(16)(E)Nobelium-235Consider the following redox reaction that occurs in an electrochemical cell:Fe2+ (aq) + Al(s) → Fe (s) + Al³+ (aq)What is the standard Gibbs free energy (AG°) for this electron transfer?(A)-117 kJ(B)-700 kJ(C)-350 kJ(D)1222 kJ(E)-1222 kJ

16) Given, Fe2+(aq) + Al(s) ➝ Fe(s) + Al3+(aq) Standard gibbs free energy (∆G°) = ? Standard…

(16) Consider the following redox reaction that occurs in an electrochemical cell: Fe²+ (aq) + Al(s) → Fe (s) + Al³+ (aq) What is the standard Gibbs free energy (AG°) for this electron transfer? (A) -117 kJ (B) -700 kJ (C) -350 kJ (D) 1222 kJ (E) -1222 kJ

(16) Consider the following redox reaction that occurs in an electrochemical cell: Fe²+ (aq) + Al(s) → Fe (s) + Al³+ (aq) What is the standard Gibbs free energy (AG°) for this electron transfer? (A) -117 kJ (B) -700 kJ (C) -350 kJ (D) 1222 kJ (E) -1222 kJ

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 half-reactions: (1) The strongest oxidizing agent is: (2) The weakest…

A: Give half cell reaction and standard reduction potential of three species Hg , Co and Zn. We have…

Q: Indicate if each of the following statements is true of false. If false, rewrite it to make it a…

Q: A redox reaction has an equilibrium constant of K = 1.2 * 103. Which statement is true regarding…

A: lets suppose,

Q: Consider the following unbalanced redox reaction that occurs in an electrochemical cell: Fe (s) +…

A: Given, Fe (s) + Al3+ (aq) -->Fe2+ (aq) + Al (s) standard gibbs free energy (∆G°) = ? Note:…

Q: (1)Using the Table, rank the following species from the strongest to the weakest reducing agent:…

Q: Calculate ΔG˚, in kJ, for the following reaction at 25˚C. 3 Cu(s) 2 NO3-(aq) + 8 H+(aq) → 3…

Q: What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0170 2?(F =…

Q: Mg(s) + Pb²*(aq) → Mg²*(aq) + Pb(s) If the above galvanic cell starts at standard state conditions,…

A: Option D When reactants decrease and product concentration increases the reaction quotient…

Q: The nickel-cadmium rechargeable cell follows this overall reaction: Cds) + NiO2(s) + 2H2O + 2OH- ⇌…

A: The objective is to to compute the value of equilibrium constant, K of the reaction. Given…

Q: The free energy available from a 1.10-volt Cu(II)-Zn cell under standard conditions is -212 kJ…

A: Given that: Standard electrode potential of cell = 1.10 V To find: Standard Gibbs free energy =?

Q: In an electrochemical cell, Q = 0.0010 and K = 0.10. What can you conclude about Ecell and…

Q: A voltaic cell is to be designed at standard state conditions using the following two half-…

A: If the value of cell potential is positive; then the reaction is spontaneous. If the value of cell…

Q: (a) Calculate ΔrG0 for the reactionMg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s)Given : E0cell = + 2.71 V,…

A: The reaction is

Q: (a) Calculate ArG° for the reaction:Mg(s) + Cu22+(aq) > Mg2+(aq) + Cu(s)Given: E°cell = + 2.71 V,…

A: (a) The given reaction is, E◦ cell = 2.71 V Number of electrons transferred, n = 2 1 F = 96500…

Q: Calculate the free energy, ΔG°, (kJ/mol) for the galvanic cell performing the following reaction as…

A: The cell reaction given is V + Sr2+ → Sr + V2+ Temperature, T = 25 °C = (25 + 273.15) K = 298.15 K…

Q: A galvanic cell has the overall reaction: Zn(s) + 2Eu(NO3)3(aq) → Zn(NO3)2(aq) + 2Eu(NO3)2(aq) Which…

Q: Consider the following half-reactions: Half-reaction E° (V) C2(g) + 2e → 2C1'(aq) 1.360V cd2*(aq) +…

Q: Determine the Ecell for the given redox reaction. Assume that the reaction reached equilibrium at…

Q: Calculate the maximum work available (in kJ) from 52.3 g of aluminum in the following cell when the…

Q: The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.19 M and [Cr3+] =…

A: The cell reaction given is, => 3 Cu2+ (aq) + 2 Cr (s) ↔ 2 Cr3+ (aq) + 3 Cu (s) Given: [Cu2+ ] =…

Q: Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e → 2Br (aq)|1.080V 2H"(aq) +…

A: To solve this problem we will use the given reduction potential of each species .

