**Topic: Calculation of Actual Cell Potential Using the Nernst Equation**Given the following overall reaction, standard cell potential ($E^\circ_{\text{cell}}$), concentrations, and temperature; use the Nernst equation to calculate the actual cell potential ($E_{\text{cell}}$).**Reaction:**\[ \text{A}^{2+}_{(aq)} + 2 \text{B}_{(s)} \rightarrow \text{A}_{(s)} + 2 \text{B}^{+}_{(aq)} \]- Standard Cell Potential, $E^\circ_{\text{cell}} = 0.775 \, \text{V}$- Concentration of $\text{A}^{2+}_{(aq)} = 0.308 \, \text{M}$- Concentration of $\text{B}^{+}_{(aq)} = 1.833 \, \text{M}$- Temperature = $16.76^\circ \text{C}$Constants:- $R = 8.314462 \, \text{J/K} \cdot \text{mol}$- $F = 96,485.34 \, \text{C/mol e}^-$**Instructions for Answer Submission:**- Enter the number only (no units).- Do not leave any spaces.- Use a leading zero before the decimal when necessary.- Report your number to 3 decimal places (regardless of the significant figures).- Correctly round your answer to the 3rd decimal place (margin of allowed error is only $\pm 0.001$, so always use un-rounded numbers in your calculations).**Examples:**- $0.123$ or $9.876$

Answered: Image /qna-images/answer/7484998f-9f8b-49ca-bcdd-9a7514a54730.jpg

Given the following overall reaction, standard cell potential (E°cell), concentrations, and temperature; use the Nernst equation to calculate the actual cell potential (Ecell). 424 + 2 B(s) As) + 2 B*(aq) E°cell = 0.775 V %3D Conc. A2*a0) = 0.308 MA²+ %3D Conc. B"(aq) = 1.833 MB* Temperature = 16.76 °C %3D R = 8.314462 J/K-mol F = 96,485.34 C/mol e

Given the following overall reaction, standard cell potential (E°cell), concentrations, and temperature; use the Nernst equation to calculate the actual cell potential (Ecell). 424 + 2 B(s) As) + 2 B(aq) E°cell = 0.775 V %3D Conc. A2a0) = 0.308 MA²+ %3D Conc. B"(aq) = 1.833 MB* Temperature = 16.76 °C %3D R = 8.314462 J/K-mol F = 96,485.34 C/mol e

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: Which of the following electrochemical cells requires an inert electrode? Sn4+ (aq) |Sn²+ (aq) || Zn…

A: Inert electrodes: They don't take part in electrochemical reaction. They provide there interface or…

Q: Consider the cell Zn(s)|ZnCl2(0.005 mol kg-1)|Hg2Cl2(s)|Hg(l), for which the cell reaction is…

Q: Consider the cell: Pt(s) | H2(g, 0.100 bar) | H+(aq, pH = 2.54) || Cl−(aq, 0.200 M) | Hg2Cl2(s) |…

Q: In the standard electrochemical cell, Pt(s)|H2SO3laq), H*(aq), SO4 (aq)||Ag*(aq)|Ag(s), v¥hat can be…

A: In a electrochemical cell representation RHS is cathode s reduction all happen over there, LHS in…

Q: Consider the following data for the cell: Pt(s) |H2(g)| HBr(aq,b)|AgBr(s) |Ag(s), taking place at…

A: ### Step 1: Use Nernst Equation to Determine Standard Cell PotentialThe cell potential (E_cell) at…

Q: In the temperature range 0-90 ºC , the potential difference of the following cell: Pt (s) | H2 (g, f…

Q: A Cr(s) | Cr(aq)|| Fe*(aq) | Fe(s) galvanic cell has a standard cell potential of 0.700 V. Calculate…

A: We have find out the ∆G and maximum amount of work done by the cell on the surrounding.

