**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.

Science

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...

See similar textbooks

Related questions

Q: Consider the following cell reaction: Mn(s) + 2 H+(? M) Mn2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: According to the question, The cell reaction is as follows, Mn(s) + 2 H+(? M) Mn2+(1.00 M) +…

Q: 2. In another cell, the potential of the copper metal, copper(II) ion electrode was found to be…

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: In the given question we have to calculate the pH of unknown solution, by electrochemical…

Q: Consider the following cell reaction: Fe(s) + 2 H*(? M)→FE²*(1.00 M)+ H2(g)(1.00 atm) - If the cell…

A: Given: A cell reaction: Fes + 2H+?M → Fe2+1.00M + H2g1.00atm Temperature = 298K Cell potential =…

Q: Can you help me solve 19.81?

A: Redox reaction is a simultaneous reduction of one compound and oxidation of another compound.…

Q: 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the…

A: Given reaction: 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g) E∘=0.483 V [Co3+]= 0.896 M [Co2+]= 0.548 M…

Q: Given the following half-reactions, Ag+ (aq) +e → Ag(s) AgCl(s) +e → Ag(s) +Cl-(aq) E° = +0.222 V…

Q: The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.87…

A: Consider the temperature of the system is 298.15 K. The concentration of X+ ion in the cathode…

Q: Consider the following redox reaction: Sn2+ + Sr(s) --> Sn(s) + Sr2+ What is the cell…

A: Given, concentrations of Sn2+ and Sr2+ are 3.5M & 0.05M respectively at temperature 10°C. The…

Q: Cr3+ (1 M) Cr2+ (1 M) T13+ (1 M) T13+ (aq) + 3e-> TI (s) Cr2 (aq) Cr3 (aq) + e- Using the list of…

A: Given reaction : E°cell = +1.14 V Reduction half Reaction takes place at Cathode Tl3+ (aq) + 3 e-…

Q: Determine Ecell∘, ΔG∘, and K for this reaction. Calculate the value for the cell potential, Ecell,…

Q: Calculate the standard cell potential (E∘cell�cell∘) for the reaction…

Q: Calculate the standard potential, ?∘, for this reaction from its equilibrium constant at 298 K.…

A: This question is related thermodynamics. We have to deal with the formulas to arrive at the…

Q: X(s)|X1+ (0.99 M) || Mn O4 1 minus (0.18 M)|Mn2+ (1.90 M)|H+ (2.64 M) The reduction potential for…

A: The reduction potential of X+1 = 0.32vThe reduction potential of MnO4- = 1.51v

Q: HOx is a monoprotic weak acid with an acid dissociation constant of 4.78 × 10-5. H₂ Red² is a…

Q: Consider the following cell reaction: Cd(s) + 2 H+(? M) Cd2+(1.00 M) + H2(g)(1.00 atm) If the cell…

Q: Consider the following cell reaction: Mn(s) + 2 H+(? M) Mn2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: Given data : Mn(s) + 2 H+(_____M) gives Mn2+(1.00 M) + H2(g)(1.00 atm)the cell potential (E cell…

Q: A silver metal electrode is immersed into an AgNO3 Solution. A potential value of 0.734 V is…

A: Electrode potential is the electromotive force for the galvanic cell developed from a standard…

Q: X(s)|X1+ (0.99 M) || Mn O4 1 minus (0.18 M)|Mn2+ (1.90 M)|H+ (2.64 M) The reduction potential for…

Q: Consider the following cell reaction: Cd(s) + 2 H*(? M) Ca2*(1.00 M) +H>(g)(1.00 atm) If the cell…

A: The cell reaction given is, Given: Cell potential = 0.186 V. And temperature = 298 K

Q: For the reaction 2Co 3+(aq)+2Cl -(aq)→2Co 2+(aq)+Cl 2(g) E∘=0.483 V what is the cell…

A: P ( Cl2 ) = 4.10 atm P V = n R T P = ( n/ V ) R T = c R T c = P / R T T ( temperature ) = 25…

Q: Use standard reduction potentials to find the equilibrium constant for the following reaction at 25…

A: Standard reduction potential is defined as the tendency of a chemical species to be reduced and this…

Q: Which of the following is not true of standard reduction potential? Select the correct answer below:…

A: The standard reduction potential is a measure of the tendency of a chemical species to acquire…

