Using the following standard reduction potentials: Ag+ (aq) + e- ⇌ Ag (s) E o = +0.80 V Pb2+ (aq) + 2e - ⇌ Pb (s) Eo = -0.13 V i. Write a balanced redox reaction that represents the overall cell reaction for the feasible galvanic cell. ii. Calculate the standard cell potential. iii. Draw a fully labelled galvanic cell for this redox system. Your labels should show (but not limited to): the electron and ion flow; the anode and cathode, the half cells where oxidation and reduction take place. B. Describe the process involved in electroplating a silver coin.

Q: The standard cell potential for the reaction Cu 2+ (aq) + Fe 2+ (aq) + I - (aq) ⟶ CuI (s) + Fe 3+…

A: Nernst equation The equation that gives the relationship between cell potential and concentration of…

Q: Given the standard reduction potentials for an element A, at 25 °C: А2"(аg) + е > A (ag) E1° = 1.09…

A: Standard cell potential is an intensive property which does not depend on amount or mass of the…

Q: Consider the following pairs of reactions: Fe2+ (aq) + 2 e- → Fe (s) E° = – 0.44 V Au3+ (aq) + 3…

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

Q: calculate the standard cell potential for the galvanic cell reaction given below, and determine…

A: Standard EMF of the cell can be calculated using the formula: E°=E°(cathode) - E°(anode)…

Q: The following electrochemical cell is constructed at standard state: Mg(s) | Mg2+ || Cr2+ | Cr(s) a)…

A: Answers are explained below.

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

A: Use Nerenst  equation and standard  data E (cathode) =0.53 V E (Anode) =- 0.15 V

Q: A galvanic cell is constructed that uses the following half-cell reactions: Cu+(aq) + e−→ Cu(s)…

A: Find the complete solution given below

Q: (a) The cell potential for the following electrochemical cell at 25°C is 1.00 V. Pt(s) |H2 (g, x…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

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

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Q: Cr³*(aq) + 3 e¯ → Cr(s) E°red = -0.744 V Zn**(aq) + 2 e → Zn(s) E°red = -0.763 V Given that the…

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Q: A galvanic cell was prepared by immersing an anode and a cathode of the same material (of A type) in…

A:

Q: Consider the following reaction and its AG° at 25.00 °C. Fe2+ (aq)+Zn(s) → Fe(s) + Zn²*(aq) AG° =…

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

A: Standard cell potential, E0: The standard cell potential (E°cell) is the potential of the cell under…

Q: A galvanic cell consists of a lead anode immersed in a 1.00 M solution of Pb(NO3)2 and a platinum…

A:

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

A: Answer -

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

A:

Q: Given the following unbalanced½ reactions and their respective reduction cell potentials: Ni0,(s) →…

A: Given that, the unbalanced half-cell reaction and their respective reduction potential values:…

Q: Calculate the standard cell potential for this reaction. b. 2ClO2(g) + 1l-(aq) --> 2ClO2-(aq) +…

A: The given reaction; 2ClO2(g) + 2l-(aq) --> 2ClO2-(aq) + I2(s) Here ClO2 is getting reduced and I-…

Q: Given that the standard electrode potentials (E°) of metals are:K+/K = -2.93 V, Ag+/Ag = 0.80…

A: standard electrode potentials (E°) is inversely proportional to reducing power  Higher standard…

Q: The galvanic cell Zn(s) | Zn2+(aq) | | Ni2+(aq)| Ni(s) is constructed using a completely immersed…

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

Q: 11.)

