**Calculate the Formal Potential, \( E' \), for the Given Reaction****Reaction Equation:**\[\text{NO}_3^-(aq) + 3 \text{H}^+(aq) + 2 \text{e}^- \rightleftharpoons \text{HNO}_2(aq) + \text{H}_2\text{O}(l) \quad E^\circ = 0.940 \, \text{V}\]**Additional Information:**- Nitrous acid, \(\text{HNO}_2\), has a dissociation constant, \( K_a \), of \( 7.1 \times 10^{-4} \).**Task:**Calculate the formal potential, \( E' \), for the above reaction.**Provided Calculation:**- An incorrect answer was submitted: \( E' = 0.845 \, \text{V} \).This task involves understanding electrochemical cell potentials and the relationship between standard reduction potentials and equilibrium constants. More precise calculations would take into account the influence of the \( K_a \) on the system's \( E' \).

The formal potential is the potential of a half-reaction with respect to a standard hydrogen electrode. It is measured by when the formal concentrations of all the reactants and products are unity and the pH of the solution is 7. Given that: Standard cell potential, Eo = 0.940 V The given reaction is as follows: NO3-aq+3H+aq+2e-⇔HNO2aq+H2Ol The Nernst equation to calculate the potential at 25oC is as follows: E°'=E°-0.0592nlogredox Here, Eo = Standard cell potential n = number of electrons [red] = concentration of reduced species [ox] = concentration of oxidized speciesFor the given reaction the Nernst equation can be written as follows: E°'=E°-0.0592nlogHNO2H2ONO3-H+3 pH of the solution is given by the following expression: pH=-logH+ Rearrange the above expression to calculate H+ ion concentration. H+=10-pH Substitute 7 for pH in the above formula to calculate H+ ion concentration. H+=10-7 MNow substitute 2 for n, 0.940 V for Eo, 10-7 M for [H+], and 1 M for all other concentration terms like [HNO2], [H2O], and [NO3-] in the Nernst equation to calculate the formal potential of the cell. E°'=0.940 V-0.05922log1×11×10-73=0.940 V-0.05922×21 V=0.940 V-0.6216 V=0.3184 V Conclusion: The formal potential for the given reaction is 0.3184 V.

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Chemistry

Calculate the formal potential, Eº, for the given reaction. NO3(aq) + 3H+ (aq) + 2 e¯ ⇒ HNO₂ (aq) + H₂O(1) Nitrous acid, HNO₂, has a K₁ of 7.1 × 10-4. E⁹ 0.845 Incorrect E° = 0.940 V V

Calculate the formal potential, Eº, for the given reaction. NO3(aq) + 3H+ (aq) + 2 e¯ ⇒ HNO₂ (aq) + H₂O(1) Nitrous acid, HNO₂, has a K₁ of 7.1 × 10-4. E⁹ 0.845 Incorrect E° = 0.940 V V

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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