The slope of this plot shows the nature of the process: a slope near unity indicates adsorption-controlled, and near 0.5 indicates a diffusion-controlled reaction [32,34].We plotted the log of a scan rate vs. the log of a peak current in Figure 2c. Figure 2c shows the slope close to ~0.5, which indicates that the reaction is diffusion-controlled.In the following sections, we calculated the transfer coefficient, diffusion coefficient, and electron transfer rate constant.
Electrochem 2024, 5, FOR PEER REVIEW 4 The first criterion we need to know is whether the reaction is adsorption-controlled or diffusion-controlled because both processes require different forms of electrochemistry.Generally, Ip correlates with the scan rate raised to some power, which is supposedly b here.If the reaction is adsorption-controlled, the Ip vs. scan rate is linear (b = 1); if diffusioncontrolled, the Ip vs. sq.root of the scan rate is linear (b = 0.5).We plotted Ip vs. the scan rate and Ip vs. the sq.root of the scan rate in Figure 2a,b, respectively.Comparatively, the best fit for Ip vs. the sq.root of the scan rate (Figure 2b) shows that the process is diffusioncontrolled.However, R 2 for Figure 2a is 0.984 and 0.964, and Figure 2b is 0.997 (for both lines), indicating a very small difference in the values of R 2 .We adapted an alternate approach to confirm the nature of processes in which the log of the scan rate vs. the log of the peak current is plotted.The slope of this plot shows the nature of the process: a slope near unity indicates adsorption-controlled, and near 0.5 indicates a diffusion-controlled reaction [32,34].We plotted the log of a scan rate vs. the log of a peak current in Figure 2c. Figure 2c shows the slope close to ~0.5, which indicates that the reaction is diffusion-controlled.In the following sections, we calculated the transfer coefficient, diffusion coefficient, and electron transfer rate constant.

Transfer Coefficient
The transfer coefficient, a critical parameter in electrochemical studies, significantly affects the activation energy of the electron transfer rate.The transfer coefficient typically ranges from 0.3 to 0.7, with a general assumption of 0.5 in calculations of the electron transfer rate constant.However, for accurate measurements of the heterogeneous electron transfer rate constant, the precise quantification of the transfer coefficient is essential.In this study, we determined the transfer coefficient using the following two methods: the Tafel plot and another method referred to as Equation (1).
The Tafel plot method involves plotting the logarithm of the current against potential.For our measurements, we selected the current and potential values from the cyclic voltammograms of paracetamol at scan rates of 0.025 V/s and 0.300 V/s, focusing on the potential range of 0.62 V to 0.75 V, where the oxidation peaks are prominent as shown in Figure 3.In these Tafel plots, we observed slopes of −22.69 at 0.025 V/s and −14.65 at 0.300 V/s, corresponding to transfer coefficient values of 0.34 and 0.57, respectively.These values were calculated using the following relation: slope = −(1 − α)nF/2.3RT.It is crucial to carefully select the points for slope measurement in the Tafel plot, aiming for the descending straight part of the curve that is close to the horizontal current line.The lines used to calculate slopes are shown in Figure S2 in the Supplementary Information.This careful selection is important because even a minor error in identifying the slope points can lead to significant deviations in the transfer coefficient value.

