Given:              Fe2+   +   2e-   -->   Fe                Eº = -0.44V Fe3+   +   3e-   -->   Fe                Eº = -0.04V Fe3+   +   e-   -->   Fe2+               Eº = +0.77V Cl2   +   2e-   -->   2Cl-                 Eº = +1.36V Calculate Eº cell of the reaction:                      Fe   +   Cl2   -->   Fe2+   +   2Cl- note: 2 decimal places

Q: Consider a voltaic cell constructed using the following two reductions: Fe+3 +3e- -->Fe…

A: When there if flow of electrons from one half cell to the another due to which some potential…

Q: Consider the galvanic cell based on the following half-reactions: Mn2+ + 2e –→ Mn €° = -1.18 V Fe?+…

A: Given, Reaction : Mn2++2e-→Mn           E°=-1.18 VFe2++2e-→ Fe           E°=-0.44 V

Q: below Ba2+ + 2e --- Ba(s) E° = - 2.91 v Mg2+ + 2e --- Mg(s) E° = -2.38 v Fe2+ ​​+ 2e --- Fe(s) E°…

A: Reduction occur at cathode and oxidation occur at anode. E°cell = E° reduction + E°Oxiation

Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

A: In order for a reaction to run spontaneously, E° cell must be positive, and for the same nickel must…

Q: A cell was prepared by creating the following cells: Anode: a Zr wire in a 1 M Zr4+ solution (Zr4+…

A:

Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

A:

Q: Calculate the equilibrium constant, Keq, for each electrochemical cell given the following…

A: The equilibrium constant Keq can be calculated from the change in Gibb's free energy (∆G0) of the…

Q: The following reaction proceeds spontaneously under standard conditions because E°cell > 0 (which…

A:

Q: 7. Calculate Ecell and AG for the following voltaic cell under non-standard conditions: [Cu²*] =…

A: We have to predict the Ecell and ∆G of the reaction.

Q: e7→ Sn E° = -0.14 v %3D e Cu E° = 0.34 v conditions, which species are prodi

A: In galvanic cell,  Oxidation takes place at anode and reduction takes place at cathode.  Reduction…

Q: Consider an electrochemical cell involving Iron and Copper.  Fe2+(aq) + 2e- → Fe(s)     Eo = -0.45…

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

Q: Consider the following reaction at 25 °C. (Ans.: 0.369 V) Cd*2 + 2e → Cd Zn* + 2e –→ Zn E° = -0.403…

A: Given:  E°(Cd+2|Cd) = -0.403 V And E°(Zn+2|Zn) = -0.763 V [Zn+2] = 0.05 M  [Cd+2] = 0.1M

Q: An AgO-Cd cell is used in satellite batteries. This cell is very compact, and it can supply much…

A: A question based on electrochemical cells that is to be accomplished.

Q: The following reaction is non-spontaneous as written when the components are in their standard…

A: Given: Co(s) + Fe2+(aq) ----> Co2+(aq) + Fe(s) Eocell = - 0.16 V

Q: 5. The following galvanic cell has a potential (E) of 0.98 V at 298 K. Zn(s) | ZnX,2* (0.010 M), X…

A: Given the potential of the cell, E = 0.98 V  T = 298 K  Here Zn(s) is oxidized to ZnX42+(aq) at the…

Q: Consider a galvanic cell built on the following half-reactions with their standard reduction…

A: The reactions are – Oxidation half cell-2Cr3+ + 7H2O ↔Cr2O7 +14H++ 6e-.....E∘red.=1.33 VReduction…

Q: Given the following half-cell reactions: Cr+3  +  3e-  ->  Cr           E° = -0.74 V Zn+2  +  2e-…

A: Given: Cr+3+3e-→Cr           Eo=-0.74 VZn+2+2e→Zn            Eo =-0.83 V To determine:…

Q: Payalben

A: The objective of this question is to calculate the cell potential of an electrochemical cell at 25…

Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

A:

Q: cell is constructed at 25 o C as follows. One half-cell consists of a chlorine/chloride, Cl 2 |Cl -…

A: First identify standard electrode potential and then use nernest equation  Total no of transfer…

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: The nickel–cadmium battery (NiCd battery or NiCad battery) is a type of rechargeable battery using…

A: The nickel–cadmium battery (NiCd battery or NiCad battery) is a type of rechargeable battery using…

Q: Fe (s) | FESO4(0.30 M) || KIO3(0.50 M), 12(s), pH 4.0 | Pt(s) Given: Fe2+ +2 e Fe (s) EO - 0.44 %3D…

A: Firstly half cell reactions are set. Reaction with highest value of reduction potential will undergo…

Q: At 298 K temperature, a voltaic cell produces a standard; E°cell = 0.718 V. Calculate the value of n…

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

Q: Calculate E' for the spontaneous reaction when an Ag*/Ag half-cell is joined to an Hg²*/Hg…

A:

Q: 4. Calculate at which Zn² concentration (x) the following electrochemical cell has an EMF of 0.9 V.…

A:

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.