2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g)      E∘=0.46 V2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g)      E∘=0.46 V   what is the cell potential at 25 ∘C∘C if the concentrations are [Co3+]=[Co3+]= 0.359 MM , [Co2+]=[Co2+]= 8.20×10−2 MM , and [Cl−]=[Cl−]= 0.789 MM and the pressur

Q: Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: 3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) What would be the pH of…

A: Given cell reaction: 3Co(s)+2NO3-(aq)+8H+→3Co+2(aq)+2NO(g)+4H2O(l)

Q: Use the tabulated electrode potentials to calculate ΔG° for the reaction:I2(s) + 2…

A: Oxidation half cell: 2Br- (aq) → Br2 (l) + 2e- Eₒ oxid. = -1.09V … (1) Reduction half cell: I2(s) +…

Q: What is the calculated value of the cell potential at 298 K for an electrochemical cell with the…

A: Given: The overall cell reaction will be as follows: 2H+(aq) + Zn(s)---------> H2(g) + Zn2+(aq).…

Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: Oxidation takes place at anode and reduction takes place at cathode. Loss of electrons is oxidation…

Q: two grams of copper (A.W. = 63.54g g/mol, density = 8.93g/cm^3) dissolves in 500g of water to…

A: Reaction: Cu→Cu2+ + 2e- Using Nernst equation: ECell=Ecell∘-0.05912logCu2+

Q: The standard cell potential for the following galvanic cell is 0.390 V.  What is the cell potential…

A: Given: Temperature = 325 K Eocell = 0.390 V Concentration of Sc+3 = 0.077 M Concentration of Ti+2 =…

Q: E Za a) ) Define the term standard electrode potential 2e 2 ZA Explain

A: Redox reactions are a kind of chemical reaction that involves oxidation and reduction. The element…

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

A: Given reaction: 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g)  E∘=0.483 V [Co3+]= 0.896 M [Co2+]= 0.548 M…

Q: Your mystery voltaic cell has a standard cell potential of 0.741 V and can be written in cell…

A: The importance of Gibbs energy is that it gives information about the spontaneity of the reaction or…

Q: Use the tabulated electrode potentials to calculate K for the oxidation of zinc by H+ (at 25 ∘C):…

A: The Nernst equation at 298 K is as follows,                                     E = Eo - 0.0592n…

Q: Calculate the standard potential, E°, for this reaction from its ΔG° value.…

A: The reaction given is  X (s) + Y4+ (aq) ------> X4+ (aq) + Y (s) In the above balanced reaction,…

Q: Manganese dioxide (MnO2) for use in dry cell batteries is made by electrolyzing solutions of Mn2*…

A:

Q: The standard reduction potential of Eu2+(aq) is -0.43 V.Using Appendix E, which of the following…

A: Concept introduction: Reduction potential indicates the ability of a substance to gain electron and…

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: A certain metal M forms a soluble nitrate salt M M(NO3)₂. Suppose the left half cell of a galvanic…

A:

Q: What is the potential of a cell at 25oC

A:

Q: For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483…

A: Given equation :             2Co3+(aq)+ 2Cl-(aq) → 2Co2+(aq)+ Cl2(g)                       Eο =…

Q: For a given equation: 2H2O(l) + Cr3+(aq) Mn2+(aq) → MnO2(s) + 4 H+(aq) + Cr (s) the reaction…

A:

Q: Consider the following galvanic cell:     E° (V) Sn4+  +  2 e−   →   Sn2+ 0.139 Ag+  +  e−   →…

A:

Q: Consider the reaction 2Co3+ (aq)+2CI-(aq)-2Co2+(aq)+Cl2(g) EOcell=0.71 V What is the cell potential…

A: Given data: E°cell = 0.71V  [Co3+] = 0.258V [CO2+] = 0.249V  [Cl-1] = 0.523V Pressure of Cl2 =…

Q: Calculate the standard potential, E°, for this reaction from its ΔG° value.…

A:

Q: Use the Nernst equation to calculate the cell potential, Ecell, for a galvanic cell consisting of…