Transfer Coefficient
The transfer coefficient, a critical parameter in electrochemical studies, significantly affects the activation energy of the electron transfer rate.The transfer coefficient typically ranges from 0.3 to 0.7, with a general assumption of 0.5 in calculations of the electron transfer rate constant.However, for accurate measurements of the heterogeneous electron transfer rate constant, the precise quantification of the transfer coefficient is essential.In this study, we determined the transfer coefficient using the following two methods: the Tafel plot and another method referred to as Equation (1).
The Tafel plot method involves plotting the logarithm of the current against potential.For our measurements, we selected the current and potential values from the cyclic voltammograms of paracetamol at scan rates of 0.025 V/s and 0.300 V/s, focusing on the potential range of 0.62 V to 0.75 V, where the oxidation peaks are prominent as shown in Figure 3.In these Tafel plots, we observed slopes of −22.69 at 0.025 V/s and −14.65 at 0.300 V/s, corresponding to transfer coefficient values of 0.34 and 0.57, respectively.These values were calculated using the following relation: slope = −(1 − α)nF/2.3RT.It is crucial to carefully select the points for slope measurement in the Tafel plot, aiming for the descending straight part of the curve that is close to the horizontal current line.The lines used to calculate slopes are shown in Figure S2 in the Supplementary Information.This careful selection is important because even a minor error in identifying the slope points can lead to significant deviations in the transfer coefficient value.To validate the transfer coefficient values obtained from the Tafel plot, we also employed another method, referred to as Equation (1) [34,35].This method requires only two electrochemical parameters as follows: Ep and Ep/2, as shown in Equation ( 1), and values calculated from Equation ( 1) are presented in Table 1.
Here, α is the transfer coefficient, n is the number of electrons involved (n = 2) [31,33], and Ep and Ep/2 are in mV.We found the values of the transfer coefficient between 0.62 and 0.36 at scan rates ranging from 0.025 V/s to 0.300 V/s, respectively, as shown in Table 1.The average value is 0.43.Table 1 shows that the value of α depends on the scan rate; as the scan rate increases, α decreases, as previously reported [36].Here, the values of transfer coefficients are in close agreement with the values calculated using the Tafel plots.Additionally, this method is easy compared to the Tafel plot method, which requires a very careful selection of points for calculating the slope.To validate the transfer coefficient values obtained from the Tafel plot, we also employed another method, referred to as Equation (1) [34,35].This method requires only two electrochemical parameters as follows: E p and E p/2 , as shown in Equation ( 1), and values calculated from Equation ( 1) are presented in Table 1.
Here, α is the transfer coefficient, n is the number of electrons involved (n = 2) [31,33], and E p and E p/2 are in mV.We found the values of the transfer coefficient between 0.62 and 0.36 at scan rates ranging from 0.025 V/s to 0.300 V/s, respectively, as shown in Table 1.The average value is 0.43.Table 1 shows that the value of α depends on the scan rate; as the scan rate increases, α decreases, as previously reported [36].Here, the values of transfer coefficients are in close agreement with the values calculated using the Tafel plots.Additionally, this method is easy compared to the Tafel plot method, which requires a very careful selection of points for calculating the slope.

Diffusion Coefficient
The diffusion coefficient was determined using the modified Randles-Ševčík equation for a quasi-reversible process, as presented in Equation (2) [37] I p = 2.99 × 10 5 ACn(αnD 0 ν) 1/2  (2) Here, I p is the peak current, A is the area of the working electrode in cm 2 , C is the concentration in mmol/cm 3 , n is the number of electrons involved (n = 2) [31], ν is the scan rate in V/s, D 0 is the diffusion constant in cm 2 /s, and α is the transfer coefficient.The calculated values using Equation ( 2) are presented in Table 2.These values are averaged to 2.19 × 10 −5 cm 2 /s with the smallest value of 1.25 × 10 −5 cm 2 /s and the largest value of 3.10 × 10 −5 cm 2 /s at a scan rate of 0.025 and 0.300 V/s, respectively.Additionally, D 0 can be determined using the slope of I p vs. the sq.root of the scan rate (from Figure 2b) according to Equation (3).This method gives the value of 2.42 × 10 −5 cm 2 /s, which is in close agreement with the average value determined from Equation (2).D 0 = (slope/(2.99× 10 5 ACn(αnD 0 ν) This value from the slop method had an added advantage of background subtraction due to uncompensated resistance and contribution from the capacitive current.

