Calculate the standard cell potential of the following cell at 25°C: Pb(s) | Pb?+ (ag) || Cu2+ (ag) | Cu(s) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E" (V) Zn2+ (aq) + 2e Zn(s) -0.76 Fe2+ (aq) + 2e Fe(s) -0.41 Cd+ (ag) + 2e - Cd(s) -0.40 Sn2+ (ag)+2e Sn(s) -0.14 Pb?+ (ag) + 2e- Pb(s) -0.13 Fe+ (ag) + 3e - Fe(s) -0.04 Snt (ag) + 2e - Sn2+ (aq) 0.15 Cu+ (ag) + e - Cu* (ag) 0.16 Cu2+ (aq) + 2e Cu(s) 0.34 Standard cell potential = V

Calculate the standard cell potential of the following cell at 25°C: Pb(s) | Pb?+ (ag) || Cu2+ (ag) | Cu(s) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E" (V) Zn2+ (aq) + 2e Zn(s) -0.76 Fe2+ (aq) + 2e Fe(s) -0.41 Cd+ (ag) + 2e - Cd(s) -0.40 Sn2+ (ag)+2e Sn(s) -0.14 Pb?+ (ag) + 2e- Pb(s) -0.13 Fe+ (ag) + 3e - Fe(s) -0.04 Snt (ag) + 2e - Sn2+ (aq) 0.15 Cu+ (ag) + e - Cu* (ag) 0.16 Cu2+ (aq) + 2e Cu(s) 0.34 Standard cell potential = 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: For the cell reaction, Zn(s) | Zn2+(aq, 1 M) || Cu2+(aq, 1 M) | Cu(s), the electrode potential of…

A: In the given question we have to calculate the cell potential. cell Reaction, Zn(s) + Cu2+(aq)…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3559 V at 25 °C. Pt(s) | H₂(g, 0.767…

Q: The standard cell potential for the following galvanic cell is 0.390 V. What is the cell potential…

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: andard potentials given in the appendices s for the following reactions: Cu(s) +2Ag*(aq) Cu2*…

A: In an electrochemical cell, the standard cell potential can be calculated by using the following…

Q: The standard cell potential for the following galvanic cell is 0.390 V. What is the cell potential…

A: Given: Temperature = 325 K Eocell = 0.390 V Concentration of Sc+3 = 0.077 M Concentration of Ti+2 =…

Q: The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g)…

A: Ni(s) + 2 H+(aq) ⇔ Ni+2(aq) + H2 (g) Ecello = 0.23…

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: ) Determine the cell potential, Eo, for an electrochemical cell described by the following cell…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3657 V at 25 °C. Pt(s) | H₂(g, 0.777…

A: Ecell = 0.3657 V PH2 = 0.777 atm The balanced reduction half reactions 2 H+ (aq) + 2 e- ----->…

Q: Give the standard line notation for each cell. (a) 2103 (ад) + 10 Fe2+ (ag) + 10 H* (aд) — 10 Fest…

Q: Calculate the standard Gibbs energy in kJ/mol change for the following voltaic cell A(s) | A3+(aq)…

Q: 11.)

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

Q: For the cell shown, the measured cell potential, ?cellEcell, is −0.3669 V at 25 °C. Pt(s) |…

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

A: a.)

Q: For the cell shown, the measured cell potential, Ecell, is -0.3725 V at 25 °C. Pt(s) | H₂(g,0.849…

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

Q: Gibbs energy change, A;G°, is related to cell potential, Eel, by the equation A;G° = -nFEl Part B…

A: The given reaction is as follows: Xs+2Y+(aq) → X2+(aq) + 2Y(s) ∆rG° of the reaction can be…

Q: For the cell shown, the measured cell potential, Ecell, is –0.3525 V at 25 °C. Pt(s) | H,(g, 0.851…

A: The cell given is, Given: Ecell = -0.3525 V Temperature = 25 oC And the half-reactions are,

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

A: Standard reduction potential of nickel = -0.257 V Standard reduction potential of silver = 0.7996 V…

Q: where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as…

A: Standard cell potential (Eo) is the EMF of the cell when the concentrations of electrolytes is 1M ,…

Q: Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard…

A: The process of breaking the electrolyte by applying an electric charge to its constituent ions is…

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

Q: For the cell shown, the measured cell potential, Ecell, is -0.3521 V at 25 °C. Pt(s) | H,(g, 0.785…

Question

Calculate the standard cell potential of the following cell at 25°C:
Pb(s) | Pb?+ (ag) || Cu²+ (ag) | Cu(s)
Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C
Cathode (Reduction)
Standard
Half-Reaction
Potential, E (V)
Zn2+ (aq) + 2e - Zn(s)
-0.76
Fe2+ (aq) + 2e Fe(s)
-0.41
Cd?+ (ag) + 2e - Cd(s)
-0.40
Sn2+
(ag) + 2e Sn(s)
-0.14
Pb?+ (ag) + 2e Pb(s)
-0.13
Fet (ag) + 3e Fe(s)
-0.04
Sn+ (aq) + 2e- - Sn+ (ag)
0.15
Cu+ (ag) +e Cut (ag)
0.16
Cu?+ (ag) + 2e - Cu(s)
0.34
Standard cell potential
V

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

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

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
7
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
For the cell shown, the measured cell potential, Ecell, is -0.3619 V at 25 °C. Pt(s) | H₂(g, 0.721 atm) | H¹ (aq, ? M) || Cd²+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2 e H₂(g) Eº = 0.00 V Cd²+ (aq) + 2e → Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+] = TOOLS x10 M
Prepare a sketch and write the half-reactions and overall cell reaction for the electrochemical cell designated by: Pt(s) | Ag(s) |AgCl(s) | Cl-(a = 1) | Cl2(g, 1 bar)| C(graphite) | Pt(s)
+|| 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
For the cell shown, the measured cell potential, Ecell, is −0.3627 V at 25 °C. Pt(s) | H2(g,0.735 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, ?o, are 2H+(aq)+2e−⟶H2(g) ?o=0.00 V Cd2+(aq)+2e−⟶Cd(s) ?o=−0.403 V Calculate the H+ concentration in M.