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

Q: Use the Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of…

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: Pt|H; (1.6 atm)|H (0.80 M) || C,Hs O2 (0.20 M), AgC,HO2 (s)|Ag The cathode is essentially a silver…

A: The standard reduction potentials of half- cell reactions are, The most positive standard reduction…

Q: Consider the following galvanic cell at 25°C Pt|Br (aq) (0.25 M), H* (aq) (0.1 M) |Br2 () || O2 (g)…

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Q: Given: NO3 -> NO(g) ɛ° = 0.96 V %3D Sn4+ -> Sn2+ ɛ° = 0.13 V The two half cells were coupled to…

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

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

A:

Q: The galvanic cell consisting of a lead electrode and a zinc electrode was set up and connected by a…

A: We have been asked to provide short hand notation for the given electrochemical cell reaction and to…

Q: The above cell shows the standard half-cell potentials as follows: 4+ 3+ Pu*t + e → Pu' E° = 0.97V…

A:

Q: 2Sc(s) + Cr203 (aq) + 14H*(aq) → 2Sc3+ (aq) + 2Cr3+ (aq) + 7H20 (1) Cr20 (aq) + 14H* (aq) + 6e- →…

A:

Q: Half-Reaction Standard Reduction Potential, E° (V) Ag+ (ag) + e- → Ag(s) +0.80 Au+ (ag) + 3 e →…

A:

Q: Calculate the standard cell potential of the following cell at 25°C: Pb(s) | Pb?+ (ag) || Cu2+ (ag)…

A: In a galvanic cell, oxidation takes place in anode and reduction takes place in cathode. Non…

Q: The cell notation for the Galvanic cell is Cd(s)/Cd2+//I2(s)/I- The Standard…

A:

Q: What is the cell potential (E) for a galvanic cell formed from the following two half-reactions?…

A:

Q: Half-Reaction Standard Reduction Potential   ,      E°(V) Ag+(aq)+e−→Ag(s)…

A: Given that                                           E°(V) Ag+(aq)+e−→Ag(s)         +0.80…

Q: A galvanic cell with a measured standard cell potencial of 0.27 V is constructed using two beakers…

A: In the galvanic cell, the given reactions are: Cathode: Ni2+(aq)+ 2e-➡Ni(s) Anode:Ga(s)➡Ga3+ (aq) +…

Q: Three voltaic cells were constructed from solutions of CuSO4(aq), ZnSO4(aq), and Pb(NO3)2(aq) and…

A: According to the question, we have three voltaic cells constructed from solutions of CuSO4(aq),…

Q: Half-Reaction Standard Reduction Potential, E°(V) Ag+(aq)+e−→Ag(s) +0.80 Pb2+(aq)+2e−→Pb(s) −0.13…

A:

Q: Calculate the cell potential of a cell operating with the following reaction at 25°C in which [Cry…

A:

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+]=0.793 M and…

A: Recall Nernst equation to determine cell potential    E=Eo-0.059nlogProductReactantHere,Eo is…

Q: red +1.69 V Half-reaction Au^ + (aq) + e^ - Au (s) Fe^ 3+ (aq) + 3 e^ - Fe (s) -0.040 V Now ,…

A:

Q: Three voltaic cells can be constructed from solutions of Cusoa(aq), ZnSOa(aq), and Reaction E…

A:

Q: The above cell shows the standard half-cell potentials as follows: Pu*t + e 4+ Pu 3+ E° = 0.97V…

A: The EMF a full cell is given by the Nernst equation,which is mathematically- Ecell=E0cell - RTnF…

Q: Determine the cell potential for the following cell Zn(s) | Zn2+(aq), 0.500 M || Ag+(aq), 0.010 M |…

A:

Q: Given the following two half-reactions, write the overall reaction in the direction in which it is…

A: We have to write the overall reaction in the direction in which it is product-favored, and calculate…

Q: Use the Nernst equation to calculate the actual cell potential of a galvanic cell under the…

A: The reduction half cell reaction is, The oxidation half cell reaction is, Zn2+(aq) + 2e-⇌Zn(s)…

Q: Gibbs free energy= -434250 J/mol for a galvanic cell whose two half-reactions: Mt3+ (aq) + 3 e1- →…

A: The half reactions are  1) Mt3+ (aq) + 3 e- → Mt (s)                                Eo = 1.09 V 2)…

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.