Calculate AG° and the equilibrium constant for the following reaction at 298 K:Zn*(aq) + Ni(s) → Zn(s) + Ni²*(aq)Acidic SolutionStandard Electrode Potential, E (volts)H2O2(aq) + 2 H'(aq) + 2 eAu*(aq) + e- Au(s)Au (aq) + 3 e- Au(s)Br2(8) +2 e-→2 Br(aq)NO: (aq) + 4 H'(aq) + 3 e NO(g) + 2 H20Agʻ(aq) + e Ag(s)Hg2"(aq) + 2 eFe (aq) + e-- Fe2"(aq)Cu2*(aq) + 2 e Cu(s)HgzClz(s) + 2 e →2 Hg(t) + 2 C(aq)Sn(aq) + 2e Sn2 (aq)2 H*(aq) + 2 e → Hz(g)Pb2*(aq) + 2 e Pb(s)Sn2"(aq) + 2 e Sn(s)Ni (aq) + 2 e → Ni(s)Cd2*(aq) + 2 e Cd(s)Cr (aq) + e - Cr*(aq)Fe2 (aq) + 2 e →Fe(s)Zn2*(aq) + 2 e Zn(s)Cr2*( aq) + 2 e Cr(s)Al3 (aq) + 3 e →Al(s)Mg2 (aq) + 2 e Mg(s)2 H20({)+1.77+1.68+1.50+1.08+0.96+0.802 Hg(8)+0.789+0.77+0.337+0.27+0.15 .0.00-0.126-0.14-0.25-0.40-0.408-0.44-0.763-0.91-1.66-2.37AG° =JK =

Science

Chemistry

Calculate AG° and the equilibrium constant for the following reaction at 298 K: 2+ Zn*(aq) + Ni(s) → Zn(s) + Ni²*(aq)

Calculate AG° and the equilibrium constant for the following reaction at 298 K: 2+ Zn(aq) + Ni(s) → Zn(s) + Ni²(aq)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 160MP

See similar textbooks

Related questions

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr³+ (aq) +…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu²* (aq)+…

A: The reaction given is, Cu2+aq+Zns→Cus+Zn2+aq Cu2+ is being reduced to Cu and Zn is being oxidised to…

Q: (a) Balance the following simple redox reaction. Fe (s) + O2(g) + 2H2O (l) → Fe3+ + 4 OH- (3) (b) If…

A: Redox reaction : it is the reaction where oxidation and reduction are occurred simultaneously . the…

Q: Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these…

A: Note: Since you have posted a question with multiple subparts, we will solve the first three…

Q: The standard cell potential for the reaction: A (s) + B2* (aq) = A2* (aq) + B (s) is - 0.371 V. What…

Q: How long in seconds would it take to deposit 59.07 g of Pt from an aqueous solution of Pt 2+ with a…

Q: A galvanic cell consists of a cathode with a nickel electrode in a 0.186 M solution of Ni(NO3)2 and…

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: How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous…

A: The balanced chemical equation for the reduction of copper is: Thus, for the production of 1 mole…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized…

A: electrochemical cell is a device which generates electrical energy from chemical emery , in…

Q: Write the cell diagram for a galvanic cell consisting of an Al electrode placed in a 1 M Al(NO3)3…

A: Given:- Al electrode placed in IM AlNO33 solution Ag electrode placed in IM…

Q: Use cell potential to calculate an equilibrium constant. Calculate the cell potential and the…

Q: The equilibrium constant for the reaction Zn(s) + Fe2+(aq)⇌ Zn2+(aq) + Fe(s) is 6.66 x 1010 at 25…

Q: The reaction Sn (s) + 2 Cu²+ (aq) = Sn²+ (aq) + 2 Cu+ (aq) has a standard potential of 0.29 V at 25…

Q: How many seconds are required to deposit 0.239 grams of zinc metal from a solution that contains…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Sn…

A: The cell reaction taking place is given as, => Sn2+ (aq) + Ba (s) -------> Sn (s) + Ba2+ (aq)…

Q: Calculate the standard cell potential of the following cell at 25°C:

A: From electrochemical cells standard reduction potential (SRP) values of Pd and Cu electrodes are…

Q: Calculate the standard cell potential, standard free energy change, and equilibrium constant for the…

Q: What does a negative standard cell potential imply about the reaction?