Q: Consider the voltaic cell H+(aq, ?? M)|H2(g, 1 atm)||Cu(s)|Cu2+(aq. 0.1 M). The measured Ecell for…

A: Given that, the voltaic cell H+(aq, ?? M)|H2(g, 1 atm)||Cu(s)|Cu2+(aq. 0.1 M). So, [Cu2+] = 0.1 M,…

Q: SVhat is the cell potential (Ecl) of a spontaneous cell that is run at 25°C and contains Cr*| = 0.10…

A: To calculate Ecell use Nernst equation: where, Q = reaction quotient

Q: The standard cell potential for the reaction provided below is-2.431V, calculate the cell potential…

Q: The cell potential of the following electrochemical cell depends on the pH of the solution in the…

A: The question is based on the concept of redox reactions reactions. Reactions in which simultaneous…

Q: The standard reduction potential of the zinc cation is -0.76 V. The measured cell potential for the…

Q: Tempjetes Symbo Gibbs energy change, ArG", is related to cell potential, Ee. by the equation A,G" =…

A: Part A: Answer: ∆rG° = -372 kJ/mol

Q: 11.)

A: We have given that From representation of the cell reaction Oxidation half reaction : Zn(s)…

Q: Calculate the cell potential at 25°C for the reaction Fe(s)| Fe^3+ (aq,0.0952 M)|| C12(g,7.62 atm)…

A: Given -> T = 25°C Fe(s)/Fe3+(aq,0.0952M)//Cl2(g,7.62atm)/Cl-(aq,0.0577M)/pt(s) E°cell = 1.396 V…

Q: The cell potential E for the cell Pt(s) H2(g, =1.00) H (aq, =1.00)| NaCI(aq, 0.100 m) AgC(s) Ag(s)…

A: .

Q: Calculate the potential (emf) of a working galvanic cell that is based on these two half cells and…

A: Given: Cr3+(aq) → Cr2+(aq) E°(Cr3+/Cr2+) = −0.40 V IO−(aq) → I2(aq) E°(…

Q: The standard cell potential of a Daniell cell, with cell reactionZn(s) + Cu2+(aq) → Zn2+(aq) +…

A: Given, a Daniell cell with the cell reaction as follows,Zn(s)+Cu2+→Zn2++Cu(s)the standard cell…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: a.)

Q: Gibbs energy change, A:G®, is related to cell potential, E, by the equation Calculate the standard…

A: For the given cell, change in enthalpy and entropy at 25oC is as follows: ∆rHo = -729 kJ mol-1∆rSo =…

Q: The standard Gibbs energy change for the following voltaic cell Cu(s) | Cu2+(aq) || Ag+(aq) | Ag (s)…

Q: The measured cell potential, Ecell, for the cell shown is –0.3549 V at 25 °C. Calculate the Ht…

A: Given: E∘cell is -0.3549 V. H2→2H+aq+ 2e- Eo=0.00 V Cd2+aq+ 2e-→Cds Eo=-0.403 V…

Q: Zn cation has 0.76 V as it's standard reduction potential.the cell potential is measured for the…

A: 0.0203 mol/L

Q: The standard reduction potential of the zinc cation is -0.76 V. The measured cell potential for the…

Q: The net ionic cell reaction for the 'Bunsen cell ' is Zn(s) +2 NO3-(aq) + 4 H+(aq) → Zn2+(aq) + 2…

Q: An aqueous sodium chloride solution is electrolyzed using a current of 4.42 A. How much time (min)…

A: An aqueous sodium chloride solution is electrolyzed using a current of 4.42 A. How much time (min)…

Q: For the reaction 2Co3+(aq)+2Cl(aq)->2Co2+(aq)+C12(g). Eocell=0.46 V what is the cell potential at 25…

A: Answer:Value of cell potential at 298.15K temperature is:Here:n is equal to number of electrons…

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

100%

**Topic: Calculation of Actual Cell Potential Using the Nernst Equation**

Given the following overall reaction, standard cell potential ($E^\circ_{\text{cell}}$), concentrations, and temperature; use the Nernst equation to calculate the actual cell potential ($E_{\text{cell}}$).