Heterogeneous Electron Transfer Rate Constant
The determination of the heterogeneous electron transfer rate constant (k 0 ) is a pivotal aspect of characterizing any new electrochemical system.This parameter is integral to understanding the kinetics of electron transfer processes at the electrode-electrolyte interface.
In our study, we employed three different methods to calculate k 0 , each contributing to a comprehensive understanding of the electrochemical behavior of the system.The first method utilized was the Nicholson and Shain method [7]: a widely recognized approach in electrochemical kinetics.This method, based on the analysis of cyclic voltammograms, allows for the estimation of k 0 by examining the relationship between peak separation and scan rates using a dimensionless parameter Ψ.In addition to Nicholson and Shain method, we also employed Kochi's method [14].Kochi's approach offers a different perspective on determining k 0 , focusing on the relationship between the electron transfer rate, overpotential and transfer coefficient.Lastly, the Gileadi method [38] was applied.This method is renowned for its robustness in analyzing the heterogeneous electron transfer processes, particularly in systems where electron transfer is coupled with other chemical reactions, i.e., for irreversible reactions.

Nicholson and Shain Method
Nicholson and Shain provided a simple and elegant method to determine k 0 , as shown in Equation ( 4) [30] k 0 = Ψ(πnD 0 Fν/RT) 1/2 (4) Here, Ψ is a dimensionless kinetic parameter that depends on peak separation.All other symbols have their usual meaning, as discussed earlier in Equations ( 1)-(3).Later, Lavagnini et al. provided a quantitative relationship between Ψ and peak separation according to Equation ( 5) [39] Here, ∆E p is the peak separation in mV.The values of ∆E p in (mv), Ψ, and k 0 are provided in Table 3.The average value of k 0 was found to be 0.022 cm/s.Alternatively, Equation ( 5) can be rearranged into Equation (6).
Here, the value of k 0 can be calculated using the slope of the plot of Ψ versus (ν) −1/2 .The slope is equal to the expression k 0 (RT/πnD 0 F) 1/2 .We present the plot of Ψ vs. (ν) −1/2 in Figure 4.The value calculated for k 0 from the trend line from Figure 4 was found to be 0.010 cm/s, which is smaller than the values calculated for the values of k 0 from those calculated from Equation (4) (Table 3).
4. The value calculated for k 0 from the trend line from Figure 4 was found to be 0.010 cm/s, which is smaller than the values calculated for the values of k 0 from those calculated from Equation (4) (Table 3).

Kochi Method
In order to compare the value of k 0 with another method, we used the Kochi method to calculate the value of k 0 .Kochi and Klinger formulated this correlation between k 0 and peak separation.They developed this formula using the Nicholson and Shain expressions [40,41] In this expression, all symbols have their usual meanings.In this expression, the value of the transfer coefficient is retained, which is not in the Nicholson and Shain equation.The values of calculated k 0 using Equation ( 7) are presented in Table 4.The values of k 0 range from 0.001 to 0.013 cm/s, with an average value of 0.07 cm/s.This value could be more reliable because it considers the value of the transfer coefficient.

Gileadi Method
The Gileadi method is relatively simple and does not require peak separation.This method works well for the system where a reversible peak is absent [32,38].

Kochi Method
In order to compare the value of k 0 with another method, we used the Kochi method to calculate the value of k 0 .Kochi and Klinger formulated this correlation between k 0 and peak separation.They developed this formula using the Nicholson and Shain expressions [40,41] In this expression, all symbols have their usual meanings.In this expression, the value of the transfer coefficient is retained, which is not in the Nicholson and Shain equation.The values of calculated k 0 using Equation (7) are presented in Table 4.The values of k 0 range from 0.001 to 0.013 cm/s, with an average value of 0.07 cm/s.This value could be more reliable because it considers the value of the transfer coefficient.

Gileadi Method
The Gileadi method is relatively simple and does not require peak separation.This method works well for the system where a reversible peak is absent [32,38].
Here, all symbols have their usual meaning.Vc is the critical scan rate where the system undergoes a transition from a quasi-reversible to an irreversible system.Vc is determined using the plot of peak potential versus the log of the scan rate, as shown in Figure 5. Two straight trends were found at lower and higher scan rates with different slopes, and their intersection provided the value of Vc. Figure 5 shows that the log of the scan rate value is about −0.72, which corresponds to the 0.190 V/s scan rate (indicated by pink arrow).At the 0.190 V/s scan rate, Equation ( 8) produces the value of 0.017 cm/s.logk 0 = −4.8α+ 0.52 + log (αnD0FVc/2.303RT) 1/2  (8) Here, all symbols have their usual meaning.Vc is the critical scan rate where the system undergoes a transition from a quasi-reversible to an irreversible system.Vc is determined using the plot of peak potential versus the log of the scan rate, as shown in Figure 5. Two straight trends were found at lower and higher scan rates with different slopes, and their intersection provided the value of Vc. Figure 5 shows that the log of the scan rate value is about −0.72, which corresponds to the 0.190 V/s scan rate (indicated by pink arrow).At the 0.190 V/s scan rate, Equation ( 8) produces the value of 0.017 cm/s.

Digital Simulation
The digital simulation of the cyclic voltammogram is a method to validate the transfer coefficient, diffusion coefficient, and heterogeneous electron transfer rate constant using all these parameters together.In a digital simulation, input data from experiments were fed into simulation software, which generated a cyclic voltammogram using theoretical equations involving second or higher-order chemical reactions coupled with electron transfer.This method can be particularly used to calculate the rate constants for homogeneous chemical reactions and coupled reactions with electron transfer.
We used the reaction mechanism shown in Scheme 1 to simulate the cyclic voltammogram.A simple representation is shown in the lower part of Scheme 1. Paracetamol undergoes two electron transfers and forms acetic acid and p-Benzoquinone imine in the aqueous solution.

Digital Simulation
The digital simulation of the cyclic voltammogram is a method to validate the transfer coefficient, diffusion coefficient, and heterogeneous electron transfer rate constant using all these parameters together.In a digital simulation, input data from experiments were fed into simulation software, which generated a cyclic voltammogram using theoretical equations involving second or higher-order chemical reactions coupled with electron transfer.This method can be particularly used to calculate the rate constants for homogeneous chemical reactions and coupled reactions with electron transfer.
We used the reaction mechanism shown in Scheme 1 to simulate the cyclic voltammogram.A simple representation is shown in the lower part of Scheme 1. Paracetamol undergoes two electron transfers and forms acetic acid and p-Benzoquinone imine in the aqueous solution.logk 0 = −4.8α+ 0.52 + log (αnD0FVc/2.303RT) 1/2  (8)   Here, all symbols have their usual meaning.Vc is the critical scan rate where the system undergoes a transition from a quasi-reversible to an irreversible system.Vc is determined using the plot of peak potential versus the log of the scan rate, as shown in Figure 5. Two straight trends were found at lower and higher scan rates with different slopes, and their intersection provided the value of Vc. Figure 5 shows that the log of the scan rate value is about −0.72, which corresponds to the 0.190 V/s scan rate (indicated by pink arrow).At the 0.190 V/s scan rate, Equation ( 8) produces the value of 0.017 cm/s.

Digital Simulation
The digital simulation of the cyclic voltammogram is a method to validate the transfer coefficient, diffusion coefficient, and heterogeneous electron transfer rate constant using all these parameters together.In a digital simulation, input data from experiments were fed into simulation software, which generated a cyclic voltammogram using theoretical equations involving second or higher-order chemical reactions coupled with electron transfer.This method can be particularly used to calculate the rate constants for homogeneous chemical reactions and coupled reactions with electron transfer.
We used the reaction mechanism shown in Scheme 1 to simulate the cyclic voltammogram.A simple representation is shown in the lower part of Scheme 1. Paracetamol undergoes two electron transfers and forms acetic acid and p-Benzoquinone imine in the aqueous solution.The best fit of the simulated voltammogram at 0.300 V/s is presented in Figure 6.The best fit of CV was achieved using the following parameters: E 1/2 = 0.645 V; α = 0.28; D 0 = 2.45 × 10 −5 cm 2 /s; k 0 0.017 cm/s; K f = 9 × 10 −6 M −1 s −1 and K b = 850 M −1 s −1 .The reproduction of a fitted cyclic voltammogram using these parameters validates the accuracy of the methodologies used in this study.
The best fit of the simulated voltammogram at 0.300 V/s is presented in Figure 6.The best fit of CV was achieved using the following parameters: E1/2 = 0.645 V; α = 0.28; D0 = 2.45 × 10 −5 cm 2 /s; k 0 0.017 cm/s; Kf = 9 × 10 −6 M −1 s −1 and Kb = 850 M −1 s −1 .The reproduction of a fitted cyclic voltammogram using these parameters validates the accuracy of the methodologies used in this study.