A: Electrons flow from anode to cathode in a galvanic cell.  In order to prevent the build-up of…

Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: In this question, we want to determine the standard reduction potential of the cell.  You can see…

Q: Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of…

A: Given data: Concentration of solution = 0.4 M Emf of cell = 0.015 V Formula used:…

Q: Consider the following cell reaction: Ni(s) + 2 H+(? M) Ni2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: cell potential at 298 K is 0.125 volt

Q: For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483…

A: The given reaction is, 2Co3+(aq) + 2Cl-(aq) → 2Co2+(aq) + Cl2(g) The equilibrium constant of the…

Q: For the reaction 2Co 3+(aq)+2Cl -(aq)→2Co 2+(aq)+Cl 2(g)           E∘=0.483 V what is the cell…

A: P ( Cl2 ) = 4.10 atm  P V = n R T  P  = ( n/ V ) R T = c R T  c = P / R T  T ( temperature ) = 25…

Q: d.) Calculate the standard free energy change, AG cel, for the battery. F = 9.65 x 104 C/mol e.)…

A: Given :  Ag+(aq) + e- -----> Ag(s)  E° = 0.80 V  Cd+2(aq) + 2e- ------> Cd(s)  E° = -0.40 V…

Q: Given the reaction: Anode: NO3- + 2H + +e- ---> NO2 + H2O Cathode: 2H + 2e- ---> H2 Redox:…

A:

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

A:

Q: What is the potential (volts, V) of the spontaneous galvanic cell under the conditions outlined…

A:

Q: Gibbs energy change, A;G°, is related to cell potential, Eel, by the equation A;G° = -nFEl Part B…

A: The given reaction is as follows: Xs+2Y+(aq) → X2+(aq) + 2Y(s) ∆rG° of the reaction can be…

Q: Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of…

A: A cell made up of the same metal and same electrolyte with different concentrations are known as…

Q: The free energy change for the following reaction at 25 °C, when [Cd2+] = 3.67×10-3 M and [Ag+] =…

A: Answer:- This question is answered by using the simple concept of calculation cell potential using…

Q: Calculate the value of the EMF of galvanic cells and write the electrode reactions occurring in…

A: a)                    Zn/Zn2+(0.001)∥Cd2+(0.1)/Cd                         Anode : Zn = Zn2+ + 2e-…

Q: alculate the standard potential, ?∘, for this reaction from its Δ⁢G° value.…

A: Standard Reduction Potential - It is the difference between the reduction potential of cathode and…

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

A:

Q: The reduction half-reaction in your car lead-acid battery is the reduction of lead (IV) oxide (MW =…

A: Given:  Mass of PbO2 = 221 g             Current supplied = 138 A

Q: The cell shown below has a measured cell potential of +0.06839 V at 25.0 °C. A graph of the cell…

A:

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.887 M and…

A: Introduction :  We have to tell Ecell of the reaction . Given : [Cr2+] = 0.887 M [Ni2+] = 0.0150 M…

Q: Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of…

A: Nernst equation as follows,

Q: Consider the following reactions. Are they spontaneous in the direction written, under standard…

A: Cell with positive EMF represents negative free energy change with accompanies spontaneous change.

Q: How long (in hours) must a current of 5.0 amperes be maintained to electroplate 60g of calcium from…

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Q: 4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the…

A:

Q: Use the Nernst equation to Calculate the cell potential E for the Galvanic cell at 25ºC U=while…

A: The cell given is Al Ι Al3+(aq) ΙΙ Au3+(aq) Ι Au. Given: [Al3+ ] = 3.00 M [Au3+ ] = 5.00 × 10-5 M.…

Q: Consider these two entries from a fictional table of standard reduction potentials. X3++3e−⟶X(s)…

A:

Q: The Nernst Equation A nonstandard cell or half-cell potential can be calculated using the Nernst…

A:

Q: The oxidation of methanol, as described by the equation below, has a ΔG° value of -937.9 kJ/mol.…

A: Given Oxidation of Methanol 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l)∆Gcell° = -937.9 kJ/mol =…

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.