Consider Zn+2 (0.056 M) | Zn || TI*3 (9.86 x 102M) I TI* (0.048 M) Pt E° (Zn*2/ Zn) = -0.763 V E° T*/T) = + 1.25 V Calculate E cell, AG (free energy) and kEq for this cell and explain whether is galvanic or electrolytic cell. ( do not forget to wite half reactions).

Q: 1)))) How many faradays must pass through an electrolytic cell to reduce 0.32 mol Ag+ ion to silver…

A:

Q: 31. Calculate AG° for the following galvanic cell: Mn(s) | Mn²"(aq) || Fe"(aq) [Fe(s), given these…

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Q: Calculate the electromotive force for the galvanic element composed of electrodes: Pt, H2 (1 atm) |…

A:

Q: Calculate the cell potential at 25°C for the cell             Fe(s) ∣ (Fe2+(0.100 M) ∣∣ Pd2+(1.0 ×…

A: The cell given is Fe(s) ∣ (Fe2+ (0.100 M) ∣∣ Pd2+ (1.0 X 10-5 M) ∣ Pd(s) Since the oxidation half is…

Q: 6) A galvanic cell is composed of these two half-cells, with the standard reduction potentials…

A: It is based on the concept of electrochemistry.  Here we are required to find the standard Gibbs…

Q: 15. Calculate AG° for the following galvanic cell: Mn(s) I Mn²*(aq) || Fe2+(aq) IFe(s), given these…

A:

Q: Given: Cr3+(aq) + 3e– ----> Cr(s); E° = –0.74 V Ag+(aq) + e–   --------> Ag(s); E° = 0.80 V What…

A: Answer:

Q: X(s)|X3+ (2.04 M) || Mn O4 1 minus (1.62 M)|Mn2+ (0.25 M)|H+ (2.64 M) The reduction potential for…

A: Given   The concentration of X3+ is 2.04 M. The concentration of MnO4- is 1.62 M. The concentration…

Q: 7) A galvanic cell is being made of iron & chromium. The standard reduction potentials are: Fe^2+…

A: Here we are required to find the standard cell potential of the given electrochemical reaction

Q: 5) Suppose a galvanic cell employs the following half-reactions: Ni²*(aq) + 2é Ni(s) Cr*(aq) + 3é >…

A:

Q: At 25 oC a zinc-copper battery is constructed as follows:  Zn|Zn2+(0.1000 M)||Cu2+(2.500 M)|Cu…

A: Using Nerst equation  Ecell  = Eocell - (0.0591/n ) log [ Zn2+ ]/[ Cu2+ ]

Q: Use the Nernst equation to calculate the cell potential for the following cell in Volts: Cr|Cr3+,…

A: The cell given is, => Cr (s) | Cr3+ (aq, 0.0010 M) || Cu2+ (aq, 1.0 M) | Cu (s)

Q: at 25 ° C, the galvanic element Pt | MnO4- 0.1M, Mn2 + 0.1M, pH = 1 || Ag + 0.0001M | Ag has the…

A: Welcome to bartleby !

Q: 7. Calculate AG° for the following galvanic cell Zn(s) | Zn²*(aq) || Fo2*(aq) IFe(s) given these…

A: The standard electrode potential of a Galvanic cell is given by the formula  E° = E°(cathode) -…

Q: The standard reduction potentials for Mg2+/Mg (E'= -2.37 V) and Fe2*/Fe (E'= -0.44 V). When a piece…

A: Concept- By the help of nernst equation, this problem can be solved. Ecell=Eocell− 0.0592/n log10Q…

Q: Given the following standard reduction potentials, Pb2+(aq) + 2 e → Pb(s) E° = -0.126 V PBSO4(s) + 2…

A: First the standard cell potential value is calculated from given reduction potentials.