Q: Pt(s) | V³+ (aq, 0.210 M), V²+ (aq, 0.00600 M) || S.H.E. Ecell = V E√³+√√2+ = -0.255 V The Pt…

Q: X(s)|X4+ (2.75 M) || Mn O4 1 minus (2.58 M)|Mn2+ (2.75 M)|H+ (0.30 M) The reduction potential for…

A: According to the cell diagram given,Anode is at left side to salt bridge and cathode is at right…

Q: What is the potential of a cell at 25oC for which the reaction below applies, if the molar…

A: Answer:- This question is answered by using the simple concept of calculation of potential of cell…

Q: K Given: Br2 (1) +2e 12 (s) + 2e O -1.63 V O -0.55 V O 0.55 V What is the standard cell potential…

Q: The enzyme hydrogenase carries out the reduction of hydronium ions to molecular hydrogen: 2H3O++…

A: The given reaction is:

Q: The standard potential for the reaction below is -0.308 V at 25°C. 3 Y+2 (aq) +2 X (s) → 3 Y (s) +…

Q: If the coefficients of a balanced reaction are all multiplied by 2, the cell potential is also twice…

A: Given that we have to multiply the coefficient of a cell reaction with 2.

Q: Consider the following cell reaction: Zn(s) + 2 H*(? M) —>Zn²+ (1.00 M) + H2(g)(1.00 atm) If the…

A: Answer:Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical…

Q: The cell potential was 0.151 V at 25oC and a Ni2+(aq) concentration of 0.153 M. What was the pH of…

A: Given: Ecell = 0.151 V Eocell =0.2600 V R = 8.314 J/mole K T =25oC=298K Faraday's constant , F =…

Q: Consider the following cell reaction: Mn(s) + 2 H*(? M) –→MN2*(1.00 M) + H2(g)(1.00 atm) If the cell…

Q: An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a.…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

**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 \( E' \).

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Trending now

This is a popular solution!

