Consider the electrochemical cell, Zn (s) | ZNBR2 (0.235 mol kg – 1) | Br2 (1) | C (s), for which the reaction is Br2 (I) + Zn (s) → 2 Br - (aq) + Zn 2+ (aq). Since Eo (Zn2 +, Zn) = -0.763 V, Eo (Br -, Br2) = +1.09 V a. Determine the standard potential, b. Determine the average ionic activity coefficient of ZnBr2 from the Debye-Hückel limit law. c. Determine the potential of the electrochemical cell for the given conditions at 298 K. d. ArG, ArGo, and K for the reaction, e. Given that (ƏE / ƏT) p = 8.45 x 10-5 V K – 1. Calculate AS and

Q: (c) Calculate the standard cell potential, E° of the following reaction at equilibrium. Show your…

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Q: Why is it necessary to use the standard hydrogen half-cell as a reference when calculating standard…

A: Given statement is :  Why is it necessary to use the standard hydrogen half-cell as a reference when…

Q: Calculate the cell voltage under these conditions around your hands to three significant digits…

A: The two half cell reactionsand their standard reduction potentials are given below.MnO 4 - (aq) + 8H…

Q: The following half-reactions were combined to construct a new galvanic cell. What is the standard…

A: Given-> [AuBr4]-(aq) + 3e- --------> Au(s) + 4Br-(aq).   E°=0.854 V Au3+(aq) + 3e- ------->…

Q: The standard potential of a Daniell cell, with cell reaction Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s), is…

A: The reaction:

Q: Consider the following reaction at 298K. 2Fe³+ (aq) + Fe(s) 2Fe2+ (aq) + Fe²+ (aq) The standard…

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Q: Calculate the standard free-energy change at 298K for the zinc-copper voltaic cell, which has a…

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Q: From the biological standard half-cell potentialsE⊕(O2,H+,H2O) = +0.82 V and E⊕(NADH+,H+,NADH) =…

A: E0cell- E0cell= E0cathode - E0anode Oxidation takes place at anode Reduction takes place at cathode…

Q: For the reaction 2Co+ (aq) + 2Cl (aq)→2C02+ (aq) + Cl2 (g). what is the cell potential at.25°C if…

A: Given that, a cell reaction is  2Co3+(aq) + 2Cl-(aq) →2Co2+(aq) + Cl2(g). The concentrations are…

Q: Under standard conditions, the ΔGo of the reactants for a given redox reaction is measured to be…

A: Since the relationship between the Eocell and the ΔGo is given by  ΔGocell = -nFEocell  where n =…

Q: Consider the following reaction at 298K. Hg2+ (aq) + Co(s)→→→ Hg(t) + Co²+ (aq) The standard Gibbs…

A: Given-> ∆G° = -219.06 KJ = -219.06 × 1000 J = -219060 J

Q: For a hydrogen/oxygen fuel cell, with an overall four-electron cell reaction 2 H2(g) + O2(g) → 2…

A: Gibb’s free energy- Where, ∆G0=change in standard Gibb’s free energy n= Number of electrons…

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

A: The reactions taking place at anode and cathode respectively are: At anode:  At anode:As → A+ aq M +…

Q: Given the schematic representation Cd | Cd2+ (1 M) || Ag+ (1 M) | Ag,  write the overall cell…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Q: Tabulated thermodynamic data can be used to predict the standard potential of a cell even if it…

A: Given: The balanced equation of the reaction is given as, Standard Gibbs energy of the reaction =…

Q: A. Calculate the standard free-energy change at 25 ∘C for the following reaction:…

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Q: Consider the cell, Zn(s)|ZnCl2(0.0050 mol kg−1)|Hg2Cl2(s)|Hg(l), for which the cell reaction is…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

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

A: The given reaction is

Q: During an electrolysis process a current of 3.20 amperes was used for a period of 2 hours and 49…

A: The charge deposited is given by, Q=It where I is the current and t is the time.

Q: Fe (s) + O2(g) + 2H2O (l) → Fe3+ + 4OH- Balance the  simple redox reaction, If the standard change…

A: Oxidation is the loss of electrons and reduction is the gain of electrons.

