Kinetics and mechanism of the electrochemical oxidation of the NO−2 ion on platinum in AgNO2-acetonitrile solution

TLDR: In this article, the anodic oxidation of NO − 2 ion dissolved as AgNO 2 in ACN, in the range − 12° to 68°C, was investigated using platinum electrodes.

About: This article is published in Electrochimica Acta.The article was published on 1974-11-01 and is currently open access. It has received 14 citations till now. The article focuses on the topics: Electrochemical reaction mechanism & Reaction mechanism.

Figures

Fig 10 Arrhenius plot of the anodic current peak related to NO; ion oxidation. Data are taken from voltammograms run :it diKcrent I’: I.7 x II) ’ M AgNU, + O-5 M L.i<‘lO,.

Fig. 23. Log(current) 1.9. log(NOJ ion concentration) at u constant overvoltage (0.5 VI, and 0 C’. The stragbtline carresponds to the Ist. order law.

Frequently asked questions

Q1. What have the authors contributed in "Kinetics and mechanism of the electrochemical oxidation of the no, ion on platinum in agno,-acetonitrile solution" ?

The electrochemical reaction is interpreted with the following sequence of reactions: 

Q2. What is the mechanism of oxidation of NO?

It should also be mentioned that any oxidation reaction of NO, yielding NO: ion must occur at a potential more anodic than that of the NO electrochemical oxidation. 

Q3. What is the mechanism of oxidation of NOz?

The anodic oxidation of NOz, as inferred from its behaviour on Pt in 98% H,S04, is much more irreversible than the NO oxidation[ 18, I’)]. 

Q4. What is the kinetic analysis of the E/I curves?

the kinetic analysis of the E/I curves must be restricted to anodic potentials lower than 0.5 V depending on T, where the interference of the reversible anodic oxidation of NO is still negligible. 

Q5. What is the theory of voltammetric curves?

According to the theory of vol-tammetric E/I curves for an ece mechanism[lS], for the case just described, the observed single sweep voltammogram can be conceived as the addition of the voltammograms of the individual electron transfer processes. 

Q6. What is the peak height of the oxidation of NO?

The peak height depends approximately linearly on c”‘. but the line does not intercept the orlgln of coordinates, as it is expected for a catalytic electrochemical reaction. 

Q7. What is the limiting current in NO?

the apparent solvodynamic radius of NO; ion both in ACN and DMSO obtained from the Einstein-Stokes ratio is about 4 A.~1 he anodlc current peaks and the limiting current increase with temperature according to arl Arrherriustype law. 

Q8. What is the voltammogram for the first anodic peak?

the experimental voltammogram for the first anodic peak was theoretically calculated from the equation derived for an irreversible diffusioncontrolled process[ 163.I = nFAC1;(7c &b)“‘$(bt) (7)where II is the number of electrons per mole of reacting species; A is the electrode area; C$ is the concentration of the reacting species whose diffusion coefficient is D,; h is equal to the ratio m,Ft,/RT, where ~1, is the product of b, the transfer coeficent, and n,, the number of electrons entering the rate determining step and $(bt) corresponds to the current function of the irreversible diffusion controlled reaction[16]. 

Q9. What is the transfer coefliclent derived from these calculations?

The transfer coefliclent derived from these calculations is again O-5 in a good correspondcncc with that employed in equation (71 to draw the first peak of the voltammogram. 

Q10. What is the voltammetric equation for the second anodic current peak?

The second anodic current peak was calculated according to the equation of a reversible diffusion-controlled reaction[16]:I = nFAC;(n L+,a)“‘$(at) (f-9where a = nFv/RT and $(at) is the corresponding current function.