A: The potential difference between the cathode and anode half cell under the standard conditions of…

Q: How long, in minutes, will it take to produce 370.0 g of pure lithium by running a current of 330 A…

A: Given, Current passing = 330 A Mass of Li = 370.0 g Molar mass of Li = 6.94 g/mol

Q: How many hours are required to plate 12.00 g of nickel metal from 1.00 M NİSO4(aq), using a current…

Q: Calculate the equilibrium constant K for the following reaction at 25°C from standard electrode…

A: As the question contains more than one question, only the first one is solved in this attempt. If…

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

Q: (b) Fe(s) | Fe²*(aq) || Ce³+ (aq), Ce**(aq) | Pt

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn²+…

Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

Q: The standard cell potential for the reaction at 298.15 K: Fe (s) + Zn2+ (aq) ⇋ Fe2+ (aq) + Zn (s)…

Q: A voltaic cell employs the following redox reaction: 2 Fe³+ (aq) +3 Mg (s) → 2 Fe (s) +3 Mg²+ (aq)…

A: Given- 2Fe+3 (aq) + 3 Mg (s) → 2Fe (s) + 3 Mg2+(aq) Oxidation half reaction = 3 Mg (s) →3…

Q: A. Calculate the standard potential of each of the following cell: Cu(s) + Pb2+(aq) → Cu2+(aq) +…

A: The Standard potential of the cell is having the formula, Ecell°=Ecathode°-Eanode° The Standard…

Q: At 298 K a cell reaction has a standard cell potential of +0.17 V. The equilibrium constant for the…

A: Given: T = Temperature in K = 298 K E = standard emf = 0.17 V K = equilibrium constant = 5.5 X 105…

Q: 3.2 calculate the standard cell potential of the following cell at 250 Sn(s)|Sn*(aq)||Cu*(aq)|Cu(s)…

Q: 11. Consider the following reaction and its AG-AGo at 25.00 °C. 2Ag(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG…

A: Given reaction is : 2Ag+ (aq) + Cu (s) ------------> 2Ag (s) + Cu2+ (aq) , ΔG0 = -88660 J/mole…

Q: A cell has a standard emf of+ 0.134 V at 298 K.

Q: 11. Consider the following reaction and its AG-AG• at 25.00 °C. 2Ag(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG…

A: For given reaction and given ∆G° value , E°cell and K can be calculated using relations with ∆G° .

Q: 3.2 calculate the standard cell potential of the following cell at 25C 2+…

A: Standard electrode potential of equations Cu2+ + 2e- ——> Cu(S) Eo = 0.34V Sn2+ + 2e- ——> Sn…

Q: A galvanic cell is made up of one electrode consisting of a copper metal immersed in 0.00500 M…

A: Given, A galvanic cell is made up of one electrode consisting of a copper metal immersed in 0.00500…

Q: Calculate the cell potential for the following reactions and predict whether the reaction will take…

A: Zn + 2 Ag+ (aq) ------> Zn2+ + 2Ag At anode ( oxidation) Zn -----> Zn+2 + 2 e- Eoxd =…

Q: Consider the reaction below: 2 Ag(aq) + +Fe(s) → 2 Ag(s) + Fe^2+(aq) ΔG° = −241.0kJmol a.…

Q: Consider the following reaction and its AG° at 25.00 ° 2 Ag*(aq) + Cu(s) → 2 Ag(s) + Cu²+(aq) AG° =…

A: Given that: temperature, T = 25 oC ∆G°= -88.66 kJ/mol To find: standard cell potential, Eocell?…

Q: How many grams of zinc metal will be deposited from a solution that contains Zn^2+ ions if a…

A: In this question, we will determine the mass of Zn metal which is deposited from the Solution in…