Q: Consider the following reaction at 298K. 2+ Hg (aq) + H2(g) Hg(f) + 2H*(aq) The standard Gibbs free…

A: Hg2+ (aq)  +  H2(g)   →  Hg(l)  + 2H+ (aq)Oxidation half cellH2(g)   →2 H+(aq)+ 2 e-Reduction half…

Q: For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483 V What is the cell potential at 25…

A: For the reaction   2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V   What is the cell potential at…

Q: One ecologically important equilibrium is that between carbonate and hydrogencarbonate (bicarbonate)…

A: The relation between free energy and cell potential is shown below: ∆G0 =-nFE0cell where; ∆G =…

Q: Consider the galvanic cell. In a certain experiment, the emf () of the cell is found to be Q.54 V at…

A: Solution :    Nernst equation is used to calculate the potential of the cell at non-standard…

Q: The standard cell potential of a Daniell cell, with cell reactionZn(s) + Cu2+(aq) → Zn2+(aq) +…

A: Given, a Daniell cell with the cell reaction as follows,Zn(s)+Cu2+→Zn2++Cu(s)the standard cell…

Q: Consider a hydrogen electrode in H Br(aq) at 25 °C operating at 145 bar. Estimate the change in the…

A: From the given data, it is known that for a SHE with PH2 value 145 bar in aqueous solution of HBr.…

Q: A fuel cell develops an electric potential from the chemical reaction between reagents supplied from…

A: (a) hydrogen and oxygen,

Q: Consider a galvanic cell that uses the reaction Zn(s) + 2H+(aq) →Zn2+(aq) + H2(g) Calculate the…

A: Concentrations [H+] = 1.0 M  [Zn2+] = 0.0010 M pH2 = 0.10 atm Cell reaction Zn(s) + 2H+(aq)…

Q: For the reaction; 4H+   +  PbO2  + 2 Fe 2+ →  2 Fe 3+ + Pb2+  +  2 H2O, the standard electrode…

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Q: A nonstandard cell is made by replacing the 1.0 M solutions of Cu(NO3)2 and Sn(NO3)2 in the standard…

A: Answer: 1. Let the standard electrode potential 1 M solution of Cu(NO3)2 and Sn(NO3)2 be E0 So,…

Q: Calculate the standard cell potential, ?∘cell,Ecell∘, for the equation…

A: Since the cell potentials for the half reactions are as Sn(s)  -----> Sn2+ (aq) + 2 e-…

Q: Consider a galvanic cell consisting of the Cr3+/Cr (Eo=-0.74 V) and the Ag+/Ag (Eo=+0.8 V) systems…

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

Q: 3. For the reaction: Zn(s) + 2Ag (aq)-Zn2(aq) 2Ag(s).. a. Determine the standard cell potential. b.…

A: Standard cell potential: E°cell =E°reduction -E°oxidation Where E°reduction = standard reduction…

Q: The cell whose diagram is Pb(s) I PbCl,(s) I KCI(aq) I Hg,Cl,(s) I Hg(1) Has a standard emf of…

A: Given :  E°cell = 0.5359 V  Temperature coefficient = 1.45 x 10-4 V/K  T = 298.15 K

Q: The redox potentials for the Zn2+/Zn and Cl2/Cl– couples are -0.764 V and 1.395 V, respectively.…

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Q: Consider the cell Pt|H,(g)| HCI(aq)|AgCl(s)|Ag, for which the cell reaction is 2 AgCl(s) + H,(g) → 2…

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Q: Using the electrochemical data found at the top of the Canvas page, calculate the equilibrium…

A: Given reaction is :  In (s) + Md3+ (aq) <----------> In+ (aq) + Md2+ (aq)  Calculate the value…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2103 (aq) +…

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Q: What mass of iron (III) sulfate is present in 100 cm3 of the solution used to measure the standard…

A: 39.9 g

Q: Calculate the cell potential and the equilibrium constant for the following reaction at 298 K:…

A: Cell potential can be calculated using formula :  E° = E° ( cathode ) - E° (anode )  So, we would…

Q: For the reaction: Zn(s) + 2Ag*(aq) → Zn*2(aq) 2Ag(s). a. Determine the standard cell potential. b.…

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Q: 6. For the cell Cd(Hg)|CdSO,. H,0(s)|Hg,SO,(s)|Hg the emf is given as a function of temperature t…

A: Given : E(V) = 1.01845 - (4.05x10-5)(t-20) -(9.5x10-7)(t-20)2  We have to calculate : ∆G , ∆H , ∆S

Q: Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g,…

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Q: Calculate the standard potential of the cell Ag(s)|AgNO3(aq)||Cu(NO3)2(aq)|Cu(s) and the standard…

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Q: Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker…

A: Interpretation - To write the half cell reaction that occurs at each electrode To check here which…

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

A: The oxidation number represents the number of electrons gain or loses by an element to become…

Q: By how much does the cell potential change when Q is increased by a factor of 5 for a reaction in…

A: Formula  Ecell = Ecello -0.05913logQ  E2-E1 = -0.05913 ( logQ2 -logQ1)              =  -0.05913 (…

Q: Consider the following reaction at 298K. Hg2+ (aq) + Ni(s)→→→→→ Hg(l) + Ni²+ (aq) The standard Gibbs…

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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.