Q: A cell is prepared by dipping a copper rod in 0.01 M CuSO4 solution and zinc rod in 0.02 M of ZnSO4…

A: Given :  E°Zn+2/Zn  = -0.76 V  E°Cu+2/Cu = 0.34 V  [CuSO4] = 0.01 M  [ZnSO4] = 0.02 M

Q: Cr3+(aq) + 3e– -> Cr(s); E° = –0.74 V Ag+(aq) + e– -> Ag(s); E° = 0.80 V What is the cell…

A: We will use nernest Equation

Q: Fe2+ (0.2 M) | Pt (s) A)  At 25 ºC, when the reaction quotient, Q, is equal to the equilibrium…

A:

Q: The cell notation for the Galvanic cell is              A(s)/A2+//B2(s)/B- The Standard Reduction…

A:

Q: Given the electrochemical reaction shown, what is the standard free energy change AG° if E° = +1.61…

A: ∆G° = - n F Eo n= The elctrons transfered from anode to cathode in the cell = 2. F = 96500 columbs.…

Q: X(s)|X5+ (0.94 M) || Mn O4 1 minus (1.10 M)|Mn O2(s)|H+ (0.51 M) The reduction potential for X5+ is…

A: The Nernst equation is shown below: Where: Ecell = cell potential E0cell = standard cell potential…

Q: A galvanic cell is made of a Ni*/Ni half cell with [Ni²-] = 1.00 × 103 M and a Ag:/Ag half cell with…

A: We can solve the problem by constructing the cell first. We can write the two half reactions to…

Q: The voltaic cell Ca(o)Ca²+ (aq) || Ni?+(1.0 M)|Ni(s) has a cell potential of 0.300 V at 25°C. What…

A: Given : Ecell = 0.300 V Temperature = 25 oC Concentration of Ni2+, [Ni2+ ] = 1.0 M And Eocell =…

Q: Calculate the potential measured for the following cell at 298 K. Cr(s) | Cr3*(aq) (0.0055 M) ||…

A: Given that: molarity of Cr/Cr3+ = 0.0055 M molarity of Ni/Ni2+ = 1.27 M Eocell = 0.50 V To find:…

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

A: Cell notation for the Galvanic cell is :-             Cd(s)/Cd2+//I2(s)/I-

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: Calculate the [Ni2+] in the following galvanic cell, given that the measured voltage of the cell is…

A:

Q: The free energy change for the following reaction at 25 °C, when [Fe²+] = 1.18 M and [Cr³+] =…

A: an electrochemical cell reaction is an example of redox process

Q: Calculate ECELL and indicate whether the cell is galvanic or electrolytic 8. Zn | 0.0364 M Zn+2 ||…

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: 1. Calculate E for the following electrochemical cell at 25 °C Pt(s) | H2(g, 1.00 atm)| H*(aq, 1.00…

A: Answer: This question will be solved using Nernst equation which is shown below:…

Q: Calculate the EMF of the following electrochemical cell: Pt | VO2+(0.25 M), V3+(0.10 M), H+ (0.001…

A: Answer:Here, n is the number of electrons transferred from anode to cathode and Q is reaction…

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

A: The given cell is, Therefore,

Q: Mn(k) | Mn²+(0.2 M) || H+ (pH= ?) | H2 (g, 1.5 atm) | The cell potential of the Pt(k) Cell was found…

A:

Q: for the following galvanic elements determine the electromotive force at 25 ° C Cu | Cu2 + 0.01M ||…

A: For the cell  Cu(s) | Cu2+aq. (0.01M) || Cu2+aq. (1.0M) | Cu(s) It is a concentration cell and it…

Q: 1) Calculate the following for the reaction at 298.0 K . The reaction is 2 SmCl3(aq) + 6 LiCl(aq) +…

A: As per instruction given in our Q&A guidelines I can answer first question only. This question…

Q: Consider the following cell: Ni(s)|Ni2+(aq, 0.100 M)||Cl–(aq, 0.200 M)|Cl2(g, 1.50 atm)|Pt If the…

A: Electromotive force is the potential difference generated between the two electrodes of the cell.…

Q: The free energy change for the following reaction at 25 °C, when [Cr**]= 2.80×10-3 M and [H*]= 1.11…

A: The formula of calculation of Gibbs free energy is: ∆G=-nFE (a) The chemical reaction taking place…

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.