Discussion
In this study, we investigated the electrochemical oxidation of paracetamol in an aqueous medium using cyclic voltammetry and a digital simulation.We determined the transfer coefficient using the following two different methods: the Tafel plot and Equation (1).The diffusion coefficient was determined for the individual scan rate, average value, and slope method using the modified Randles-Ševčík equation.The heterogeneous electron transfer rate constant was determined using the following three different methods: the Nicholson and Shain method and the Kochi and Gileadi method.Then, all parameters were used to simulate the voltammogram with the built-in feature of the CHI 760D electrochemical workstation, which reproduced sufficiently with the experimental cyclic voltammogram (Figure 5).
These results show that the value of α depends on the scan rate for paracetamol, even in the narrow range of the scan rate.The value of α varied from 0.62 to 0.31 at 0.025 V/s to a 0.300 V/s scan rate, respectively.Additionally, Equation ( 1) is an easy approach to determine α compared to the Tafel plot method.While taking points for the slop, a slop needs to be taken as near as possible to the horizontal line, as shown in Figure S2 in the Supplementary Information.
The value of D0 using the modified Randles-Ševčík equation ranges from 1.25 to 3.10 × 10 −5 cm 2 /s with an average value of 2.19 × 10 −5 cm 2 /s.Moreover, the value of D0 calculated from the slope of the plot of Ip versus (ν) 1/2 was found to be 2.42 × 10 −5 cm 2 /s, which is closer to the average value.The slop method is considered feasible because of the cancellation of the capacitive current contribution in Ip.
The value of k 0 from Nicholson and Shain using Equation (4) lies between 0.018 and 0.025 cm/s with an average value of 0.022 cm/s.However, the value of k 0 calculated from the linear plot of (ν) -1/2 versus Ψ is 0.010 cm/s, which is lower than the values calculated

Discussion
In this study, we investigated the electrochemical oxidation of paracetamol in an aqueous medium using cyclic voltammetry and a digital simulation.We determined the transfer coefficient using the following two different methods: the Tafel plot and Equation (1).The diffusion coefficient was determined for the individual scan rate, average value, and slope method using the modified Randles-Ševčík equation.The heterogeneous electron transfer rate constant was determined using the following three different methods: the Nicholson and Shain method and the Kochi and Gileadi method.Then, all parameters were used to simulate the voltammogram with the built-in feature of the CHI 760D electrochemical workstation, which reproduced sufficiently with the experimental cyclic voltammogram (Figure 5).
These results show that the value of α depends on the scan rate for paracetamol, even in the narrow range of the scan rate.The value of α varied from 0.62 to 0.31 at 0.025 V/s to a 0.300 V/s scan rate, respectively.Additionally, Equation ( 1) is an easy approach to determine α compared to the Tafel plot method.While taking points for the slop, a slop needs to be taken as near as possible to the horizontal line, as shown in Figure S2 in the Supplementary Information.
The value of D 0 using the modified Randles-Ševčík equation ranges from 1.25 to 3.10 × 10 −5 cm 2 /s with an average value of 2.19 × 10 −5 cm 2 /s.Moreover, the value of D 0 calculated from the slope of the plot of I p versus (ν) 1/2 was found to be 2.42 × 10 −5 cm 2 /s, which is closer to the average value.The slop method is considered feasible because of the cancellation of the capacitive current contribution in I p .
The value of k 0 from Nicholson and Shain using Equation (4) lies between 0.018 and 0.025 cm/s with an average value of 0.022 cm/s.However, the value of k 0 calculated from the linear plot of (ν) −1/2 versus Ψ is 0.010 cm/s, which is lower than the values calculated from Equation (4).The value of k 0 from the Kochi method lies in the range of 0.001 to 0.013 cm 2 /s with an average value of 0.070 cm 2 /s.The value of k 0 using the Gileadi method is 0.017 cm/s.Nicholson and Shain's method calculated from the plot of (ν) −1/2 versus Ψ is closer to the value calculated from Kochi and Gileadi's methods.Additionally, Kochi and Gileadi's methods are a better choice for an electron transfer followed by a coupled chemical reaction, as in the case of paracetamol here.The value of k 0 from the Nicholson and Shain method is slightly different, as noted in previous studies [28,32].We also note that the Kochi method shows that the value of k 0 varies with the change in the scan rate, which is possibly due to the change in the transfer coefficient.In Nicholson and Shain's method, the value of 0.5 was assumed while calculating the kinetic parameter Ψ, hence reproducing a constant value.At last, the digital simulation shows that the values calculated from these methods have reasonable accuracy, which reproduces a cyclic voltammogram with very good fitting.

