Given the following standard reduction potentials: Fe³+ (aq) + e Fe²+(aq), E°= +0.77V - O₂(g)+ 4 H (aq) + 4e → 2 H₂O(1), Eº= +1.23V Fe²+ (aq) + 2e → Fe(s), Eº = -0.44 V Which of the following is a correct cell diagram of a galvanic cell under standard conditions? 1. Fe Fe²+||Fe³+|Fe²+|Pt II. FelFe²+||H₂O,H*|O₂|Pt Select one: a. I only Ob. Neither I nor II Oc. Il only Od. Both I and II

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: Consider the galvanic cell shown below (the contents of each half-cell are written beneath each…

A: This question can be solved via nernest equation. In the above question half cell reactions are…

Q: Calculate the standard cell potential for the reaction shown below .  Mn(s)+Ni^2+(aq) -> Mn^ 2+…

A: Voltic cell:  It is also called a Galvanic cell where chemical energy converted into electrical…

Q: Cr3+(aq)  +  3e- = Cr(s)                          -0.763 V Au+(aq)  +  e-  = Au(s)…

A: GIVEN:- Cr3+(aq)  +  3e- = Cr(s)                          -0.763 V Au+(aq)  +  e-  = Au(s)…

Q: A galvanic cell is constructed that carries out the reaction 2Ag(s) + Cl2 (g) → 2Ag+(aq) + 2CI- (ag)…

A:

Q: Given the following standard reduction potentials: Half reaction E° (V) Cr3*(aq) + 3e → Cr(s) -0.740…

A:

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

A:

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…

A:

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 is based on the following reaction(at 25°C)： Cu (aq)+Sn(s) → Cu(s)+Sn (aq) If the…

A: Note - The given reaction is incorrect. So, we will use the correct reaction for the question.   A…

Q: Consider the following standard reduction potentials:   Fe3+(aq) + e- → Fe2+( aq)…

A: Electrode reduction potential of all the species are there in a series which is known as…

Q: Calculate the Gibbs free energy, AG°, for a galvanic cell whose two half-reactions: Mt3+ (aq) +3…

A: Mt is getting reduced and R is getting oxidized in the above reaction. Electrode potential at…

Q: Consider the battery represented by the following notation. Ni(s) | Ni*"(aq) || Ag*(aq) | Ag(s)…

A:

Q: Consider the following standard reduction potentials: Fe3+ (aq) + e MnO4 (aq) + 8 H*(aq) + 5e → Mn2+…

A: In this question, we will see the strongest oxidizing agent.  You can see below.

Q: Using the following standard reduction potentials:         Fe3+(aq) + e- → Fe2+(aq)        E° =…

A:

Q: 2) Using the following reduction half-reactions and their respective standard reduction potentials…

A: The half reactions given are

Q: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: 8.15mA current flows which is equal to 0.00815A time is 12.6min = 756s The molar mass of I2 =…

Q: Half-Reaction Standard Reduction Potential, E (V) Ag* (aq) +e- -→ Ag(s) +0.80 Cu?+ (aq) + 2 e- →…

A: The correct option is explained below.

Q: What is the standard reduction potential for the galvanic cell described by the cell notation: Fe(s)…

A: A galvanic cell is composed of a cathode and anode. The cathode involves the reduction reaction,…

Q: Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.30 M), Cr³+ (2.0 M) || Co2+ (0.20 M) | Co…

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Q: Consider the following reaction and its AG AG° = -408.0 kJ/mol Mg(s) + Ni?+(aq) → Mg²+(aq) + Ni(s)…

A: Given-> Mg(s) + Ni2+(aq) ----> Mg2+(aq) + Ni(s)  ∆G° = -408.0 KJ/mole = -408000 J/mole (1 KJ =…

Q: In the following: Al³+ (aq) + 3 e Al(s) E° = -1.66 V Cr³+ (aq) + 3e →→ Cr(s) E° = -0.74 V What is…

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Q: Calculate E for the following electrochemical cell at 25 °C Pt(s) | H2(g, 1.00 atm)| H+(aq, 1.00 M)…

A: According to Nernst…

Q: The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn^2+(0.20 M)|| H+ (test solution)|…

A: Given, Cell potential = 0.475 V Temperature = 25°C =(25+273)K=298 K

Q: The cell notation for a galvanic cell is shown below. What is the oxidizing agent?…

A: The species undergoing an increase in oxidation state is oxidation or reducing agent whereas species…

Q: What is the overall reaction for the following cell line notation of a galvanic cell? Al(s)|AI3*(aq)…

A: Cell line notation of a galvanic cell :  Al(s)|Al3+(aq) || H+(aq)|H2(g)|Pt  Overall reaction for…

Q: Electrolysis of an aqueous solution of sodium chloride produces chlorine, . The reaction that occurs…

A: Give that: the reaction of anode is: 2Cl- (aq) →Cl2 (g) + 2e- Mass of Cl2 produced, w =182 g, time…

Q: What is the cell potential (E0) for a galvanic cell formed from the following two half-reactions?…

A:

Q: Given Pt² + (aq) + 2 e→→ Pt(s) Ag (aq)+eAg(s) 2 H*(aq) + 2 e -0.00 V Fe2+ (aq) + 2 e 8,-0.45 V If…

A: The standard electrode potential values of the some half cells are given above. Pt2+(aq) + 2e-…

Q: Given the cell reaction, Zn(s) + Cut2(a the cathode in the cell is: Cu(s) Cu +2 OPt (aq) Zn(s) +2…

A: The objective of the question is to calculate the standard cell potential, Eº, for the given…

Q: A chemist designs a galvanic cell from the following two half-reactions NO3(aq) + 4H+ (aq) + 3e →…

A: two half reactions and reduction potential of each is given

Q: Calculate the cell potential for the following reaction that takes place in an electrochemical cell…

A: Al(s)|Al3+(aq),( 0.115 M)||  Al+3(aq),(3.89 M)∣Al(s)

Q: Fe+ (ag) + Zn(s) Fe(s) + Zn?+(aq) E cell = +0.32 V A galvanic cell generates a cell potential of…

A:

Q: Calculate the standard cell potential for each of the following reaction:…

A: We have to Calculate the standard cell potential for Given  reaction:

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

A: We have to find standard electrode potential  Eocell = Eocathode - Eoanode

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.