Hello, i was trying to perform cyclic voltammetry experiment for one of my copper complex for Hydrogen evolution. I have recorded the CV of my catalyst first at different different scan rate. Then i fixed one of the scan rate and after that added Acetic acid in the mixture and perform the electrochemistry where the current rises during reductive scan. Now i am unable to understand how i will use this Cyclic Voltammogram to calculate the K(obs) i.e. TOF and Overpotential also.
Can you please provide me solution for this or any useful contents/articles where i could resolve this issue.
To perform the Hydrogen Evolution Reaction (HER) in an acetic acid medium, the turnover frequency (TOF) can be calculated using the formula: TOF = (j × A) / (2 × n × F × M), where jis the current density (A/cm²), A is the surface area of the electrode (cm²), n is the number of electrons transferred (typically 2 for HER), Fis Faraday's constant (96485 C/mol), and M is the catalyst's molar mass in g/mol, calculated as molar mass / 0.005. For the overpotential (η), plot the logarithm of the current density (log j) on the x-axis against the corresponding potential (V) on the y-axis.
create a table in Excel listing current density (j) and corresponding overpotential values(Pot vs RHE-1.23). Locate the overpotential value in the row where the current density equals 10 mA/cm². Multiply the result by 1000 to convert it to millivolts (mV).
Here you may find a thorough and foundational publication that also encloses answer to your points, hope it helps
Article Turnover Numbers, Turnover Frequencies, and Overpotential in...
According to IUPAC definition, the apparent TurnOver Frequency is the TON/(reaction time), where TON of the TurnOver Number. TON =(the amount of product in moles)/(amount of catalyst in moles). Thus, in order to measure TOF you MUST quantify the amount of products. Other formulas are based on assumptions.
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