**Reaction:**
\[ \text{A}^{2+}_{(aq)} + 2 \text{B}_{(s)} \rightarrow \text{A}_{(s)} + 2 \text{B}^{+}_{(aq)} \]

- Standard Cell Potential, $E^\circ_{\text{cell}} = 0.775 \, \text{V}$
- Concentration of $\text{A}^{2+}_{(aq)} = 0.308 \, \text{M}$
- Concentration of $\text{B}^{+}_{(aq)} = 1.833 \, \text{M}$
- Temperature = $16.76^\circ \text{C}$

Constants:
- $R = 8.314462 \, \text{J/K} \cdot \text{mol}$
- $F = 96,485.34 \, \text{C/mol e}^-$

**Instructions for Answer Submission:**

- Enter the number only (no units).
- Do not leave any spaces.
- Use a leading zero before the decimal when necessary.
- Report your number to 3 decimal places (regardless of the significant figures).
- Correctly round your answer to the 3rd decimal place (margin of allowed error is only $\pm 0.001$, so always use un-rounded numbers in your calculations).

**Examples:**
- $0.123$ or $9.876$

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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

The standard cell potential for the reactions Sn(s) + CuSO4(aq) → Cu(s) + SnSO4(aq) at 25 °C exceeds +0.20V
A galvanic cell Mn(s)|Mn2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Mn electrode that weighs 34.9 g and a Pb electrode immersed in 532 mL of 1.00 M Pb2+(ag) solution. A steady current of 0.0519 A is drawn from the cell as the electrons move from the Mn electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Pb electrode gained when the cell is completely discharged? g (d) What is the concentration of the Pb2+(aq) when the cell is completely discharged? (Assume that the limiting reactant is 100% reacted.) M
Like equilibrium constants, E values are temperature dependent. At 80°C, E for the cell cell cell diagram shown is 0.18 V. Pt | H₂(g) | HCl(aq) || AgCl(s) | Ag(s) The corresponding cell reaction is H₂(g) + 2AgCl(s) + 2Ag(s) + 2H¹ (aq) + 2C1 (aq) Calculate the equilibrium constant for this reaction at 80°C. x 10 (Enter your answer in scientific notation).
Consider the following cell. Ag(s)|AgCI(s)|NaCI(aq)|Hg2Cl2(s)|Hg(/)|Pt(s) (a) Write the half-cell reactions. (Include states-of-matter under the given conditions in your answer.) Cathode: chemPad Help Greek - Anode: chemPad O Help X.X"| Greek - (b) The standard emfs of the cell at several temperatures are as follows. T/K 291 298 303 311 E°/mV 43.0 45.4 47.1 50.1 Calculate the values of A,G°, A,Sº, and A,H° for the reaction at 303 K. A,G°: A,S° kJ•mol-1 J-mol -1.к-1 %3D A,H° kJ•mol-1
Gibbs energy change, A-G", is related to cell potential, E. by the equation A,G nFE Part A where n is the number of moles of electrons transferred and F = 96 500 C mo]1 is the Faraday's constant. Calculate the standard Gibbs energy change at 25 °C for the following reaction: Mg(s) + Fe" (ag) »Mg+ (ag) + Fe(s) Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? kJ A,G = 380.20 mol- Submit Previous Answers
+|| Σ D. For the cell shown, the measured cell potential, Ecell, is-0.3621 V at 25 °C. Pt(s) | H, (g, 0.853 atm) | H* (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2H*(aq) + 2 e¯ – H, (g) A 00'0 = 07 24, Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V %3D Calculate the Ht concentration. M. = [,H] 10:23 AM M. 11/9/2021 7734 F4 F5 F7 F8 F10 F11 F12 PrtScr Insert Delete Eゴ #3 Backspace 2$ ) 4. 5. 9. 7. R } 1 Enter F. K. H. Sh
3. At 298 K, the EMF of the cell shown below is +0.84 V. Pt(s)|Fe²*(aq, a = 1), Fe³*(aq, 1)|| Ce**(aq, a = 1), Ce³*(aq, a = 1)|Pt(s) a = (i) Define what is meant by the standard EMF of the cell. (ii) Write down the cell reaction and the Nernst equation for the cell. (iii) Calculate the equilibrium constant for the cell reaction at 298 K.