Q: Calculate ΔG° for the electrochemical cell Pb(s) | Pb ⁺²(aq) || Fe ⁺³(aq) | Fe ⁺²(aq) | Pt(s) A)…

Q: Consider the following electrochemical cell:…

A: In electrochemical cell redox reaction occur

Q: (a) In the electrolysis of aqueous NaCO3, how many liters of O₂(g) (at STP) are generated by a…

A: It is given that for an electrolysis reaction:current = 53.9 Atime = 73.9 minconvert min to sec.We…

Q: (2) Using the standard reduction potentials listed in the Table, determine which of the following…

A: The answer is as follows:

Q: Consider the following half reactions: Na+(aq) + e- → Na(s) E○red= -2.71 v Zn2+(aq) +…

A: The species which have maximum standard reduction potential will have the potential to gain the…

Q: Consider a voltaic cell whose overall reaction isPb2+(aq) + Zn(s)---->Pb(s) + Zn2+(aq). What is…

A: At 298 K, the emf (ECell) generated by the cell is calculated as shown below in equation (1) where…

Q: What is the cell potential (in V) for the reaction below with the given concentrations at 33.0 oC?…

A: Given concentrations:[H+] = 0.152 M[NO3- ] = 0.470 M[Fe3+ ] = 0.885 M[NO] = 0.623 MFirst, let's…

Q: Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e → 2Br (aq)|1.080V Sn2*(aq) +…

A: Species with higher Ereduction value are the strongest oxidizing agent and weakest reducing agent.…

Q: The potential in an electrochemical cell, E, is related to the Gibb's free energy change (ΔG) for…

A: The objective of this question is to calculate the standard Gibbs free energy change (ΔG0) for the…

Q: The free energy change for the following reaction at 25 °C, when [Pb2+] = 1.17 M and [Ni2+] =…

A: The energy which are used in reaction to do work is known as Gibbs free energy.

Q: (2) Using the standard reduction potentials listed in the Table, determine which of the following…

A: The solution is as follows:

Q: E°cell = 1.66 V for the following cell reaction: P4(8) + 3OH´(aq) + 3H2O(1) → PH3(g) + 3H2PO2¯(aq)…

Q: Consider the following half-reactions: Half-reaction E° (V) Br,(1) + 2e → 2Br (aq) |1.080V Co2+…

Q: Calculate AG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C) MnO4…

A: MnO4-(aq) + 8H+(aq) + 5e- ---> Mn2+(aq) + 4H2O(l) ; E° = 1.51 V Fe3+(aq) + e- ---> Fe2+(aq)…

Q: Consider the following half-reactions: Half-reaction E° (V) 1(s) + 2e 21(aq) 0.535V Cd2*(aq) + 2e →…

A: Here to identify the oxidizing and reducing power, we will consider the reduction potential of each…

Q: Metallic iron can be made by the electrolysis of molten Fe2O3. (a) What mass of Fe is formed by…

Q: Half-reaction E° (V) I2(s) + 2e→ 21I(aq) 0.535V Pb"(aq) + 2e → Pb(s)|-0.126V Zn-(aq) + 2e →…

A: Since you have asked a question with multiple subparts, we will answer only first three subparts for…

Q: liters of Cl₂(g) is generated by this electrolysis. (b) How many moles of NaOH(aq) are formed in the…

Q: Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F°(aq) 2.870V 2+ Pb"(aq) +…

Q: Consider the following half-reactions: Half-reaction E° (V) Hg2+(aq) + 2e Cu2+(aq) + 2e™ Hg(1)…

A: Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

Q: Be sure to answer all parts. (a) Balance the skeleton reaction. Include the states of matter for…

Q: Consider the following half-reactions: Half-reaction E° (V) Ag"(aq) + e » Ag(s) 0.799V 2+ Co(s)…

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

Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag ℰ° = +0.80 V…

A: The cell's feasibility as well as potential are estimated using Nernst equation which derives the…

Q: Given the following data, answer the following questions: Fe2+(aq) + 2e- → Fe(s) E○red = -0.44 v,…

A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.

Q: Calculate ΔG° for the following balanced redox reaction and determine if the reaction is…

A: given reaction

Concept explainers

Batteries

A battery is simply an electrochemical cell or group of cells that generate electric current. Batteries are the devices that generate current using redox reactions. These reactions proceed by the transfer of electrons. An ideal battery or cell should produce a constant voltage. A battery should actually be light in weight.