Q: At 298 K a cell reaction has a standard emf of +0.18 V. The equilibrium constant for the cell…

A: Since the relationship between equilibrium constant and cell emf is given by nFE = RTln(k) where n…

Q: Suppose a galvanic cell is established using the following cell reaction, Cu(s) + 2Ag+(0.100 M)…

A: Given the cell reaction is: Cu(s) + 2Ag+(aq) (0.100 M) <-----> Cu2+(aq) (0.200 M) + 2Ag(s)…

Q: Balance the following reactions. Calculate the cell potential and the Gibbs free ener these…

A: The question is based on concept of electrochemistry. we have been given a cell. We have to…

Q: A student does an experiment to determine the molar solubility of lead(II) iodide. She constructs a…

A: Write the reactions taking place at anode and cathode,

Q: Consider the following reaction and its AG° at 25.00 °C. 2 Ag*(aq)+Cu(s) → 2 Ag(s) + Cu2+(aq) AG° =…

A: ∆G = -88.66 KJ/mol = -88660 J/mol Temperature (T) = 25°C = 25+273 = 298 K R = 8.314 J/mol.K Keq =…

Q: Calculate the standard cell potential, and note whether the reaction is spontaneous under standard…

A: We have given that cell : Cu(s)│Cu2+(aq)║Au3+(aq)│Au(s) To know whether the reaction is…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu2* (aq)+…

A: The cell reaction taking place is given as, => 3 Cu2+ (aq) + 2 Al (s) -------> 3 Cu (s) + 2…

Q: Calculate the equilibrium constant, K for the reaction at 298 K,Zn (s) + Cu2+(aq) ——–> Zn2+(aq)…

A: Equilibrium constant may be defined as the ratio of the multiplication of the concentration of the…

Q: O21g) + 4H°(aq) + 2Zn¢ → 2H20µ + 2Zn²" ag) C.

Q: Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these…

A: For a.) Adding these 2 eqn we get,

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 AG° and the equilibrium constant for the following reaction at 298 K:
Zn*(aq) + Ni(s) → Zn(s) + Ni²*(aq)
Acidic Solution
Standard Electrode Potential, E (volts)
H2O2(aq) + 2 H'(aq) + 2 e
Au*(aq) + e- Au(s)
Au (aq) + 3 e- Au(s)
Br2(8) +2 e-→2 Br(aq)
NO: (aq) + 4 H'(aq) + 3 e NO(g) + 2 H20
Agʻ(aq) + e Ag(s)
Hg2"(aq) + 2 e
Fe (aq) + e-- Fe2"(aq)
Cu2*(aq) + 2 e Cu(s)
HgzClz(s) + 2 e →2 Hg(t) + 2 C(aq)
Sn(aq) + 2e Sn2 (aq)
2 H*(aq) + 2 e → Hz(g)
Pb2*(aq) + 2 e Pb(s)
Sn2"(aq) + 2 e Sn(s)
Ni (aq) + 2 e → Ni(s)
Cd2*(aq) + 2 e Cd(s)
Cr (aq) + e - Cr*(aq)
Fe2 (aq) + 2 e →Fe(s)
Zn2*(aq) + 2 e Zn(s)
Cr2*( aq) + 2 e Cr(s)
Al3 (aq) + 3 e →Al(s)
Mg2 (aq) + 2 e Mg(s)
2 H20({)
+1.77
+1.68
+1.50
+1.08
+0.96
+0.80
2 Hg(8)
+0.789
+0.77
+0.337
+0.27
+0.15 .
0.00
-0.126
-0.14
-0.25
-0.40
-0.408
-0.44
-0.763
-0.91
-1.66
-2.37
AG° =
J
K =

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 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 half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
Calculate the electrode potentials of the following half-cells. (a) Ag+(0.0436 M)|Ag (b) Fe3+ (5.34 10-4M),Fe2+ (0.090 M)|Pt (c) AgBr(sat’d),Br- (0.037 M)|Ag
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).

Recommended textbooks for you

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry