General Spectroscopy - Nitric acid as oxidizing agent

We have not found a reference on this topic that goes into detail. However, the chemistry of nitric acid is of interest to Inorganic Ventures. The following is our understanding of this chemistry:There are two reactions that nitric acid follows. In dilute solutions the reaction is: NO₃^- + 4H⁺ + 3e- = NO + 2H₂O; E⁰ = 0.96. Assuming you are working in dilute solutions then the expression for ΔE (the reduction potential difference between two half cells) is: (ΔE) = 0.0591/n logK, where ΔE is from the oxidation reduction reaction equation, n is number of electrons, and logK is the equilibrium expression for the reaction. In addition, the half reaction potential (E) for nitric acid may be estimated using the Nernst Equation, where E = E⁰ + 0.0591/3log[(H⁺)⁴ (NO₃^-)]/(P_NO). This equation predicts an increase in the reduction potential (increase in oxidizing ability) as the acidity and molarity of nitric acid increases. Please keep in mind that this assumes a reaction that is not kinetically limited (irreversible).