Question

(16)
(E)
Nobelium-235
Consider the following redox reaction that occurs in an electrochemical cell:
Fe2+ (aq) + Al(s) → Fe (s) + Al³+ (aq)
What is the standard Gibbs free energy (AG°) for this electron transfer?
(A)
-117 kJ
(B)
-700 kJ
(C)
-350 kJ
(D)
1222 kJ
(E)
-1222 kJ

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

Trending now

This is a popular solution!

Step by step

Solved in 4 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 the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H*(aq) → Au³*(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);
Calculate AG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C) MnO4 (aq) + 8H*(aq) + 5e → Mn2+(aq) + 4H20(1) E° = 1.51 V Fe3+ (aq) + e → Fe2*(aq) E°= 0.77 V
Which statement is true regarding the galvanic cell in which an electric current is being produced? Zn²* + 2e¯→Zn E° = -0.76 V Cu2* + 2e¯→Cu E° = +0.34 V V Salt Bridge Zn - Cu ZnSO«(aq) CUSO:(aq) (A) Oxidation occurs at the copper electrode. (B) The mass of the copper electrode is increasing. (C) Zinc ions are produced at the copper electrode. (D) Copper ions are produced at the copper electrode.
Consider the following half-reactions: Half-reaction E° (V) 2+ Hg"(aq) + 2e → Hg(1) 0.855V Co**(aq) + 2e → Co(s) -0.280V 2+ Fe"(aq) + 2e → Fe(s) |-0.440v (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Hg*(aq) oxidize Fe(s) to Fe2*(aq)?| (6) Which species can be oxidized by Co2*(aq)? If none, leave box blank.
Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F*(aq) 2.870V Co2+*(aq) + 2e → Co(s) |-0.28OV 2+ Mg"(aq) + 2e → Mg(s) -2.37OV (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Mg(s) reduce F2(g) to F"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
Metallic nickel can be made by the electrolysis of molten NiCl₂. (a) What mass of Ni is formed by passing a current of 7.09 A through molten NiCl₂ for 4.70 days? The unbalanced chemical reaction representing this electrolysis is shown below. NiCl₂ → Ni + Cl₂ g of Ni is formed by this electrolysis. (b) How many minutes are needed to plate out 18.00 g of Ni from molten NiCl₂ using 6.93 A current? minutes are needed.
Consider the following galvanic cell: Cu(s) | Cu²+ (aq) || Ag+(aq) | Ag(s) Identify the cathode and state if it is being oxidized or reduced (please refer to chart on reference data page.) (A) Cu is the cathode; it is being oxidized (B) Cu is the cathode; it is being reduced (C) Ag is the cathode; it is being oxidized (D) Ag is the cathode; it is being reduced (E) Since the E values for both Ag and Cu are positive, they are both cathodes and being reduced
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e - Zn(s) :-0.763 V (red |Cro (aq)+4 H2O(1)+3e Cr(OH)3(s)+5OH (aq) :-0.13 V = - (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.
114. One type of breathalyzer employs a fuel cell to measure the quantity of alcohol in the breath. When a suspect blows into the breathalyzer, ethyl alcohol is oxidized to acetic acid at the anode: CH;CH,OH(g) + 4 OH (aq) - HC,H;O;(g) + 3 H2O(1) + 4 e ethyl alcohol acetic acid At the cathode, oxygen is reduced: 0,(g) + 2 H,O(1) + 4 e 4 OH (aq) The overall reaction is the oxidation of ethyl alcohol to acetic acid and water. When a suspected drunk driver blows 188 mL of his breath through this breathalyzer, the breathalyzer produces an average of 324 mA of current for 10 s. Assuming a pressure of 1.0 atm and a temperature of 25°C what percent (by volume) of the driver's breath is ethanol?
(a) A silver wire is placed in a solution of CuCl₂. Does this reaction occur under standard conditions? O The reaction occurs. No reaction occurs. (b) Cl2 gas is bubbled into a solution of Nal. Write a balanced net-ionic equation. (Use the lowest possible coefficients. Specify states such as (aq) or (s). If a box is not needed, leave it blank.) 21 (aq) +C1₂(g) Calculate E, AG, and K. E = 0.82 AG = -158.235 K =7.345x10^13 →2Cl(aq) + 1,(s) The reaction occurs. O No reaction occurs. V kj Does this reaction occur, under standard conditions?
What is the equilibrium constant K at 25 °C for an electrochemical cell when E° = +0.0235 V and n = 2?(F = 96,500 J/(V･mol), R = 8.314 J/(mol･K))
What is the balanced equation for the galvanic cell reaction expressed using the following shorthand notation? Mg (s) | Mg2+ (aq) || Cl2 (g) | Cl– (aq) | C (s)