Conclusions
This study presents a comprehensive analysis of the various methods used for calculating key electrochemical parameters, with a particular focus on paracetamol.Through meticulous experiments and comparisons, we demonstrated that the combined application of the E p − E p/2 equation, Randles-Ševčík equation, and Kochi and Gileadi method approaches were particularly effective for accurately determining the transfer coefficient, diffusion coefficient, and heterogeneous electron transfer rate constant, respectively.These findings reveal that the Kochi and Gileadi methods are reliable alternatives for calculating the heterogeneous electron transfer rate constant for chemically coupled electron transfer processes.Moreover, our study successfully employed digital simulation as a tool to validate these electrochemical parameters, ensuring their accuracy and reliability.This approach also unraveled the kinetics of chemically coupled reactions, offering deeper insights into the complex interplay of reactions in electrochemical systems.The methodologies validated and the insights gained can be applied to a wide range of electrochemical studies, particularly those involving complex electron transfer and coupled chemical reactions.

Figure 1 .
Figure 1.Cyclic voltammograms of 1 × 10 −6 M of the paracetamol solution with 0.1 M of LiClO4 as the supporting electrolyte in the aqueous solution at different scan rates.Arrows show the direction of potential scan.

Figure 1 .
Figure 1.Cyclic voltammograms of 1 × 10 −6 M of the paracetamol solution with 0.1 M of LiClO 4 as the supporting electrolyte in the aqueous solution at different scan rates.Arrows show the direction of potential scan.

Figure 2 .
Figure 2. The plot of the (a) peak current versus scan rate and (b) peak current versus the sq.root of the scan rate.(c) The log of peak current versus the log of the scan rate (blue, anodic; red, cathodic).

Figure 2 .
Figure 2. The plot of the (a) peak current versus scan rate and (b) peak current versus the sq.root of the scan rate.(c) The log of peak current versus the log of the scan rate (blue, anodic; red, cathodic).

Figure 3 .
Figure 3. Tafel plots drawn at 0.025 V/s and 0.300 V/s for the anodic peak.

Figure 3 .
Figure 3. Tafel plots drawn at 0.025 V/s and 0.300 V/s for the anodic peak.

Figure 5 .
Figure 5.The plot of peak potential versus the log of the scan rate (Vc corresponds to 0.190 V/s as indicated by pink vertical arrow).

Scheme 1 .
Scheme 1.The reaction mechanism used to simulate the cyclic voltammogram.

Figure 5 .
Figure 5.The plot of peak potential versus the log of the scan rate (Vc corresponds to 0.190 V/s as indicated by pink vertical arrow).

Figure 5 .
Figure 5.The plot of peak potential versus the log of the scan rate (Vc corresponds to 0.190 V/s as indicated by pink vertical arrow).

Scheme 1 . 1 .
Scheme 1.The reaction mechanism used to simulate the cyclic voltammogram.Scheme 1.The reaction mechanism used to simulate the cyclic voltammogram.

Table 1 .
The value of transfer coefficients calculated from Equation (1) at different scan rates.

Table 2 .
The values of the diffusion coefficient calculated from Equation (2) at different scan rates.

Table 4 .
Calculated values of k 0 using the Kochi and Klinger method.

Table 4 .
Calculated values of k 0 using the Kochi and Klinger method.