Step by step

Solved in 6 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

HOx is a monoprotic weak acid with an acid dissociation constant of 3.00 × 10¯5. H₂Red²¯ is a diprotic weak acid with acid dissociation constants of 3.80 × 10−4 and 3.72 × 10-8. For the half reaction shown, calculate the standard reduction potential, Eº, at 25 °C. HOX(aq) + 2 e E = 0.00996 Incorrect H₂Red² (aq) E' = 0.0431 V V
Give the standard line notation for each cell. (a) 2 IO3(aq) + 10 Fe²+ (aq) + 10 H+ (aq) 10 Fe³+ (aq) + I₂ (aq) + 5 H₂O(1) Pt(s) | Fe³+ (aq), I₂ (aq) || Fe²+ (aq), IO3¯(aq), H+ (aq) | Pt(s) Pt(s) | Fe²+ (aq), Fe³+ (aq) || IO3(aq), H+ (aq), I₂ (aq) | Pt(s) Pt(s) | IO3(aq), H+ (aq), I₂ (aq) || Fe²+ (aq), Fe³+ (aq) | Pt(s) Pt(s) | Fe²+ (aq), IO3¯¯(aq), H+ (aq) || Fe³+ (aq), I₂ (aq) | Pt(s) (b) (c) (d) Zn(s) + 2 Ag+ (aq) = Zn²+ (aq) + 2 Ag(s) Ag(s) | Zn²+ (aq) || Ag+ (aq) | Zn(s) Zn(s) | Zn²+ (aq) || Ag+ (aq) | Ag(s) Ag(s) | Ag+ (aq) || Zn²+ (aq) | Zn(s) Zn(s) | Ag+ (aq) || Zn²+ (aq) | Ag(s) H₂O₂ (aq) + 2 H+ (aq) + 2e → 2 H₂O(l) O2(g) + 2 H+ (aq) + 2 e¯ → H₂O₂ (aq) Pt(s) | H₂O₂ (aq) | Pt(s) ○ Pt(s) | O₂(g) | H₂O₂ (aq), H+ (aq) || H₂O₂ (aq), H+ (aq) | Pt(s) Pt(s) | H₂O₂ (aq), H+ (aq) || O₂(g) | H₂O₂ (aq), H+ (aq) | Pt(s) ○ Pt(s) | H₂O₂ (aq) | O₂(g) || H+ (aq) | Pt(s) Mn²+ (aq) + 2 e → Mn(s) Fe³+ (aq) + 3e → Fe(s) Fe(s) | Mn²+ (aq) || Fe³+ (aq) | Mn(s) Mn(s) | Mn²+ (aq) || Fe³+ (aq) | Fe(s)…
The standard potential for the reaction below is -1.036 V at 25°C. 3 Y+ (aq) + X (s) → 3 Y (s) + X+3 (aq) Calculate the value of the equilibrium constant for the reaction at 25°C. [Do not be surprised by very large or very small values. Large or small values should be entered in scientific notation.] Example: 3.40×10-6 = 3.40E-6 Example: 8.22×1020 = 8.22E20 K = Answer
Calculate K (both parts of the question)
Help on these two please
Give the standard line notation for each cell. (a) 2 IO3¯(aq) + 10 Cr²+ (aq) + 10 H+ (aq) ⇒ 10 Cr³+(aq) + I₂ (aq) + 5 H₂O(1) Pt(s) | Cr²+ (aq), IO3¯(aq), H+ (aq) || Cr³+ (aq), I2 (aq) | Pt(s) Pt(s) | Cr³+ (aq), I2 (aq) || Cr²+ (aq), 103¯(aq), H+ (aq) | Pt(s) Pt(s) | IO3¯(aq), H+ (aq), I2 (aq) || Cr²+ (aq), Cr³+ (aq) | Pt(s) Pt(s) | Cr²+ (aq), Cr³+ (aq) || IO3¯¯(aq), H† (aq), I₂ (aq) | Pt(s) (b) (c) (d) Co(s) + 2 Ag+ (aq) ⇒ Co²+ (aq) + 2 Ag(s) Co(s) | Ag+ (aq) || Co²+ (aq) | Ag(s) (aq) || Ag* (aq) | Co(s) Ag(s) | Co²+ 2+ Ag(s) | Ag+ (aq) || Co²+ (aq) | Co(s) 2+ Co(s) | Co²+ (aq) || Ag+ (aq) | Ag(s) H2O2(aq)+2 H*(aq)+2e O₂(g) + 2 H+(aq) + 2 e¯ → H2O2(aq) Pt(s) | H₂O₂ (aq) | 02 (9) || H+ (aq) | Pt(s) Pt(s) | H₂O₂ (aq) | Pt(s) Pt(s) | H₂O2 (aq), H+ (aq) || O2(g) | H₂O₂ (aq), H+ (aq) | Pt(s) Pt(s) | O2(g) | H₂O2 (aq), H† (aq) || H₂O2 (aq), H† (aq) | Pt(s) 00 Mn²+ (aq) + 2 e → Mn(s) → 2H,O(l) 3+ Fe³+ (aq) + 3 e → Fe(s) Eº E° -1.18 V 3+ Fe(s) | Fe³+ (aq) || Mn²+ (aq) | Mn(s) Fe(s) | Mn²+ (aq)…
The cell potential was 1.271 V at 25oC and a Al3+(aq) concentration of 0.178 M. What was the hydronium ion concentration? The H2(g) pressure was 1 atm at 25oC.6H+(aq) + 2Al(s) ↔ 2Al3+(aq) + 3H2(g) Ecoell = 1.660 V
Calculate the potential for each cell as written at 25 ∘C.25 ∘C. Indicate whether the metal electrode in the half‑reaction opposite the standard hydrogen electrode, S.H.E., would be the anode or the cathode if the cell was shorted and electrons were allowed to flow freely. S.H.E.‖‖Zn2+(aq,0.0570 M)||Zn(s)?∘Zn2+/Zn=−0.762 V
Consider the following cell reaction: Ni(s) + 2 H*(? M). Ni?*(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.118 volts, what is the pH of the hydrogen electrode? pH =
The standard cell potential for the reaction shown here is .653 V. Calculate the cell potential at 25°C with [Hg^2+] = 0.0500 M, [V^2+] = 0.100 M, [Hg2^2+] = 0.00500 M and [V^3+] = %3D 0.0200 M. [Hg?+] do.o500 M [V2+] = 0.100 M H0.0500 M [Hg* = 0.00500 M [V³*] = 0.0200 M 2 Hg²+ (aq) + 2 V²+ (aq) = Hg2²+ (aq) + 2 V³+ (aq)