Using the values from the table of standard reduction potentials, calculate the cell potentials ofthe following cells:(a) Ga(s) | Ga³"(aq) || Ag*(aq) | Ag(s)(b) Zn(s) | Zn²-(aq) | Cr**(aq) | Cr(s)(c) Fe(s), FeS(3) | S² (aq) | Sn²*(aq) | Sn(s)Calculate the standard free energy change of the following reactions using the standard cellpotentials for the half reactions that are involved:(a) Fe(s) + Hg;*"(aq) →F²²*(aq) + 2 Hg(4)(b) Fe*"(aq) + Ag(s) + CI (aq) → Fe²"(aq) + AgC(s)Use the Nernst equation to calculate the cell potential of the given cell at 298K:12 Ag"(aq)(0.50 M) + Ni(s) → 2 Ag(s) + Ni²^(aq)(0.20 M)Write the equilibrium expressions for each of the following reactions:(a) CaCO,(s) 2C2²*(aq) + CO,²-(aq)(b) Mg;(PO4);(s) 23 Mg²*(aq) + 2 PO,"(aq)(c) CO(g) + NO;(g)=C0;(g) + NO(g)Which of the following is more likely to precipitate the sulfate ion?(a) PbSO4(9) Pb²*(aq) + SO,²"(aq) K= 1.8 × 10(b) CASO,(s) #Ca²*(aq) + SO,²-(aq) K=9.1 × 10-6

Ga/Ga+3∥Ag+/AgE0Ga+3/Ga=-0.56 V (anode)E0Ag+/Ag=+0.80 V (cathode)E0cell =E0c-E0A=0.80-(-0.56) =+1.36…

Using the values from the table of standard reduction potentials, calculate the cell potentials of the following cells: (a) Ga(s) | Ga³"(aq) || Ag*(aq) | Ag(s) (b) Zn(s) | Zn²“(aq) | Cr*(aq) | Cr(s) (c) Fe(s), FeS(s) | S²-(aq) || Sn²*(aq) | Sn(s)

Using the values from the table of standard reduction potentials, calculate the cell potentials of the following cells: (a) Ga(s) | Ga³"(aq) || Ag(aq) | Ag(s) (b) Zn(s) | Zn²“(aq) | Cr(aq) | Cr(s) (c) Fe(s), FeS(s) | S²-(aq) || Sn²*(aq) | Sn(s)

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: What is the cell reaction for the voltaic cell Cr(s) | Cr3*(aq) I|| CI- (aq) | Cl2(g) | Pt? O Cr(s)…

A: We have to predict the correct cell reaction.

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

A: In electrochemical cell , the value of potential difference between two electrodes is known as cell…

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au³*(aq) = Fe*(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: For the cell shown, the measured cell potential, Ecell, is –0.3613 V at 25 °C. Pt(s) | H,(g, 0.771…

A: This question can be solved using Nernst equation. Please refer to the attached picture for the full…

Q: Given the standard cell potential, E°ce = 1.10 V, for the cell, Zn(s) | Zn(NO,)(aq) || Cu(NO,)(aq) |…

A: Standard cell potential (E°cell) = 1.10 V Temperature = 25°C. The reaction : Zn(s) + Cu2+(aq)…

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: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: The point should be kept in mind while solving this problem, If the value of ΔGo is positive then…

Q: Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is…

A: Given : Table of half reactions and reduction potential. To find: Complete the given table.…

Q: =

A: Given: Sn | Sn2+ (aq) =−0.140 V Pb | Pb2+(aq) =−0.126 V, T= 298 K

Q: For the cell shown, the measured cell potential, ?cell, is −0.3681 V at 25 °C. Pt(s) |…

Q: Calculate the standard cell potential at 25°C for the following cell reaction from standard free…

A: The question contains more than one question so only the first one is solved here, if the other one…

Q: Predict the standard potential for the galvanic cell. Refer to the table of standard reduction…

Q: 4. The cell potentials of many oxidation-reduction reactions are highly dependent on pH. Consider…

A: The question is based on the concept of electrochemistry. we need to calculate standard cell…

Q: Calculate K for scandium fluoride, SCF3, given that the cell potential at 25 °C for the following…

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

A: We have tp Calculate the standards potential value for the following cell reaction…

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

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

Q: Calculate the cell potential of the concentration cell described by Ag(s)|Ag⁺(aq, 0.25 M)||Ag⁺(aq,…

A: For concentration cell , Eocell = 0 and Ecell = -0.0591/n log[product]/[reactant]

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: The cell potential of the following electrochemical cell is determined by using an unspecified…

A: We have find out the answer.

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

Q: Calculate the maximum work available from 20.0 g of aluminum in the following cell when the cell…

A: Electric work is product of charge passed through electric cell and cell potential. So, electrical…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3621 V at 25 °C. Pt(s) | H₂(g, 0.765…

A: Answer: This question is based on Nernst equation which is shown below: Ecell=Ecell0-0.0592nlogQ…

Q: Consider these metal ion/metal standard reduction potentials Cd2+ (aq)| Cd(s): -0.40 V; Zn2+ (aq)|…

Q: Consider the following electrochemical cell:…

A: In electrochemical cell redox reaction occur

Q: For the cell shown, the measured cell potential, ?cell, is −0.3553 V at 25 °C. Pt(s) |…

Q: [References] Using values from the table of standard reduction potentials, calculate the cell…

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

Q: Consider the cell diagram for an electrochemical cell: Pt | Ti2+(aq), Ti3+(aq) || Br2(g), Br-(aq) |…

A: For the electrochemical cell: Pt | Ti2+(aq), Ti3+(aq) || Br2(g), Br-(aq) | Pt having E = 1.40 V , we…

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

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au³+(aq) =…

Q: 1) The standard reduction potentials of Cu2+ (aq) Cu(s) and Ag+ (aq) Ag(s) are +0.34 and +0.80 V,…

A: Calculate the cell potential of the given galvanic cell. Given At Anode Cu/Cu2+; E°=-0.34 V At…

Q: Calculate the cell potential for the galvanic cell in which the reaction Al(s)+Au3+(aq)↽−−⇀…

A: Cell potential of a galvanic cell can be calculated using nernst equation

Q: The condensed cell diagram for the reaction occurring in silver–zinc button batteries is (-) Zn(s)…

A: This question belongs to Electrochemistry. The condensed cell diagram for the reaction occurring in…

Q: Which of the following cells is most likely to be an example of a galvanic cell? Zn(s) | Zn2+ ||…

Q: The condensed cell diagram for the reaction occurring in silver–zinc button batteries is (-) Zn(s)…

A: The cell diagram for the reaction is (-) Zn(s) | ZnO(s) | KOH(aq) || Ag2O(s) | Ag(s) (+) The…

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: 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: For the cell shown, the measured cell potential, Ecell, is -0.3537 V at 25 °C. Pt(s) | H₂(g, 0.837…

A: Cell potential, Ecell= -0.3537 VHalf-cell reactions are also given.

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

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

Using the values from the table of standard reduction potentials, calculate the cell potentials of
the following cells:
(a) Ga(s) | Ga³"(aq) || Ag*(aq) | Ag(s)
(b) Zn(s) | Zn²-(aq) | Cr**(aq) | Cr(s)
(c) Fe(s), FeS(3) | S² (aq) | Sn²*(aq) | Sn(s)
Calculate the standard free energy change of the following reactions using the standard cell
potentials for the half reactions that are involved:
(a) Fe(s) + Hg;*"(aq) →F²²*(aq) + 2 Hg(4)
(b) Fe*"(aq) + Ag(s) + CI (aq) → Fe²"(aq) + AgC(s)
Use the Nernst equation to calculate the cell potential of the given cell at 298K:
12 Ag"(aq)(0.50 M) + Ni(s) → 2 Ag(s) + Ni²^(aq)(0.20 M)
Write the equilibrium expressions for each of the following reactions:
(a) CaCO,(s) 2C2²*(aq) + CO,²-(aq)
(b) Mg;(PO4);(s) 23 Mg²*(aq) + 2 PO,"(aq)
(c) CO(g) + NO;(g)=C0;(g) + NO(g)
Which of the following is more likely to precipitate the sulfate ion?
(a) PbSO4(9) Pb²*(aq) + SO,²"(aq) K= 1.8 × 10
(b) CASO,(s) #Ca²*(aq) + SO,²-(aq) K=9.1 × 10-6

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 Que. 1 part (a)

VIEW

Step 2 Que. 1 part (b)

VIEW

Step 3 Que. 1 part (c)

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

Using these metal ion/metal reaction potentials Cu2+(aq)|Cu(s) Ag+(aq)|Ag(s) Co2+(aq)|Co(s) Zn2+(aq)|Zn(s) +0.34 V +0.80 V -0.28 V -0.76 V Calculate the standard cell potential for the cell whose reaction is Co(s) + Cu2+(aq) → Co2+(aq) + Cu(s)
For the cell shown, the measured cell potential, Ecell, is -0.3651 V at 25 °C. Pt(s) | H₂(g, 0.797 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, Eº, are 2 H+ (aq) + 2 e- → H₂(g) Cd²+ (aq) + 2e → Cd(s) Calculate the H+ concentration. [H+] = x10 TOOLS - Eº = 0.00 V Eº = -0.403 V M
The cell potential of the following cell is determined using an unspecified concentration of acid. What is [H*]given that the measured cell potential is -0.366 V and the anode reduction potential (E°) is 0.222 V at 25°C? Ag(s) | AGCI(s) | CI(1.0 M) || H*(aq, ? M) | H2(g, 1.0 atm) | Pt(s) 4.9 x 10-5 M 3.7x 10-3 M O 6.1x 10-2 M
4. Write the overall net ionic equations for the following voltaic cells: (a) Zn(s)|Zn²"(aq)||Fe²*(aq)|Fe(s): (b) Zn(s)|Zn**(aq)||Fe**,Fe²*(aq)|C(s); (C = graphite is not involved in the reaction)
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
Calculate the cell potential for the galvanic cell in which the reaction Al(s) + Au³(aq) Al³(aq) + Au(s) occurs at 25 °C, given that [A1³] = 0.00140 M and [Au³+] = 0.848 M. Refer to the table of standard reduction potentials. E=
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
calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C Fe(s) | Fe3+ (aq, 0.0011M) || Fe3+(aq, 2.33M) | Fe(s)
A galvanic cell whose cell reaction is 2Fe3+(aq) + Zn(s) → 2Fe2+(aq) + Zn2+(aq) has acell potential of 0.72V. What is the maximum electrical work that can be obtained fromthis cell per mole of iron(III) ion?
Calculate the standard cell potential for the following galvanic cell. Ni(s)Ni(NO3)>(aq)||A9NO3(aq)|Ag(s)
3. Calculate the standard potentials for each of the cells at 298 K. Is each combination spontaneous as written? (a) Ag (s) | Ag + (aq) || Au *3 (aq) | Au (s) (b) Cu (s) | Cu +2 (aq) || Al *3 (aq) | Al (s)
Write a balanced equation for the overall cell reaction in the following galvanic cell and tell why inert electrodes are required at the anode and cathode. Pt(s) | Br (aq) | Br₂ (1) || Cl; (g) | Cl(aq) | Pt(s)